Download MULTIPLY CHOICE QUESTIONS ON MEDICAL CHEMISTRY

DANYLO HALYTSKY LVIV NATIONAL MEDICAL UNIVERSITY
DEPARTMENT of GENERAL, BIOINORGANIC, PHYSICAL and
COLLOIDAL CHEMISTRY
V.V. Ogurtsov, O.V. Klenina, O.M. Roman
MULTIPLY CHOICE QUESTIONS
ON MEDICAL CHEMISTRY
(Module 2. The Equilibrium in Biological Systems Occuring on
the Interfaces)
For the 1st year students
оf medical faculty
L’VIV – 2012
Chapter 1. Energetics of Chemical Reactions and
Processes. Calculations According
Thermochemical Equations and Experimental
Determination of Heat Effects of Chemical
Processes. Bioenergetics
1.1. The mass of the substance (m) and
its volume (V) are:
А. extensive properties
B. thermodynamic properties
C. state functions of the system
D. thermodynamic potentials
E. intensive properties
1.2. Temperature (Т) and pressure (Р)
are:
А. kinetic properties
B. intensive properties
C. state functions of the system
D. extensive properties
E. thermodynamic potentials
1.3. The isothermal – isochoric
thermodynamic process is carried
out under:
А. T=const, V=const
B. P=const, T=const
C. P=const, U=const
D. T=const, U=const
E. V=const, Q=const
1.4. Thermochemistry is the study of:
А. transformations between
different kinds of matter
B. different kinds of energy
changing associated with
physical and chemical
processes
C. transformations of internal
energy into work under
chemical reactions
D. different kinds of energy
changing associated with
chemical reactions
E. transformations of heat into
internal energy under chemical
reactions
1.5. The isothermal – isobaric
thermodynamical process is
carried out under:
А. T=const, U=const
B. P=const, U=const
C. V=const, P=const
D. T=const, V=const
E. T=const, P=const
1.6. A system which can exchange
energy only with the surroundings
is called:
А. equilibrium
B. thermodynamic
C. closed
D. isolated
E. open
1.7. What is the kind of a system when
metal plate of zinc is dipped into
the test-tube with the sulfuric acid
H2SO4 solution?
А. chemical, heterogeneous, open
B. chemical, heterogeneous,
isolated
C. chemical, homogeneous, open
D. chemical, homogeneous,
isolated
E. physical, heterogeneous,
closed
1.8. What is the kind of a system when
calcium carbonate CaCO3 is
heated in a test-tube?
А. heterogeneous, nonequilibrium
B. heterogeneous, equilibrium
C. homogeneous, one-phase
D. heterogeneous, two-phases
E. heterogeneous, three-phases
1.9. Thermodynamic systems may be
divided into following types
according to the way of their
interaction with the surroundings:
А. physical and chemical
B. one-, two- and threecomponents
C. homogeneous and
heterogeneous
D. isolated, closed, open
E. equilibrium and nonequilibrium
1.10. Chemical thermodynamics is
based on:
А. two main laws of
thermodynamics
B. the main laws of physics and
chemistry
C. three main laws of
thermodynamics
D. different physical laws and
equations
E. one main laws of
thermodynamics
1.11. State functions are the parameters
of systems which depend on:
А. the path by which the process
occurs
B. the exchange by mass and
energy with the surroundings
C. the equilibrium constant value
D. the ability of a system to come
back to its initial state
E. the initial and final states of
the system
1.12. Heat and work depends on:
А. the initial and final states of
the system
B. the equilibrium constant value
C. the ability of a system to come
back to its initial state
D. the exchange by mass and
energy with the surroundings
E. the path by which the process
occurs
1.13. Does the ∆Н°298 value for a
chemical reaction depends on the
presence of a catalyst in a system?
А. depends in heterogeneous
systems
B. depends
C. depends of nature of a catalyst
D. doesn’t depend
E. depends in homogeneous
systems
1.14. The main law of thermochemistry
is:
А. law of mass action
B. Henry’s law
C. Hess’ law
D. Avogadro’ law
E. Nernst’ law
1.15. The standard enthalpy of
formation for which of the
following substances is equal to
zero?
А. O3
B. Н2О
C. О2
D. СО2
E. С6Н12О6
1.16. The standard enthalpy of
formation for which of the
following substances is equal to
zero?
А. H2O(g)
B.
C.
D.
E.
HF(liquid)
N2(solid)
HF(g)
N2 (g)
1.17. Which reactions through the listed
ones are exothermic?
1. N2 + O2 = 2NO
2. H2 + Cl2 = 2HCl
3. H2 + I2 = 2HI
А. 1, 2, 3
B. 3
C. 2
D. 1
E. 1, 3
1.18. Which reactions through the listed
ones are endothermic? 1. N2 + O2
= 2NO
2. H2 + Cl2 = 2HCl
3. H2 + S = H2S
А. 2
B. 1
C. 2, 3
D. 3
E. 1, 2, 3
1.19. Point out the correct consequence
of the thermal stability increasing
for hydrogen halogenides. The
standard enthalpies of formation
values for hydrogen halogenides
(in kJ/mol) are: ∆H°(HBr) = –
36,3; ∆H°(HI) = 26,6;
∆H°(HF) = −270,7; ∆H°(HCl) =
−92,3.
А. HI < HBr < HCl < HF
B. HF < HBr < HCl < HI
C. HF < HCl < HBr < HI
D. HBr < HCl < HF < HI
E. HI > HBr > HCl > HF
1.20. Which compound through the
listed ones can be more easily
decomposed under heating?
А. NO(g)
B. N2O3(g)
C. N2О(g)
D. all compounds are readily
decompose identically
E. NO2(g)
1.21. What will be the standard
enthalpy change for the reaction:
С(graphite) + 2 Н2(g) = СН4(g)?
А. it will decrease at 75 kJ
B. it will increase at 75 kJ
C. it will decrease at 51 kJ
D. it will decrease at 175 kJ
E. it will increase at 186 kJ
1.22. The mathematical equation for the
first law of thermodynamics is:
А. ∆U = Q + W
B. ∆U = Q – W
C. Q = – ∆Н
D. Q = ∆U + W
E. Q = ∆U – W
1.23. For which of the given substances
the standard enthalpy of formation
doesn’t equal to zero?
А. Р(white)
B. N2(g)
C. I2(solid)
D. С(graphite)
E. С(diamond)
1.24. 10.5 kJ of heat released when 11.2
L of H2S was formed. What is the
standard enthalpy of formation for
H2S?
А. 21.0 kJ/mol
B. –21.0 kJ/mol
C. 5.25 kJ/mol
D. 10.5 kJ/mol
E. –5.25 kJ/mol
1.25. Which reactions through the listed
ones are exothermic:
1. N2O4 = 2NO2
2. 1/2 N2 + 1/2 O2 = NO
3. H2 + 1/2 O2 =H2O
А. 1, 2, 3
B. no one through the listed
reactions
C. 1
D. 2
E. 3
1.26. For what kind of thermodynamic
processes the heat effect of the
reaction equals to the change of
the internal energy of the system:
Q= ∆U?
А. for isobaric processes
B. for equilibrium processes
C. for isothermal processes
D. for adiabatic processes
E. for isochoric processes
1.27. For what kind of thermodynamic
processes the heat effect of the
reaction equals to the change of
the enthalpy: Q = ∆H?
А. for adiabatic processes
B. for equilibrium processes
C. for isochoric processes
D. for isobaric processes
E. for isothermal processes
1.28. The heat effect for the process of
water transformation from liquid
to steam equals to:
А. -241.8 kJ/mol
B. 40 kJ/mol
C. - 44 kJ/mol
D. 4.4 kJ/mol
E. 44 kJ/mol
1.29. For which of the listed
compounds the standard
enthalpies of combustion
(∆Н°comb.) are equal to zero?
А. О2, Н2
B. СО, Н2
C. СО, NН3
D. NO, NH3
E. СО2, Н2О
1.30. In which of the given cases a
reaction is possible at any
temperatures?
А. no one
B. ∆H0 > 0 і ∆S0 < 0
C. |∆H0| = |T∆S0|
D. ∆H0 < 0 і ∆S0 > 0
E. ∆H0 > 0, T=0
1.31. Point out for which of the given
processes ∆S0 > 0.
А. 2CO(g) + O2(g) → 2CO2(g)
B. H2(g) + F2(g) → 2HF(g)
C. for none of the given reactions
D. 2H2S(g) + 3O2(g) →
2H2O(g) + 2SO2(g)
E. NH4NO2(solid) → 2H2O(g) +
N2(g)
1.32. Point out for which of the given
processes the entropy increases?
А. evaporation of alcohol
B. transformation of graphite into
diamond
C. ethylene polymerization
D. water freezing
E. association of ions
1.33. What is the standard entropy
change for the process of graphite
transformation into diamond?
SС(diamond)= 2,4 J/(mol•К)?
А. 5.7 J/(mol•К)
B. - 8.1 J/(mol•К)
C. 3.3 J/(mol•К)
D. 8.1 J/(mol•К)
E. -3.3 J/(mol•К)
1.34. The entropy of elements may be
equal to zero only under the
conditions of:
А. STP
B. P = const
C. normal conditions
D. T = const
E. the temperature of absolute
zero (T=0 °K)
1.35. Point out without any calculations
for which of the given processes
the entropy increases?
А. CH4(g) + Cl2(g) =
CH3Cl(liquid) + HCl(g)
B. CO(g) + Cl2(g) = COCl2(g)
C. 4 Al(solid) + 3 C(solid) =
Al4C3(solid)
D. 2 Fe(solid) + 3 Cl2(g) = 2
FeCl3(solid)
E. 2 NH3(g) = N2(g) + 3 H2(g)
1.36. The change of free Gibbs’ energy
may be calculated as:
А. ∆G = T∆S – ∆U
B. G = H + T∆S
C. F = U – TS
D. ∆G = T∆S – ∆H
E. ∆G = ∆H – T∆S
1.37. Free Gibbs’ energy is the measure
of:
А. the energy which can be used
for fulfilling a work
B. thermodynamic stability of the
system
C. dispersal energy
D. internal energy
E. non-reversible process
1.38. Point out without any calculations
for which of the given processes
the entropy increases?
А. С(graphite) + СО2(g) =
2СО(g)
B. 2SO2(g) + 2NO2(g) = 2SO2(g)
+ N2(g)
C. H2(g) + Сl2(g) = 2HCl(g)
D. 4 HСl(g) + О2(g) = 2Cl2(g) +
2 H2O(g)
E. 2СО(g) + О2(g) = 2СО(g)
1.39. A chemical reaction is impossible
at any temperature in the case of:
А. ∆H > 0, ∆S > 0, ∆G > 0
B. ∆H < 0, ∆S < 0, ∆G < 0
C. ∆H < 0, ∆S > 0, ∆G > 0
D. ∆H < 0, ∆S < 0, ∆G > 0
E. ∆H > 0, ∆S < 0, ∆G > 0
1.40. Is it possible to determine the
absolute value of the enthalpy and
free Gibbs’energy?
А. possibly to determine at STP
B. possibly to determine at
normal conditions
C. it is possibly to determine
experimentally
D. impossible
E. possible
1.41. Entropy is the measure of:
А. dispersal energy
B. reservation of energy of a
system
C. the energy which can be used
for fulfilling a work
D. heat capacity of the system
E. internal energy
1.42. Is the forward reaction
C(graphite) + CO2(g) = 2 CO(g)
possible? At what conditions?
А. possible at normal conditions
B. possible at STP
C. possible at steady pressure
D. impossible even at high
temperature
E. possible at high temperature
1.43. The decreasing of Gibbs’ free
energy shows that the forward
reaction is spontaneous at the
conditions of:
А. V = const, T = const
B. P = const
C. m = constant, heat capacity is
const
D. P = const, V = const
E. T = const, P = const
1.44. What substances are the final
products of metabolism of organic
compounds in the organism?
А. CO, NO, H2O
B. CO, H2O, SO3
C. CO2, NO, SO2
D. CO2, N2, H2O
E. CO2, NO2, SO3
1.45. What kind of system are
biological systems?
А. homogeneous open
B. homogeneous closed
C. heterogeneous nonequilibrium
D. homogeneous equilibrium
E. heterogeneous isolated
1.46. What kind of system are the living
organism cells?
А. isolated
B. open
C. equilibrium
D. closed
E. non-equilibrium
1.47. The main source of energy for the
human’s organism is:
А. ATP
B. fats
C. carbohydrates
D. proteins
E. vitamins and minerals
1.48. The daily ration of proteins for an
adult is:
А. 60–70 g
B. 50–80 g
C. 150-200 g
D. 75–85 g
E. 30–50 g
1.49. The daily ration of fats for an
adult is:
А. 70–80 g
B. 110–120 g
C. 30–50 g
D. 90-110 g
E. 60–70 g
1.50. The daily ration of carbohydrates
for an adult is:
А. 380–390 g
B. 250–280 g
C. 60–70 g
D. 90–100 g
E. 300–370 g
1.51. Energy which is accumulated in
the organism may be released
under the process of:
А. bio-polymers synthesis
B. ATP hydrolysis
C. foods metabolism
D. enzyme catalysis
E. photosynthesis
1.52. The molecules of what
compounds can act as energy
storage in bio-systems?
А. ATP
B. glucose
C. RNA
D. АDP
E. DNA
1.53. What kind of thermodynamic
system is the living organism?
А. opened system in the state of
thermodynamic equilibrium
B. opened system in stationary
state
C. closed system in in the
equilibrium state
D. isolated system in the
equilibrium state
E. closed system in stationary
state
1.54. Which one of the given equations
is the expression of the second
law of thermodynamics for
biological systems?
А. ∆Q = T ⋅ ∆S
B. S = Smax
C. ∆S > 0
∆τ
D. ∆S = ∆Q
T
E. ∆S = 0
Chapter 2. Kinetics of Chemical Reactions. Chemical
Equilibrium. Solubility Product Constant
2.1. The units of the rate of a chemical
reaction in homogeneous
systems?
А. mol⋅m2⋅min–1
B. mol⋅L–1⋅min.
C. mol⋅м3⋅s–1
D. mol⋅L–1⋅s–1
E. mol⋅mL–1⋅s–1
2.4. The expression of the Rate Law
for reaction 2NO (g)+O2(g) =
2NO2(g) is:
А. υ = k[NO] + [O2]
B. υ = k[NO]2·[O2]
C. υ = k[NO2]2·[O2]
D. υ = [2NO] 2 ·[O2]
E. υ = [NO]2 + [O2]
2.2. Сhose the reaction from the given
ones that has the highest rate:
А. 3H2 + N2 = 2NH3
t
B. MgCO3 
MgO + CO2
→
C. 2SO2 + O2 = 2SO3
D. H2 + I2 = 2HI
E. H2O + H+ = H3O+
2.5. The units of the rate of a chemical
reaction in heterogeneous
systems:
А. molּL/min
B. molּmLּs-1
C. mol/(cm3ּs)
D. kmolּм3ּmin-1
E. molּLּs-1
2.3. Сhose the reaction from the given
ones that has the highest rate:
А. 2NO + Cl2 = 2NOCl
Kt
B. C2H12O6 →
2C2H5OH +
2CO2
Kt
C. CO + 2H2 →
CH3OH
t
D. 2NH 
→ N +3H
3
2
2
E. NaOH + HCl = NaCl + H2O
2.6. The instantaneous rate may be
calculated according to equation:
А.
∆c
υ=
B.
∆τ
υ = kc 2
c2 − c1
τ 2 − τ1
D.
dc
υ =±
dτ
E.
∆c
υ =−
∆τ
C.
E. III
υ=
2.10. Сhose the reaction from the given
ones that has the highest rate:
Kt
А. 2C2H5OH →
(C2H5)2O +
H2O
t
B. 2NH 
→
N + 3H
3
2.8. Chose the reaction that take place
with the highest rate, if for the
same interval of time 1,0 grams
of products were forms?
А. 1 2 H2(g) + 1 2 Br2(g) = HBr(g)
B. 1 2 H2(g) + 1 2 Cl2(g) = HCl(g)
1
2 I2(г) = HI(г)
D. rate is the same
E. 1 2 H2(g) + 1 2 F2(g) = HF(g)
2.9. Chose the reaction that take place
with the highest rate, if for the
same interval of time 3,0 grams
of products were forms?
I.
1
2
H2(g) +
II. H2(g) +
1
2
1
2
2
+
2.7. The expression of the Rate law for
reaction 2SO2(g) + O2(g) = 2SO3(g)
is:
А. υ = k[SO2]2 [O2]
B. υ = k[SO3]
C. υ = [SО2] [O2]
D. υ = k[SO2] + [O2]
E. υ = [SO2] [O2]2
C. 1/2H2(г) +
2
C. (C6H10O5)n + nH2O
Cl2(g) = HCl(g)
O2(g) = H2O(g)
III. 1 2 H2(g) + 1 2 F2(g) = HF(g)
А. I
B. II
C. rate is the same
D. -
,t
H

→ nC6H12O6
D. 2SO2+ O2 = 2SO3
E. Ва(OH)2 + 2HCl = ВаCl2 +
2H2O
2.11. The expression of the Rate Law
for reaction 2CO(g) + O2(g) =
2CO2(g) is:
А. υ = k[CO]2⋅[O2]
B. υ = [CO]2⋅[O2]
C. υ = [CО]⋅ [O2]
D. υ = k[CO2]2
E. υ= k[2CO] [O2]
2.12. The rate increases in a
heterogeneous systems with:
А. irradiation
B. cooling
C. increasing surface area
D. all methods
E. decreasing of concentration of
reactant
2.13. The expression of the Rate Law
for reaction С(gr) + СО2(g) = 2СО(g)
is:
А. υ = k [СO2]
B. υ = k[С]
C. υ = k[СО2]
D. υ = k [С] [СO2]
E. υ = k[С] [СO]
2.14. The expression of the Rate Law
for reaction Н2О(g) + СО(g) =
СО2(g) +Н2(g) is:
А. υ = k[Н2О ] [СO]
B. υ = [Н2О ] [СO]
C. υ = k [СO]
D. υ = k [Н2 ] [СO2]
E. υ = k ([Н2О ] + [СO])
2.15. The expression of the Rate Law
for reaction N2(g) + 3Н2(g) =
2NH3(g) is:
А. υ = k[NH3 ]2
B. υ = k[N2 ]+ [H2]3
C. υ = [N2 ] [H2]3
D. υ = 2[N2 ] 3[H2]
E. υ = k[N2 ] [H2]3
2.16. How to name the main law of the
chemical kinetics?
А. B. Ostwald’s law
C. Henry’s law
D. The law of equivalents
E. Rate law
2.17. How will change the rate of
homogeneous reaction
2NO + O2 = 2NO2, if the initial
concentration increase in two
times?
А. increase in 16 times
B. increase in 12 times
C. increase in 4 times
D. increase in 2 times
E. increase in 8 times
2.18. How will change the rate of
reaction 2Fe(s) + 3Cl2(g) = 2FeCl3(s),
if the preassure decrease in 3
times?
А. decrease in 9 times
B. does not change
C. increase in 9 times
D. decrease in 27 times
E. decrease in 27 times
2.19. The rate of the reaction 2NO + O2
→ 2NO2 increases in 1000 times if
the pressure increase in:
А. 20 times
B. 100 times
C. 10 times
D. 5 times
E. 50 times
2.20. The rate of chemical reactions for
a 10ºC rise in temperature
increase in:
А. 2 times
B. 2 – 3 times
C. 2 – 4 times
D. 4 times
E. 3 times
2.21. How will change the rate of
reaction 2NO + O2 = 2NO2, if the
volume of systhem decrease in
two times?
А. decrease in 4 times
B. increase in 8 times
C. decrease in 16 times
D. increase in 16times
E. increase in 4 times
2.22. The rate of reaction 2СО(g) =
СО2(g) + С(g) increase in 9 times
when the concentration of
carbon(II) oxide increase in:
А. increase in 6 times
B. increase in 3 times
C. increase in 5 times
D. increase in 2 times
E. increase in 4 times
2.23. The rate of formation of NO2 in
the reaction 2NO + O2 → 2NO2
increase in 125 times, when the
pressure increase in:
А. increase in 50 times
B. increase in 10 times
C. increase in 5 times
D. increase in 15 times
E. increase in 25 times
2.24. How will change the rate of
reaction 2CO(g) + O2(g) = 2CO2(g),
if the initial concentration increase
in three times?
А. increase in 3 times
B. increase in 6 times
C. does not change
D. increase in 27 times
E. increase in 9 times
2.25. According to the reaction
СаСО3(s) → СаО(s) + СО2(g)
correct expression of the rate law
is:
А. υ = k[СаО ][СO2]
B. υ = k[СаО] + [СO2]
C. υ = [СаСО3 ]
D. υ = k[СаСО3 ]
E. υ = k
2.26. How will change the rate of
reaction 2NO + Cl2 = 2NOCl, if
the pressure of systhem increase
in four times?
А. does not change
B. increase in 16 times
C. decrease in 64 times
D. decrease in 16 times
E. increase in 64 times
2.27. The rate of the reaction 2Al(s) +
3Cl2(g) = 2AlCl3(s), increases in 64
times when the concentration of
Cl2 increase in:
А. 2 times
B. 4 times
C. 10 times
D. 6 times
E. 8 times
2.28. How will change the rate of
reaction 2Fe(s) + 3Cl2(g) =
2FeCl3(s), if the pressure of
systhem increase in three times?
А. increase in 9 times
B. increase in 3 times
C. decrease in 27 times
D. decrease in 9 times
E. increase in 27 times
2.29. Initial concentration of HCl in the
reaction NH3 + HCl = NH4Cl is
0.25 mol/L, in 0.2s it changes into
0.25 mol/L. What is the average
rate of this reaction?
А. 0,1 mol/ Lּs
B. 0,2 mol/ Lּs
C. 2 mol/ Lּs
D. 0,02 mol/ Lּs
E. 0,04 mol/ Lּs
2.30. How will change the rate of
reaction 3H2 + N2 ⇆ 2NH3, if the
volume of systhem decrease in
two times?
А. increase in 16 times
B. increase in 8 times
C. increase in 8 times
D. increase in 4 times
E. increase in 12 times
2.31. How will change the rate of
reaction 2NO + O2 = 2NO2, if the
initial concentrations of systhem
increase in two times?
А. increase in 16 times
B. increase in 8 times
C. increase in 2 times
D. increase in 3 times
E. increase in 4 times
2.32. Decomposition of HI (hydrogen
iodide) on the surface of gold is
the reaction of:
А. second order
B. higher order
C. first order
D. zero order
E.
D. monomolecular reaction of the
first order
E. heterogeneous, second order
2.33. Decomposition of NH3 on the
surface of tungsten (W) is the
reaction of: 2NH3
+3H2
А. higher order
B. C. zero order
D. first order
E. second order
t

→N
2
2.34. The given reaction of hydrolysis
С12Н22О11 + Н2О = С6Н12О6 (gl) +
С6Н12О6(fr) is:
А. monomolecular reaction of the
second order
B. bimolecular reaction of the
second order
C. bimolecular reaction of the
zero order
D. monomolecular reaction of the
first order
E. bimolecular reaction of the
first order
2.35. The reaction CO + Cl2 = COCl2 is
a reaction:
А. monomolecular reaction of the
second order
B. bimolecular reaction of the
first order
C. bimolecular reaction of the
second order
D. monomolecular reaction of the
zero order
E. monomolecular reaction of the
first order
2.36. The reaction CuO(s) + H2(g) = Cu(s)
+ H2O(l) is a reaction:
А. bimolecular reaction of the
first order реакція
B. homogeneous, second order
C. bimolecular reaction of the
second order
2.37. When the value of rate constant
and rate of reaction are equal?
А. concentrations of reactants are
the same, but not equal 1
mol/L
B. reaction take place in
homogeneous system
C. in all cases
D. concentrations of reactants are
equal 1 mol/L
E. reaction take place in
homogeneous system
2.38. When the order and the
molecularity are congruent?
А. always are congruent
B. for photochemical reaction
C. for complicated reaction
D. only for simple, one stage
reaction
E.
2.39. The range of the activation energy
Ea in the most of chemical
reactions:
А. 100-200 kJ/mol
B. 150-300 kJ/mol
C. 50-150 kJ/mol
D. 40-200 kJ/mol
E. 100-300 kJ/mol
2.40. Which of the given reactions take
place by the molecular mechanism
А. Ba2+ + SO42– = BaSO4
B. 2NO + O2 = 2NO2
C. H3O+ + OH– = 2H2O
D. H2 + Cl2 = 2HCl
E. 2H2 + O2 = 2H2O
2.41. Which of the given reactions take
place by the radical mechanisms?
А. HNO3 + KOH = KNO3 + H2O
B. H2 + I2 = 2HI
C. CH4 + Cl2 = CH3Cl + HCl
D. 2NO + O2 = 2NO2
E. AgNO3 + HCl = AgCl↓ +
HNO3
2.42. If the activation energy of the
chemical reaction is Еа > 120
kJ/mol, its rate is:
А. very low
B. very high
C. high
D. low
E. average
2.43. If the activation energy of the
chemical reaction is Еа ≈ 40
kJ/mol, its rate is:
А. high
B. average
C. very low
D. low
E. very high
2.44. The solubility of a slightly
dissolved salt AmBn, which
dissociate according to the scheme
n+
m–
AmBn →
← mA + nB may be
calculated as:
А.
Ksp
S= (m+n) m n
m ⋅n
B.
K
S=
C.
sp
m+n
S= (m⋅n)
D.
S= (m+n)
Ksp
m⋅n
Kp
m+n
E. S = K
sp
2.45. What is the relations between
Gibbs energy and the solubility
product constant Ksp?
А. log Ksp =–∆G/(2,303RT)
B. ∆G = - RTln Ksp
C. ∆G = RTln Ksp
D. ∆G = RTlog Ksp
E. log Ksp =∆G/(2,303RT)
2.46. In which case the solution of
BaSO4 is over-saturated?
А. [Ba2+]⋅[SO42–] ≈ Ksp
B. [Ba2+]⋅[SO42–] < Ksp
C. [Ba] ⋅[SO4]= Ksp
D. [Ba2+]⋅[SO42–] = Ksp
E. [Ba2+]⋅[SO42–] > Ksp
2.47. In which case the solution of AgI
is saturated?
А. [Ag+]+[I–] < Ksp
B. [Ag+]⋅[I–]≈ Ksp
C. [Ag+]⋅[I–] = Ksp
D. [Ag+]⋅[I–] > Ksp
E. [Ag+]⋅[I–] < Ksp
2.48. In which case the precipitate of
slightly dissolved salt will
form?(IP – ion product)
А. ІP = Ksp
B. ІP> Ksp
C. ІP< Ksp
D. E. ІP ≈ Ksp
2.49. Solubility product constant Ksp
depends on:
А. presence of catalyst
B. concentration of salt
C. molar concentration of ions
D. temperature
E. 2.50. The solubility product constant
Ksp of a slightly dissolved salt
AmBn, which dissociate according
n+
to the scheme AmBn →
← mA +
nBm– may be calculated as:
) (
m
⋅
aВ
An+
+
n
C. Ksp =
(
аА
sp
-
Bm
-
А. Ksp = [An+]⋅[Bm–]
B. K = a
⋅ a
)
D. Ksp = [A] ⋅[В]n
E. Ksp = [An+]m⋅[Bm–]n
m
H
2.55. Choose the pair of compound,
which ions can not be present
aO
2.54. Which ions can not be present
simultaneous (одночасно) in a
solution?
А. Fe2+, OH–
B. K+, NO3–
C. NH4+, Cl–
D. Cu2+, SO42–
E. Na+, SO42–
g
2.53. Compare the values for Ksp next
salts HgS, PbS, CdS, SnS, TlS2
and choose one, which is the least
soluble in a water.
А. Ksp (PbS) = 2.5·10–27
B. Ksp (HgS) = 4.0·10–53
C. Ksp (TlS2) = 5·10–21
D. Ksp (SnS) = 1.0·10–27
E. Ksp (CdS) = 1.2·10–28
+
2
2.52. The expression of the solubility
product constant Ksp for Ca3
(PO4)2 is:
А. Ksp = [Ca2+]3 + [PO43–]2
B. Ksp = 3[Ca2+]3+2[PO43–]2
C. Ksp = 3[Ca2+]3·2[PO43–]2
D. Ksp = ([Ca2+]3·[PO43–]2)/
[Ca3(PO4)2]
E. Ksp = [Ca2+]3·[PO43–]2
2.56. The expression of the solubility
product constant Ksp for
Mg(OH)2:
А. Ksp = [Mg2+]⋅[OH–]
B. Ksp = [Mg2+] 2[OH–]
C. Ksp = [Mg2+]⋅[OH–]2
D. Ksp = 2[Mg2+] 2[OH–]
E. Ksp
⋅ _
aM
=
2.51. The solubility of a slightly
dissolved salt is expressed by the:
А. coefficient of absorption
B. coefficient of solubility
C. solubility product constant
D. dissociation constant
E. percent of solubility
simultaneous in a solution:
А. AgNO3 and HCl
B. CuSO4 and BaCl2
C. Ba(OH)2 and CO2
D. NaOH and P2O5
E. Al(NO3)3 and HCl
2.57. The expression of the solubility
product constant Ksp for CaF2:
А. Ksp = [Ca2+][2F–]
B. Ksp = [Ca2+][F–]2
C. Ksp = [Ca2+] / [F–]2
D. Ksp = a(Ca2+) a(F–)
E. Ksp = [Ca2+] + [F–]
2.58. The expression of the solubility
product constant Ksp for Ag2CrO4:
А. Ksp = [Ag+]2⋅[CrO42–]
B. K = a 2 ⋅ a
sp
( )
Аg+
CrO42-
C. Ksp = [Ag+]⋅[CrO42–]
D. Ksp = 2[Ag+] [CO42–]
E. Ksp = [Ag+]+[Cr2O42–]
2.59. The solubility of Ag2S (in mol/L)
may be calculated according to
the equation:
А.
Ksp
S=
2
B. S= K
sp
C.
S= 3
Ksp
4
D.
S= 3
Ksp
constant for the reaction 2SO2 +
27
O2 ⇄ 2SO3 is:
А.
[SO3 ]
E. S= 3 4K
sp
2.60. The solubility of Fe(OH)3 (in
mol/L) may be calculated
according to the equation:
А.
Ksp
S= 3
4
B.
Ksp
S= 3
27
C.
Ksp
S= 4
27
D. S= 3 4K
sp
E. S= K
sp
2.61. Solubility of AgCl is equal
1.34⋅10–5 at the temperature 25
°С. Calculate the Ksp
А. 3.6 10–4
B. 5.2 10–5
C. 1.2 10–8
D. 8.8 10–10
E. 1.8 10–10
2.62. Solubility of СuS is equal 2,44
⋅10–18 at the temperature 25 °С.
Calculate the Ksp
А. 1.2 10–32
B. 1.2 10–18
C. 5.4 10–32
D. 6.0 10–36
E. 8.2 10–30
2.63. Expression of the equilibrium
Kp =
B.
C.
D.
E.
[SO 2 ] ⋅ [O 2 ]
Kp =
[SO3 ]2 ⋅ [O 2 ]
[SO 2 ]2
Kp =
[SO 2 ]2 ⋅ [O 2 ]
[SO3 ]2
Kp =
[SO 2 ]2
[SO3 ]2 ⋅ [O 2 ]
Kp =
[SO3 ]2
[SO 2 ]2 ⋅ [O 2 ]
2.64. Expression of the equilibrium
constant for the reaction FeO(s) +
H2(g) ⇄ Fe(s) + H2O(g) ?
А.
[FeO] ⋅ [H 2 ]
Kp =
[Fe] ⋅ [H 2 O]
B.
[H О]
Kp = 2
[H 2 ]
C.
Kp =
D.
Kp =
[H 2 ]
[H 2 O]
[H 2 O]
[H 2 ] ⋅ [FeO]
E.
[H O] ⋅ [Fe]
Kp = 2
[H 2 ] ⋅ [FeO]
Chapter 3. Measuring the Electromotive Forces of Galvanic
Cells and Electrode Potentials
3.1. In a hydrogen electrode the metal
conductor is:
А. silver
B. gold
C. hydrogen
D. iron
E. platinum
3.2. What is the value of рН of
standard hydrogen electrode?
А. 2
B. 10
C. 0
D. 1
E. 0,5
3.3. A silver chloride electrode
corresponds to:
А. II kind
B. oxidation-reduction
C. I kind
D. gaseous
E. ion-selective
3.4. A calomel electrode corresponds
to:
А. II kind
B. oxidation-reduction
C. I kind
D. ion-selective
E. gaseous
3.5. A hydrogen electrode corresponds
to:
А. I kind
B. ion-selective
C. gaseous
D. oxidation-reduction
E. II kind
3.6. A quinone-hydroquinone
electrode corresponds to:
А. oxidation-reduction
B. I kind
C. gaseous
D. second kind
E. ion-selective
3.7. A glass electrode corresponds to:
А. ion-selective
B. II kind
C. gaseous
D. I kind
E. oxidation-reduction
3.8. The electrode that is represented
schematically as Au3+| Au
corresponds to:
А. I kind
B. III kind
C. ion-selective
D. II kind
E. oxidation-reduction
3.9. The electrode that is represented
schematically as KCl,AgCl| Ag
corresponds to:
А. I kind
B. III kind
C. II kind
D. ion-selective
E. oxidation-reduction
3.10. The electrode that is represented
schematically as KCl ,Hg2Cl2 Hg
corresponds to:
А. I kind
B. III kind
C. ion-selective
D. II kind
E. oxidation-reduction
3.11. The electrode that is represented
schematically as Al3+| Al
corresponds to:
А. oxidation-reduction
B. II kind
C. ion-selective
D. III kind
E. I kind
3.12. The electrode that is represented
schematically as Au|Sn4+, Sn2+
corresponds to:
А. gaseous
B. indicators
C. reference
D. oxidation-reduction
E. ion-selective
3.13. The electrode that is represented
schematically as C|Sn4+ ,Sn2+
corresponds to:
А. indicators
B. reference
C. gaseous
D. oxidation-reduction
E. ion-selective
3.14. A copper plate is immersed in a
0.1M solution of CuSO4. What is
the charge of the electrode?
А. positive
B. negative
C. –
D. –
E. neutral
3.15. A copper plate is immersed in a
1M solution of CuCl2. What is the
charge of the electrode?
А. –
B. positive
C. negative
D. neutral
E. –
3.16. An aluminium plate is immersed
in a 0.1M solution of aluminium
sulfate. What is the charge of the
electrode?
А. –
B. neutral
C. positive
D. –
E. negative
3.17. An aluminium plate is immersed
in a 1M solution of aluminium
sulfate. What is the charge of the
electrode?
А. –
B. positive
C. negative
D. –
E. neutral
3.18. Which of the given electrodes:
magnesium, zinc, aluminium,
copper and gold has the highest
negative charge?
А. zinc
B. copper
C. gold
D. magnesium
E. aluminium
3.19. Which of the electrodes:
magnesium, zinc, aluminium,
copper and gold has the highest
positive charge?
А. aluminium
B. copper
C. zinc
D. gold
E. magnesium
3.20. The potential of hydrogen
electrode is standard, if it
responds to:
А. р(Н2) = 1 atm; а(н+) = 1
mol/L
B. р(Н2) = 10 atm; а(н+) = 10
mol/L
C. р(Н2) = 0,1 atm; а(н+) = 0,1
mol/L
D. р(Н2) = 1 atm; а(н+) = 7
mol/L
E. р(Н2) = 0 atm; а(н+) = 0
mol/L
3.21. The potential of zinc electrode is
standard, if it responds to:
А. а((Zn2+)) = 0,1 mol/L
B. а((Zn2+)) = 7 mol/L
C. а(Zn2+) = 1 mol/L
D. а((Zn2+))= 0 mol/L
E. а((Zn2+)) = 10 mol/L
3.22. Equation for the calculation of
electrode potential of the I kind of
electrodes:
А. ϕ = ϕ0 + RT/nF lna(Katn+)
B. ϕ = ϕ0 – RT/nF lna(Ann–)
C. ϕ = ϕ0 + RT/nF lga(Ann–)
D. ϕ = ϕ0 + ⋅lna(Katn+)
E. ϕ = ϕ0 + RT/nF lga(Katn+)
3.23. Equation for the calculation of
electrode potential of the II kind
of electrodes:
А. ϕ = ϕ0 + RT/nF lga(Katn+)
B. ϕ = ϕ0 – lna(Ann–)
C. ϕ = ϕ0 – RT/nF lna(Ann–)
D. ϕ = ϕ0 + RT/nF lna(Katn+)
E. ϕ = ϕ0 + RT/nF lga(Ann–)
3.24. A copper plate is immersed in a
0,1M solution of copper sulfate.
What potential occurs on the
surface area of 2th phases?
А. diffusive
B. contact
C. electrokinetic
D. electrode
E. membrane
3.25. An aluminium place is immersed
in 0.01 M solution of aluminium
sulfate. What potential occurs on
the surface area of 2th phases?
А. diffusive
B. electrokinetic
C. contact
D. electrode
E. membrane
3.26. Standard hydrogen electrode it is
the platinum plate immersed in
solution of H2SO4 at the
temperatures 298 K and
P=1.013·105Pa with activity of
ions of H3O+:
А. 0.5 mol/L
B. 1 mol/L
C. 0.1 mol/L
D. 2 mol/L
E. 0.2 mol/L
3.27. Dependence of value of the
electrode potential on different
factors is expressed by equation
of:
А. Nernst
B. Arrenius
C. Hess
D. Gibbs
E. Vant-Hoff
3.28. The electrode potential of
oxidation-reduction potential is
standard when:
А. аox = аred
B. аox > аred
C. аox = 1 mol/L
D. аred = 1 mol/L
E. аox < аred
3.29. Definition of electrode potential
is:
А. this the jump of potential on
verge of air with solution of
electrolyte
B. this the jump of potential on a
boundary between a metal and
solution of electrolyte
C. this the jump of potential on a
boundary between two metals
D. this the difference of electric
potentials in solution of
electrolyte
E. difference of diaphragm and
diffusive potentials
3.30. Diffusive potential occurs on the
surface area of such phases:
А. solution of electrolyte - air
B. a metal - air
C. a metal - solution of
electrolyte
D. a metal -a metal
E. two solutions of electrolyte of
different concentration
3.31. Diffusive potential occurs as a
result of:
А. identical speed of ions of
electrolyte
B. associations of ions of
electrolyte
C. surplus of cations in initial
solution
D. surplus of anions in initial
solution
E. different speed of ions of
electrolyte
3.32. How to name the potential that
occurs on the boundary between
two solutions divided by a semipermeable membrane?
А. diffusive
B. membrane
C. standard
D. electrode
E. oxidation-reduction
3.33. What is the value of electrode
potential of the silver chloride
electrode in the saturated solution
of KCl?
А. 0.22 V
B. – 0.44 V
C. – 0.22 V
D. 0.25 V
E. 0.44 V
3.34. What is the value of electrode
potential of the calomel electrode
in the saturated solution of KCl?
А. – 0.25 V
B. 0.22 V
C. 0.50 V
D. – 0.50 V
E. 0.25 V
3.35. Which of the given electrodes
silver chloride, calomel,
hydrogen, zinc, copper, may be
used as a reference electrode?
А. zinc
B. silver
C. silver chloride
D. copper
E. hydrogen
3.36. Which of the given electrodes
silver, calomel, hydrogen, zinc,
copper, may be used as a
reference electrode?
А. copper
B. zinc
C. hydrogen
D. silver
E. calomel
3.37. What is the potential of the
hydrogen electrode immersed in
to the distilled water at a standard
temperature?
А. + 0.8 V
B. + 0.4 V
C. – 0.8 V
D. 0 V
E. – 0.4 V
3.38. What is the potential of the
hydrogen electrode immersed in
solution with рН = 2?
А. + 0.12 V
B. + 0.6 V
C. 0 V
D. – 0.6 V
E. – 0.12 V
3.39. What is the potential of the
hydrogen electrode immersed in
solution with рН = 4?
А. – 0.24 V
B. – 0.6 V
C. 0 V
D. + 0.6 V
E. + 0.24 V
3.40. What is the value of electrode
potential of the following cell: Cu|
CuSO4, if concentration of CuSO4
equal 2mol/L and α = 0.5?
А. 0.68 V
B. –0.68 V
C. –0.34 V
D. 0.34 V
E. 0.17 V
3.41. What is the value of electrode
potential of the following cell: Zn|
ZnSO4, if concentration of ZnSO4
equal 4mol/L and α = 0.25?
А. –0.38 V
B. 0.76 V
C. 3.14 V
D. – 3.14 V
E. –0.76 V
3.42. Which of the given galvanic
elements: Weston, Jacobi-Daniell,
acidic accumulator, alkaline
accumulator is used as standard?
А. alkaline accumulator
B. Weston
C. Jacobi-Daniell
D. acidic accumulator
E. 3.43. At the anode occurs next process:
А. increase of galvanic potential
force
B. oxidation
C. reduction
D. E. decrease of galvanic potential
force
3.44. At the cathode occurs next
process:
А. oxidation
B. increase of galvanic potential
force
C. decrease of galvanic potential
force
D. reduction
E. 3.45. The Jacobi-Daniell galvanic
element is based on the reaction:
А. Hg + Zn2+→ Hg2+ + Zn
B. Hg2+ + Zn → Hg + Zn2+
C. Hg22+ + Cd → Cd2+ + 2Hg
D. Cu2+ + Zn → Cu + Zn2+
E. Cu + Zn2+→ Cu2+ + Zn
3.46. The Weston’s element is based on
the reaction:
А. Hg2+ + Zn → Hg + Zn2+
B. Cu2+ + Zn → Cu + Zn2+
C. Cu + Zn2+ →Cu2+ + Zn
D. Hg22+ + Cd →Cd2+ + 2Hg
E. Hg + Zn2+ → Hg2+ + Zn
3.47. Chose the voltaic cell with the
smallest value of galvanic
potential force without
calculation:
А. Zn|Zn2+||Cu2+|Cu
B. Mg|Mg2+||Ni2+|Ni
C. Cd|Cd2+||Ni2+|Ni
D. Cr|Cr2+||Ag+|Ag
E. Co|Co2+||Ni2+|Ni
3.48. Chose the voltaic cell with the
highest value of galvanic potential
force without calculation:
А. Ni|Ni2+||Ag+|Ag
B. Al|Al3+||Cu2+|Cu
C. Al|Al3+||Ag+|Ag
D. Al|Al3+||Fe2+|Fe
E. Mn|Mn2+||Ag+|Ag
3.49. For the experimental measuring of
galvanic potential force is used
the next method:
А. potentiometry
B. compensation
C. polarography
D. conductometry
E. -
potential force of the JacobiDaniell galvanic element if
activity of cations of metals in
electrode solutions equal 1 mol/L?
А. –0.55 V
B. 1.1 V
C. 0.55 V
D. –0.42 V
E. – 1.1 V
3.51. What is the value of galvanic
potential force of the Weston
element?
А. –1.018 V
B. –0.51 V
C. 0.25 V
D. 0.51 V
E. 1.018 V
3.50. What is the value of galvanic
Chapter 4. The Reduction-Oxidation Potentials Measuring.
Potentiometry Determining of pH for Solutions
and Biological Liquids. Potentiometry Titration
4.1. Chose the oxidation-reduction
electrode through the listed ones
whose potential depends on the
pH of solution:
А. Pt | Mn2+, MnO4–
B. Pt | Ce3+, Ce4+
C. Pt | Fe2+, Fe3+
D. Pt | Co2+, Co3+
E. Pt | Sn2+, Sn4+
4.2. To which kind of electrodes does
the chingydrone electrode belong
to?
А. a gas electrode
B. the second kind electrode
C. the ion-selective electrode
D. the first kind electrode
E. the oxidation-reduction
electrode
4.3. The direction of the oxidationreduction reaction passing may be
determined:
А. by the values of standard
electrode potentials of of the
oxidizing and reducing agents
B. by the value of pH of solution
C. by the value of the potential
jump during the redox reaction
D. by the temperature of the
system
E. by the difference of standard
electrode potentials of the
oxidizing and reducing agents
4.4. To which kind of electrodes does
the following electrode Au|Sn4+,
Sn2+ belong to?
А. the ion-selective electrode
B. the indicator electrode
C. a gas electrode
D. the oxidation-reduction
electrode
E. the reference electrode
4.5. To which kind of electrodes does
the following electrode Pt|KI, I–
belong to?
А. the reference electrode
B. a gas electrode
C. the oxidation-reduction
electrode
D. the ion-selective electrode
E. the indicator electrode
4.6. What are the criteria of the
spontaneous redox reaction?
А. E > 0; ∆G > 0
B. E < 0; ∆G = 0
C. E < 0; ∆G > 0
D. E > 0; ∆G < 0
E. E = 0; ∆G > 0
4.7. What equation is applied for the
calculation of the oxidationreduction electrodes potential?
А. Kolraush equation
B.Nernst equation
C. Peters equation
D. Gibbs equation
E. Holdman equation
4.8. Which pair of electrodes
(indicator and reference) is
impossible to use for determining
the pH of solution?
А. glass electrode – silver/silver
chloride electrode
B. standard hydrogen electrode –
hydrogen electrode
C. standard hydrogen electrode –
glass electrode
D. hydrogen electrode –
silver/silver chloride electrode
E. standard hydrogen electrode –
silver/silver chloride electrode
4.9. Which pair of electrodes
(indicator and reference) can be
used for determining the pH of
solution?
А. glass electrode– quinonehydroquinone electrode
B. hydrogen electrode –
quinone-hydroquinone
electrode
C. glass electrode – hydrogen
electrode
D. calomel – silver/silver chloride
electrode
E. hydrogen electrode –
silver/silver chloride electrode
4.10. Which electrode through the listed
ones is used as a reference
electrode for the potentiometry
determining of pH?
А. standard hydrogen electrode
B. quinone-hydroquinone
electrode
C. glass electrode
D. hydrogen electrode
E. zinc electrode
4.11. Which electrode through the listed
ones can not be used as the
indicator electrode for the
potentiometry determining of pH?
А. antimony electrode
B. quinone-hydroquinone
electrode
C. glass electrode
D. hydrogen electrode
E. standard hydrogen electrode
4.12. Which pair of electrodes
(indicator and reference) can be
used for determining the pH of
solution?
А. copper electrode – hydrogen
electrode
B. zinc electrode– silver/silver
chloride electrode
C. copper electrode – calomel
electrode
D. glass electrode – saturated
calomel electrode
E. oxygen electrode – quinonehydroquinone electrode
4.13. What is the pH of the analyte
solution, if the potential of a
galvanic cell consisting of
hydrogen and calomel electrodes
(STP) is 0.43 V. The standard
potential of the calomel electrode
is +0,25 V.
А. 3.1
B. 2.1
C. 3.3
D. 2.1
E. 4.7
4.14. What is the pH of the analyte
solution, if the potential of a
galvanic cell consisting of
hydrogen and silver/silver
chloride electrodes (STP) is 0.515
V. The standard potential of the
silver/silver chloride electrode is
+0.22 V.
А. 4
B. 2
C. 3
D. 5
E. 6
4.15. What is the value of the quinonehydroquinone electrode potential
if it is immersed in solution with
activity of hydrogen ions of H+ =
1 mol/L?
А. 0 V
B. 0.354 V
C. –0.708 V
D. 0.708 V
E. –0.354 V
4.16. What is the value of the quinonehydroquinone electrode potential
if it is immersed in solution with
pH = 5?
А. 0.5 V
B. 0.7 V
C. 0.4 V
D. –0.5 V
E. -0.4 V
4.17. Which electrode through the listed
ones can be used as the indicator
electrode for the potentiometry
determining of pH?
А. copper electrode
B. zinc electrode
C. calomel electrode
D. Silver/silver chloride electrode
E. glass electrode
4.18. Which electrode through the listed
ones is used as a reference
electrode for the potentiometry
determining of pH?
А. glass electrode
B. saturated calomel electrode
C. hydrogen electrode
D. copper electrode
E. quinone-hydroquinone
electrode
4.19. What is the pH of the analyte
solution, if the potential of a
galvanic cell consisting of
quinone-hydroquinone and
calomel electrodes (STP) is 0.31
V. The standard potentials of the
calomel and quinonehydroquinone electrodes are +0,25
V and 0.708 V, respectively.
А. 1.5
B. 4.5
C. 3.5
D. 2.5
E. 0.5
4.20. What is the pH of the analyte
solution, if the potential of a
galvanic cell consisting of
quinone-hydroquinone and
silver/silver chloride electrodes
(STP) is 0.37 V. The standard
potentials of the silver/silver
chloride and quinonehydroquinone electrodes are +0,22
V and 0.708 V, respectively.
А. 0.5
B. 5
C. 4
D. 3
E. 2
4.21. For quantitative determination of
potassium hydroxide
concentration in the solution the
method of potentiometry titration
was used. The equivalence point
in this method is determined as
the rapid change of:
А. diffusion current
B. galvanic cell potential
C. conductivity
D. strength of current
E. fluorescence intensity
4.22. The concentration of sodium
bromide NaBr solution was
determined by the method of
potentiometry titration. Standard
solution of silver nitrate AgNO3
was used as a titrant. Choose the
indicator electrode:
А. hydrogen electrode
B. antimony electrode
C. platinum electrode
D. silver/silver chloride electrode
E. silver electrode
4.23. The concentration of potassium
chloride KCl solution was
determined by the method of
potentiometry titration. Standard
solution of silver nitrate AgNO3
was used as a titrant. Choose the
indicator electrode:
А. platinum electrode
B. hydrogen electrode
C. mercury electrode
D. silver/silver chloride electrode
E. glass electrode
4.24. Which electrode through the listed
ones can be used as a reference
electrode in the potentiometry
method of determining pH of
solutions?
А. copper electrode
B. quinone-hydroquinone
electrode
C. glass electrode
D. hydrogen electrode
E. saturated calomel electrode
4.25. Which electrode through the listed
ones can be used as an indicator
electrode in the potentiometry
method of determining pH of
biological liquids?
А. silver electrode
B. calomel electrode
C. glass electrode
D. silver/silver chloride electrode
E. platinum electrode
4.26. FeSO4 solution was titrated with
the standard solution of potassium
permanganate KMnO4. Which
electrode through the listed ones
can be used as an indicator
electrode for the potentiometry
determining the end point of such
titration?
А. silver/silver chloride electrode
B. platinum electrode
C. hydrogen electrode
D. glass electrode
E. calomel electrode
4.27. Which electrode through the listed
ones can be used as an indicator
electrode for the potentiometry
titration of solution, which
contains ammonium hydroxide
NH4OH and sodium hydroxide
NaOH?
А. silver/silver chloride electrode
B. platinum electrode
C. glass electrode
D. zinc electrode
E. silver electrode
4.28. Which electrode through the listed
ones can be used as an indicator
electrode for the potentiometry
titration of solution, which
contains acetic CH3COOH and
hydrochloric HCl acids?
А. silver electrode
B. silver/silver chloride electrode
C. zinc electrode
D. glass electrode
E. platinum electrode
4.29. One of electrochemical methods
of analysis is the method of
potentiometry titration. It is based
on the measuring:
А. surface potential
B. dzeta-potential ζ
C. the potential of the reference
electrode
D. the potential of the oxidationreduction system
E. the potential of the indicator
electrode
4.30. Which electrode through the listed
ones can be used as a reference
electrode in the potentiometry?
А. hydrogen electrode
B. quinone-hydroquinone
electrode
C. saturated silver/silver chloride
electrode
D. glass electrode
E. copper electrode
4.31. Which electrode through the listed
ones can be used as an indicator
electrode in the potentiometry
titration of bases solutions?
А. glass electrode
B. platinum electrode
C. silver/silver chloride electrode
D. calomel electrode
E. quinone-hydroquinone
electrode
4.32. What kind of titration may be
carried out using the following
galvanic cell:
Ag|AgCl|HCl||glass
membrane||analyte
solution||KCl|AgCl|Ag?
А. acid –base titration
B. amperometry titration
C. oxidation-reduction titration
D. precipitation titration
E. complexometry titration
4.33. Which electrode through the listed
ones can be used as an indicator
electrode in the potentiometry
titration of KBr solutions?
А. silver electrode
B. quinone-hydroquinone
electrode
C. hydrogen electrode
D. silver/silver chloride electrode
E. calomel electrode
4.34. The following curve of titration is:
А. the curve of conductometry
titration
B. volt-amperometry curve
C. the integral curve of
potentiometry titration
D. the curve of amperometry
titration
E. the differential curve of
potentiometry titration
4.35. Which pair of electrodes
(reference and indicator) can be
used for the determining of the
sulfuric acid H2SO4 solution
concentration by the
potentiometry titration method?
А. mercury electrode –cadmium
electrode
B. copper electrode –zinc
electrode
C. silver/silver chloride electrode
–calomel electrode
D. silver/silver chloride electrode
– glass electrode
E. quinone-hydroquinone
electrode – silver/silver
chloride electrode
4.36. The equivalence point in the
potentiometry titration can by find
as:
А. the maximum value of the
galvanic cell potential E
B. the middle of jump of titration
C. the minimum of jump of
titration
D. the maximum of jump of
titration
E. the value of pH
4.37. Which point on the differential
curve of titration corresponds to
the equivalence point of the
potentiometry titration?
А. maximum of curve
B. maximum of jump of titration
C. minimum of jump of titration
D. middle of jump of titration
E. minimum of curve
4.38. Which electrode through the listed
ones can be used as an indicator
electrode for the potentiometry
acid-base titration?
А. silver/silver chloride electrode
B. glass electrode
C. calomel electrode
D. standard hydrogen electrode
E. quinone-hydroquinone
electrode
4.39. Which electrode through the listed
ones can be used as a reference
electrode in the potentiometry
titration?
А. glass electrode
B. hydrogen electrode
C. antimony electrode
D. quinone-hydroquinone
electrode
E. silver/silver chloride electrode
4.40. In the method of potentiometry
titration an electrode can be used
as the indicator electrode if its
potential value:
А. does not depend on the
temperature of solution
B. does not depend on the
concentration of certain ions
of titrant
C. is a constant
D. depends on the temperature of
solution
E. depends on the concentration
of certain ions of titrant or
analyte solution
4.41. In the method of potentiometry
titration an electrode can be used
as the reference electrode if its
potential value:
А. depends on concentration of
solution
B. depends on concentration of a
titratn
C. changes in the process of
titration
D. does not depend on a
temperature
E. is a constant under the
conditions of titration
B. antimony electrode
C. calomel electrode
D. quinone-hydroquinone
electrode
E. glass electrode
4.44. What parameters values should be
measured experimentally for
drawing the integral curve of
potentiometry titration?
А. the volume of a titrant
B. the value of the reference
electrode potential
C. point of equivalence
D. the value of galvanic cell
potential E in the process of
titration
E. the volume of the analyte
solution
4.42. Which electrode through the listed
ones can be used as an indicator
electrode in the method of
potentiometry titration which is
based on the precipitation
reactions?
А. hydrogen electrode
B. silver electrode
C. glass electrode
D. silver/silver chloride electrode
E. calomel electrode
4.45. Which pair of electrodes
(indicator and reference) can be
used for the determining of the
acetic acid CH3COOH
concentration in the solution by
the potentiometry titration
method?
А. copper electrode – hydrogen
electrode
B. copper electrode – calomel
electrode
C. glass electrode – saturated
calomel electrode
D. oxygen electrode– quinonehydroquinone electrode
E. zinc electrode – silver/silver
chloride electrode
4.43. Which electrode through the listed
ones can be used as a reference
electrode in the method of
potentiometry titration which is
based on the precipitation
reactions?
А. hydrogen electrode
4.46. Which pair of electrodes
(reference and indicator) can be
used for the determining of the
potassium hydroxide KOH
concentration in the solution by
the potentiometry titration
method?
А. silver/silver chloride electrode
– calomel electrode
B. Weston cell
C. silver/silver chloride electrode
– glass electrode
D. oxygen electrode– quinonehydroquinone electrode
E. Daniel galvanic cell
electrode in the oxidationreduction potentiometry titration?
А. calomel electrode
B. quinone-hydroquinone
electrode
C. platinum electrode
D. standard hydrogen electrode
E. silver/silver chloride electrode
4.47. Which electrode through the listed
one can be used as an indicator
Chapter 5. The Surface Tension and Surface-Active
Substances. Adsorption on the Movable
Interfaces
5.1. According to the Traube’s rule coefficient of Traube is equal:
А. 2-3
B. 3-3.5
C. 1-2
D. 0-1
E. 4-4.5
5.2. What factor influences on the
value of maximum adsorption of
surface active compounds on a
liquid – gas interfaces?
А. surface area of functional
group of surface active
compounds
B. length of hydrocarbon radical
C. area of interfaces
D. number of the active centers of
interfaces
E. concentration of solution of
surface active compounds
5.3. The positive absorption of surface
active compounds is explained by:
А. B. chemical interaction of
molecules of surface active
compounds and water
C. small solubility of surface
active compounds in water.
D. flowing of chemical reactions
E. weak interaction of dipole of
water with the molecules of
surface active compounds
5.4. Which of the given liquids has the
maximal value of surface tension?
А. chloroform
B. ethanol
C. acetone
D. benzol
E. water
5.5. Chose the surface active
compound which can be adsorbed
on a water solution – air interfaces
А. NaCl
B. sucrose
C. NaOH
D. butyric acid
E. HCI
5.6. Which equation can be used for
the calculation of surface tension
of propionic acid?
А. Langmuir’
B. Freundlich’
C. Rayleigh’
D. E. Gibbs’
5.7. The characteristic property of
structure of surface active
compound is:
А. B. C. polarity
D. no polarity
E. amphophilic
5.8. How will change physical and
chemical properties at diminishing
of length of hydrocarbon radical
in the molecules of surface active
compounds?
А. decrease interfacial tension
B. C. adsorption increases
D. increase surface activity
E. hydrophylic properties
increase
5.9. Which of the listed compounds
belong to surface active?
А. sulfoacids, amines
B. soap and hydrocarboxylic
acids
C. mineral acids and salts
D. alkalis, inorganic acids
E. alcohols and bases
5.10. Surface tension is:
А. work, required to decrease
the area of a surface on 1sm2
B. work, required to decrease the
area of a surface on 1m2
C. work, required to increase the
area of a surface on 1m2
D. free surface energy attributed
to unit of surface
E. work, required to increase the
area of a surface on 1sm2
5.11. What reason of origin of surface
free energy?
А. uncompensated forces of
interaction between the
molecules on the boundary of
two phases
B. the power field of interaction
between the molecules is
balanced
C. the molecules of superficial
layer stronger are attracted by
the molecules of gas, than
liquids
D. bad solubility in the system
E. good solubility in the system
5.12. Water has anomalous large
surface tension because:
А. large forces of attraction
between dipole of water
B. constantly evaporation
C. small forces of attraction
between dipole of water
D. small reserve of surface free
energy
E. forces of interaction between
the molecules do not exist
5.13. With increasing temperature the
surface tension:
А. increased, then decrease
B. decrease, then increased
C. decrease
D. increase
E. does not change
5.14. The reserve of surface free energy
can be decreased when:
А. B. increase the boundary between
two phases
C. decrease the boundary
between two phases
D. increase the surface tension
E. decrease the surface tension
5.15. How to explain from the
molecular point of view of
decreasing of surface tension with
the increase of temperature?
А. formation of new structures
B. forces of interaction between
the molecules increase
C. decreasing of reserve of
surface free energy
D. forces of interaction between
the molecules in the solution
and on the boundary of two
phases decrease
E. increasing of reserve of
surface free energy
5.16. For measuring of surface tension
of liquid apply methods:
А. conductometry
B. maximal pressure of formation
and tearing off a bubbles of air
C. refractometry
D. E. ponentiometry
5.17. Which of the listed compounds
belong to surface active?
А. mineral acids and salts
B. alcohols and bases
C. alkalis, inorganic acids
D. sulfoacids, amines
E. soap and hydrogen carboxylic
acids
5.18. Surface active compounds:
А. insoluble in water
B. does not change surface
tension of water
C. increase the surface tension of
water
D. decrease the surface tension of
water
E. dissolved in water
5.19. An oktanol (C8H17OH) decreases
the surface tension of water,
because it:
А. has small own surface tension
B. has large surface tension
C. insoluble in water
D. surface tension is constant
E. well absorbed
5.20. How will change the value of
surface tension of C5H11OH
when it diluted by water?
А. B. decrease rapidly
C. decrease
D. does not change
E. increase
5.21. Surface activity is:
А. increase of adsorption at
decreasing of concentration of
substance on unit
B. relation between change of
surface tension of the solution
toward the change of
concentration of substance on
unit
C. relation between surface
energy and unit of volume
D. change of surface of solution
at the change of concentration
of substance on unit
E. superficial energy attributed to
unit of surface
5.22. How does the change surface
activity of alcohols with the
increasing of number of carbon
atoms in a molecule?
А.
B.
C.
D.
E.
increase
decrease
does not change
-
5.23. Formulate the Duclo – Traube’s
rule.
А. at the increase of length of
hydrocarbon radical on a
group CH2– surface tension
increase in 3–3,5 times
B. at the decreasing of length of
hydrocarbon radical surface
tension decrease
C. surface activity increases in 33.5 times when one group
CH2– is added to the
hydrocarbon radical of
homologous row
D. at the increasing of length of
hydrocarbon radical on a
group CH2– surface tension
increase in 2–34 times
E. 5.24. In which of the given rows acid
are placed in order of decreasing
of surface tension their solutions
of the same concentration?
А. B. CH3COOH – C3H7COOH –
C4H9COOH – C8H17COOH
C. CH3COOH – HCOOH –
C3H7COOH – C5H11COOH
D. no one
E. C8H17COOH – C5H11COOH –
C2H5COOH – HCOOH
5.25. At diminishing of length of
hydrocarbon radical in the
molecules of surface active
compounds:
А. surface activity increase
B. own surface tension increase
C. solubility increase
D. no one
E. hydrophilic properties increase
5.26. In the case when surface tension
decrease, adsorption will be:
А. A > 0
B. A = 0
C. A < 0
D. A = 1
E. A < 1
5.27. The unit of measure of surface
tension:
А. N/mol
B. N/mol⋅m2
C. J/mol
D. J/mol⋅K
E. J/m2
5.28. Compounds, which decrease the
surface tension of water is
named:
А. surface no active
B. optically active
C. surface active compounds
D. nothing of listed
E. 5.29. Positive adsorption is:
А. B. solubility of compound in the
volume of solution
C. decreasing of concentration of
compound in a surface layer
D. increasing of concentration of
compound in all volume
E. increasing of concentration of
compound on the boundary of
two phases
5.30. Gibbs adsorption equation express
connection between:
А. surface tension and
concentration of solution
B. all listed
C. nothing of listed
D. adsorption, concentration of
solution and surface activity
E. surface free energy and area of
surface
А.
B.
C.
D.
E.
dissolving
sublimation
absorption
desorbtion
5.31. To the process of sorption belong:
Chapter 6. Adsorption on the Immovable Interfaces. The
Adsorptive Ability of Activated Charcoal
Studying. Ions-Exchange Adsorption and
Chromatographic Methods of Analysis
6.1. Application of active coal for
cleaning of antibiotics is based on
the process of spontaneous change
of concentration of a component
in the superficial layer of aqueous
solutions, comparatively with the
bulk of the solution. This process
is:
А. adhesion
B. moistening
C. cohesion
D. desorption
E. adsorption
6.2. Application of activated coal in
medical practice is based on its:
А. high adsorptivity
B. lipophilic properties
C. solubility in water
D. low density
E. hydrophilic properties
6.3. The adsorption of gases with a
solid adsorbent does not depend
on:
А. partial pressure
B. specific surface of the
adsorbent
C. nature of a gas
D. temperature
E. volume of a gas
6.4. A process under which the
chemical interaction between the
molecules of adsorbate and
superficially-active molecules of
adsorbent takes place is referred
to as:
А. adsorption
B. chemisorption
C. desorption
D. Sublimation
E. hydration
6.5. The adsorption process can be
referred to as:
А. the releasing of the surface of
an adsorbent from the
adsorbate molecules
B. penetration of adsorbate in
the volume of adsorbent
C. the change of concentration of
a compound on the surface of
the adsorbent
D. changing the concentration of
a compound in solution
E. interaction between two
species with different charges
6.6. Which one of the listed
phenomena belongs to the
sorption process?
А. sublimation
B. fractionating
C. desorption
D. absorption
E. dissolution
6.7. What species are called
adsorbents?
А. which absorbs other substances
both with their volume and
surface
B. which can not release their
surfaces from the adsorbate
molecules
C. on the surface of which
adsorption takes place
D. which can absorb other
substance by all volume
E. which are penetrating in the
bulk of other substance
6.8. The heat of adsorption is such
amount of heat which:
А. is released under the
desorption of all mass of
adsorbate
B. is taken in under the adsorption
with a 1 mole of the adsorbent
C. is taken in under the adsorption
of a 1 mole of adsorbate
D. is released under the
adsorption of all mass of
adsorbate
E. is released under the
adsorption of a 1 mole of
adsorbate
6.9. How does the process of physical
adsorption change with the
decreasing of temperature?
А. none is true
B. it is decreased
C. does not change
D. it is increased
E. all statements are correct
6.10. How does the process of
chemisorption change with the
increasing of temperature?
А. It is decreased sinewave
B. it is increased sinewave
C. does not change
D. it is increased
E. it is decreased
6.11. What is the main principle which
is the basis of the Langmuir
theory of mono-molecular
adsorption?
А. adsorption takes place only on
the active centers of the
adsorbent surface
B. adsorption takes place on the
whole surface of the adsorbent
C. adsorbate is distributed on an
adsorbent by a poly-molecular
layer
D. chemical interaction between
the adsorbent and adsorbate
molecules takes place
E. adsorption takes place only in
the volume of adsorbent
6.12. What is the physical meaning of
the constant “K” in empiric
Freundlich equation?
А. n/m = K, if m =100
B. n/m = K, if m =10
C. n/m = K, if m =1
D. n/m = K, if n = 1
E. n/m = K, if p = 1
6.13. What theory contains the
statement about the formation of
poly-molecular layers?
А. Gibbs theory
B. Langmuir theory
C. Freundlich theory
D. BET theory
E. Arrhenius theory
6.14. Which factors through the listed
ones can influence on the
adsorption of compounds from
solutions?
А. volume of solution, mass of
adsorbent
B. nature of solute, solvent, and
adsorbent
C. pressure, mass of solution
D. all listed factors
E. none of the listed factors
6.15. What is the physical meaning of
the coefficient “K” in the
Langmuir adsorption isotherm
equation?
А. the constant of kinetic
equilibrium
B. the constant of the adsorption
equilibrium
C. the value of the maximal
adsorption
D. the value of the surface activity
E. the value of maximal
desorption
6.16. Which one of the given equations
is the mathematical expression for
the Langmuir isotherm?
А.
Kp
a = a max
1 + Kp
1 + Kp
)
Kp
C. 1
1 1 + Kp
=
⋅
a a max
Kp
B.
log a = log(a max
D. none
E.
a = a max
1 + Kp
Kp
6.17. Which one of the given equations
is the mathematical expression for
the Freundlich isotherm?
1
А.
n 1 + KC n
a= =
m
KC
B.
1
n
a=
= KC n
m
C.
n
a = = KC n
m
D.
1
n
KC n
a= =
m 1 + KC
E. none
6.18. The constants “amax” and “K” in
the Langmuir isotherm equation
can be found out graphically. The
graph should be built for this in
the following coordinates:
А.
1
B.
C.
D.
E.
a= f( )
p
1
= f ( p)
a
1
1
log = f ( )
a
p
1
1
log = f (log )
a
p
1
1
= f( )
a
p
6.19. The constants “K” and “n” in the
Freundlich isotherm equation can
be found out graphically. The
graph should be built for this in
the following coordinates:
А. n
m
B.
C.
log
= f (log C )
n
= f (C )
m
n
1
= f (log )
m
C
D.
m
log = f (log C )
n
E.
log
log
n
= f (log C )
m
6.20. The equation of the Freundlich
adsorption isotherm can
adequately describe the process of
adsorption under the condition of:
А. high pressures
B. low pressures
C. none
D. moderate pressures
E. different pressures
6.21. The equation of the Langmuir
adsorption isotherm can
adequately describe the process of
adsorption under the condition of:
А. high and low pressures
B. none
C. different pressures
D. moderate pressures
E. doesn’t depend on pressure
6.22. The adsorption isotherm shows
the relationship between:
А. number of moles of a gas
which is adsorbed by 1 g of a
solid as a function of the gas
volume at a constant
temperature
B. volume of a gas which is
adsorbed by 1 g of a solid as a
function of the gas pressure at
a constant temperature
C. number of moles of a gas
which is adsorbed by 1 g of a
solid as a function of the gas
pressure at a constant
temperature
D. volume of a gas which is
adsorbed by 1 mole of a solid
as a function of the gas
pressure at a constant
temperature
E. volume of a gas which is
adsorbed by 1 g of a solid as a
function of the gas pressure at
a constant pressure
6.23. The constants “amax” and “K” in
the Langmuir isotherm equation
can be found out graphically. The
graph (linear) should be built for
this in the coordinates
1
1
= f ( ) . The values of amax”
a
p
and “K” then may be found as:
А.
1
OA =
a max K
1
K
B.
1
OA =
a max
tgα =
tgα =
1
a max K
C. none
D. OA = a
tgα =
max
1
K
E.
OA =
tgα =
D.
K
a max
1
a max
6.24. The constants “K” and “n” in the
Freundlich isotherm equation can
be found out graphically. The
graph (linear) should be built for
this in the coordinates
log
n
= f (log C ) . The values
m
of “K” and “n” then may be found
as:
А.
1
OA = log
B.
tgα = n
1
OA =
K
tgα = log
C.
OA = K
tgα = log
K
1
n
OA = log K
1
tgα =
n
E. none
6.25. The maximal value of adsorption
on the Langmuir isotherm
corresponds to the formation of:
А. non-saturated mono-molecular
layer of the adsorbate
molecules on the surface of
adsorbent
B. saturated mono-molecular
layer of the adsorbent
molecules on the surface of
adsorbate
C. none
D. saturated mono-molecular
layer of the adsorbate
molecules on the surface of
adsorbent
E. saturated poly-molecular layer
of the adsorbate molecules on
the surface of adsorbent
1
n
Chapter 7. Lyophobic Sols Preparation and Their Properties
Studying
7.1. To the colloids belong the systems
with the sizes of particles:
А. 10–9 – 10–4 m
B. 10–9 – 10–7 m
C. <10–9 m
D. >10–4 m
E. 10–7 – 10–4 m
7.2. Particles of AgCl in a water
solution have a size 5#10–6m.
This system is:
А. suspension
B. emulsion
C. colloid
D. aerosol
E. true solution
7.3. Cleaning of blood by a “artificial
kidney”, when a blood flows
between two membranes which
are washed outwardly by the
physiological solution, is based
on:
А. dialysis and ultra-filtration
B. electroforesis
C. D. coagulation
E. dispergation
7.4. The best method of cleaning of sol
from surplus of electrolytes is:
А. ultra-filtration
B. electrodialysis
C. dialysis
D. ordinary filtration
E. electroforesis
7.5. It is possible to clean a sol by the
method of dialysis from
admixtures of:
А. charged particles
B. all listed admixtures
C. macromolecular compounds
D. E. low-molecular compounds
7.6. Completely to separate a
dispersed phase from a dispersion
medium in colloidal solutions it is
possible by a method:
А. electrodialysis
B. ultra-filtration
C. compensative dialysis
D. dialysis
E. 7.7. The process of removing low-
molecular compounds by washing
the colloid with a solvent through
a semi-permeable membrane,
which does not allow the particles
of the colloidal system to pass
through, is named:
А. dialysis
B. diffusion
C. osmosis
D. electroforesis
E. ultra-filtration
7.8. Value of osmotic pressure of
colloid solutions is:
А. high, constant
B. low, variable
C. low, constant
D. high, variable
E. 7.9. Optical properties of sols appear
by the phenomenon:
А. scattering of light
B. diffraction of light
C. absorption of light
D. reflection of light
E. refraction of light
7.10. Which methods are used for
research of properties of colloid
solutions:
А. potentiometry, refractometry
B. polarymetry
C. ultra-microscopy,
nephelometry
D. indicator titration
E. colorymetry
7.11. Which equation is used for the
nephelometry determination of
concentration of a sol?
А. h1/h2 = C1/C2
B. C = ∆T/K
C. h1/h2 = C2/C1
D. C = Vnρ/V0
E. C = 10ρω/M
E.
7.12. Dependence of intensity of
scattering of light in the colloid
system from different factors
describes equation:
А. Bancroft
B. Schulze-Hardy
C. Rayleigh’
D. Tyndal
E. 7.13. Which of the listed methods give
the possibility to count up the
number of particles in a certain
volume of a sol?
А. B. colorymetry
C. dialysis
D. optical microscopy
E. ultra-microscopy
7.14. The sizes of particles in a sol can
be calculated using equation:
А. Stoks
B. Schulze-Hardy
C. Rayleigh’
D. Tyndal
E. 7.15. Which one of the given equation
is the mathematical expression for
the Reley equation?
2
А.
I p = I0 ⋅ K
B.
Ip = I0 ⋅ K
ν ⋅V
λ4
ν ⋅ V2
λ4
C.
ν ⋅ V2
Ip = I0 ⋅ K
λ
D.
ν ⋅ V2
Ip = I0 + K 4
λ
I p = I 0 ⋅ K lg
νV 2
λ4
7.16. At decreasing of diameter of
particles of a sol in 2 times
dispersion of the system:
А. increase in 2 times
B. decrease in 8 times
C. increase in 4 times
D. decrease in 2 times
E. decrease in 4 times
7.17. Apparatus “artificial kidney ”
works on principle:
А. adsorption
B. electrodialysis
C. ultra-filtrations
D. dialysis
E. compensative dialysis
7.18. Which one of the given
electrolytes is a stabilizator of a
sol of the Prussial blue with the
positively charged granules:
А. FeCl3
B. KCl
C. Fe3[Fe(CN)6]
D. K4[Fe(CN)6]
E. any other electrolyte
7.19. Which one of the given
electrolytes is a stabilizator of a
sol AgI with the positively
charged granules:
А. any other electrolyte
B. KNO3
C. KI
D. KCl
E. AgNO3
7.20. Which one of the given salt
hydrolyzes and gives a sol as a
result of the hydrolysis?
А. Na2S
B. NH4Cl
C. FeCl3
D. Na2CO3
E. CH3COOK
7.21. A sol will forms as a result of
interaction between:
А. Na2SO3 + O2 →
B. Na + H2O →
C. H2S + NAOH →
D. NAOH + HCl →
E. H2S + O2 →
7.22. A sol of acid can be formed at the
hydrolysis of salt:
А. Ni(NO3)2
B. FeSO4
C. ZnCl2
D. KH2PO4
E. Na2SiO3
7.23. A sol was formed as a result of
mixing of identical volumes
0,001M solutions AgNO3 and
K2CrO4. What ion is potentialdefined?
А. NO3–
B. K+
C. CrO42–
D. CrO42– or Ag+
E. Ag+
7.24. A sol was formed as a result of
mixing of identical volumes
0,002M solutions of Pb(NO3)2 and
KI. What ions will form the
diffusive layer of micelle?
А. I–
B. Pb2+
C. there is no a diffuse layer
D. K+
E. NO3–
7.25. To get a sol of Fe(OH)3 using the
method of peptisation is required
to add to precipitate of Fe(OH)3:
А. FeOCl
B. HCl
C. FeCl3
D. KOH
E. K4[Fe(CN)6]
7.26. At the standing of the diluted
solutions of FeCl3, the color of
solution darken, opalescence
appears as a result of formation of
a sol Fe(OH)3. What is the name
of method getting a sol?
А. peptization
B. chemical condensation,
reaction of hydrolysis
C. physical condensation
D. chemical condensation,
reaction of double exchange
E. chemical condensation, redox
reaction
7.27. To solution, that contains ions
Na+, Mg2+, Ba2+, Cl–, NO3–, added
solution of KOH. What sol can be
formed?
А. Ba(OH)2
B. BaCl(OH)
C. BaCl2
D. KNO3
E. Mg(OH)2
7.28. Using the reaction of hydrolysis, it
is possible to get a sol of:
А. BaSO4
B. H2SO4
C. Ba(OH)2
D. KOH
E. Ni(OH)2
7.29. What conditions are required, to
get colloids using the method of
chemical condensation?
А. low concentration of solutions,
equivalent of amount of
reactants
B. low concentration of solutions,
heating
C. high concentration of
solutions, heating
D. high concentration of
solutions, surplus of one of
reactants
E. low concentration of solutions,
surplus of one of the reactants
7.30. Which ions can be potentialdefined:
А. ions mobility of which in
solution is highest
B. only complex ions
C. ions with highest charge
D. any ions, present in solution
E. ions, which take part of
insoluble aggregate or form a
structure isomorphous with its
7.31. To get a sol is required to add to
the solution of Pb(NO3)2 :
А. Pb(CH3COO)2
B. HNO3
C. KI
D. BaSO4
E. KNO3
7.32. Specify the colloidal-sized
particle of colloids.
А. micelle
B. free radical
C. molecule
D. ion
E. atom
7.33. To the methods of physical
condensation belongs:
А. hydrolysis
B. reduction
C. double exchange
D. oxidation
E. replacement of solvent
7.34. What requirement is necessary for
the reaction, which can be used
for getting a sol?
А. one of the products of reaction
must be insoluble
B. homogenity
C. high rate
D. E. one of the products of reaction
must be gas
7.35. Which one of the given
electrolytes is a stabilizator of a
sol of the Prussian blue with the
negatively charged granules?
А. Fe3[Fe(CN)6]
B. K4[Fe(CN)6]
C. KCl
D. any other electrolyte
E. FeCl3
7.36. A sol of sulphur is formed as a
result of interaction between
Na2S2O3 with:
А. KCl
B. H2O
C. I2
D. HCl
E. NH3
Chapter 8. The Stability of Colloidal Systems. Coagulation
and Colloidal Protection
8.1. What kind of potential
predetermines the stability of the
colloid systems?
А. zeta-potential
B. diffusive potential
C. thermodynamic potential
D. chemical potential
E. electrode potential
8.2. The directed movement of
dispersion medium relative to a
stationary dispersed phase by an
applied electric field is called:
А. electro-osmosis
B. electrophoresis
C. potential of passing
D. adsorption
E. potential of sedimentation
8.3. The directed movement of
charged particles of dispersed
phase relatively to a stationary
dispersion medium by an applied
electric field is called:
А. potential of passing
B. surface potential
C. electrophoresis
D. potential of sedimentation
E. electro-osmosis
8.4. The method of albumens
separation with electrophoresis is
based on the difference between
their:
А. zeta-potentials
B. their ability to interact with the
molecules of solvent
C. the structure of their molecules
D. solubility
E. molecular masses
8.5. The value of zeta-potential may
be calculated using the following
equation:
А.
ς=
s ⋅η
τ ⋅ E ⋅ ε ⋅ ε0
B.
ς =
s ⋅ l ⋅η
τ ⋅ H ⋅ε ⋅ε 0
C.
ς=
D.
E.
s ⋅ l ⋅ ε 0 ⋅η
E ⋅ε
s ⋅ l ⋅η
ς=
τ ⋅ E ⋅ ε ⋅ ε0
s ⋅ Iscat ⋅ η
ς=
τ ⋅ λ ⋅ I0 ⋅ ε
8.6. What will be the change of the
distance which particles of a sol
will pass if the voltage of the
applied electric field would be
increased twice?
А. increase in 2 times
B. increase in 4 times
C. will not change
D. decrease in 2 times
E. decrease in 4 times
8.7. The value of zeta-potential may
be determined experimentally by
the method of:
А. potentiometry
B. nephelometry
C. electrophoresis and electroosmosis
D. voltamperometry
E. conductometry
8.8. One of the methods which can be
used for determining the charge
sign of colloid particles is:
А. dialysis
B. ultra-microscopy
C. ultra-filtration
D. electrophoresis
E. nephelometry
8.9. At electrophoresis the longest
distance during the identical time
interval can pass those particles
which have:
А. the highest molar mass
B. the least diameter
C. the highest diameter
D. the highest zeta-potential
E. the least molar mass
8.10. The gradient of potential is
calculated according to the
equation:
А. H=ζ•l
B. H=ζ/l
C. H=l/E
D. H=E/l
E. H=E•S
8.11. What part of a colloidal particle
can move in the process of
electrophoresis by an applied the
electric field?
А. micelle on the whole
B. ions only
C. aggregate
D. nuclei
E. granule
8.12. If particles of a sol do not move to
any of the electrodes by an
applied the electric field, this
means that:
А. the size of a sol particles is
greater than a critical size
B. ζ=0
C. sol is contained in a vacuum
D. ζ>0
E. ζ<0
8.13. Method of electrophoresis is
suitable for the separation of:
А. cations of metals
B. suspensions
C. anions
D. biological colloid systems and
albumens
E. electrolytes
8.14. A sol is considered to be stable, if
its zeta-potential is:
А. >30 mV
B. equals to the zero
C. <30 mV
D. >1 mV
E. >10 mV
8.15. The solution of which compound
through the listed 8ones should be
added to a sol to cause its
coagulation?
А. MgCO3
B. CaCO3
C. SrCO3
D. BaSO4
E. MgSO4
8.16. What is the critical concentration
of coagulation?
А. the minimal concentration of a
gel, at exceeding of which the
coagulation is observed
B. the minimal concentration of
non-electrolyte, at exceeding
of which the coagulation is
observed
C. the minimal concentration of
electrolyte, at exceeding of
which the coagulation of a sol
is observed
D. the minimal concentration of
emulsion at exceeding of
which the coagulation is
observed
E. the minimal concentration of a
sol, at exceeding of which the
coagulation is observed
8.17. The positively charged sol of iron
hydroxide Fe(OH)3 was prepared
by the method of hydrolysis.
Which ion through the listed ones
will have the lowest value of the
critical concentration of
coagulation for this sol?
А. bromide-ion BrB. phosphate-ions PO43C. sulfate-ion SO42D. chloride-ion ClE. nitrate-ion NO38.18. The colloidal solution of collargol
in course of time can change the
structure and lose the aggregative
stability as a result of the
aggregation of dispersed phase
particles, this process is called:
А. swelling
B. formation of a gel
C. peptisation
D. coagulation
E. sedimentation
8.19. A sol of AgI was prepared by
adding of 10 ml 0.001 M solution
of AgNO3 to 100 ml KI solution
of the same concentration. Which
electrolyte through the listed ones
will have the lowest value of the
critical concentration of
coagulation for this sol?
А. AlPO4
B. MgSO4
C. NaCl
D. K3[Fe(CN)6]
E. AlCl3
8.20. A sol of AgI was prepared by
adding of 100 ml 0.001 M
solution of AgNO3 to 10 ml KI
solution of the same
concentration. Which electrolyte
through the listed ones will have
the lowest value of the critical
concentration of coagulation for
this sol?
А.
B.
C.
D.
E.
K3[Fe(CN)6]
AlPO4
MgSO4
NaCl
AlCl3
8.21. The coagulation ability of ions
with an identical charge:
А. increases with the decreasing
of the de-hydrated ion radius
B. increases with the increasing
of the hydrated ion radius
C. increases with the increasing
of the de-hydrated ion radius
D. increases with the decreasing
of the hydrated ion radius
E. does not depend on the sizes
of ions
8.22. An ion can cause the coagulation
of a sol only in case when:
А. its charge is the same sign as
the charge of colloid particles
B. it has a positive or negative
charge not less than 2
C. its diameter is greater than the
diameter of dispersion medium
molecules
D. its charge is opposite to the
charge of colloid particles
E. its concentration in solution is
high enough
8.23. A sol of sulphur was prepared by
oxidation hydrogen sulphide H2S
by oxygen of air. Which ion
through the listed ones will have
the highest value of the
coagulation ability for this sol?
А. PO43–
B. Cl–
C. K+
D. [Fe(CN)6]4–
E. Al3+
8.24. For coagulation of a sol the
electrolyte with the 1-charged
coagulating ion was replaced with
an electrolyte with a 2-charged
ion. How the critical
concentration of coagulation will
change?
А. decrease on 2-3 orders
B. decrease in 2 times
C. increase on 2-3 orders
D. decrease in 4 times
E. increase in 2 times
8.25. Which electrolyte through the
listed ones will have the lowest
value of the critical concentration
of coagulation towards a sol of
Al(OH)3, which was prepared
under the reaction of hydrolysis?
А. K3PO4
B. KBr
C. AlCl3
D. CaCl2
E. MgSO4
8.26. A sol of sulphur was prepared by
oxidation hydrogen sulphide H2S
by oxygen of air. Which
electrolyte through the listed ones
will have the highest value of the
coagulation ability for this sol?
А. K3PO4
B. NaCl
C. K2SO4
D. CaCl2
E. AlCl3
8.27. The highest value of the
coagulation ability through the
ions with the same size and sign
of the charge will have those ones
for which:
А. consist of less number of
atoms
B. there is the greatest radius of
the de-hydrated ion
C. there is the smallest radius of
the de-hydrated ion
D. there is the smallest radius of
the hydrated ion
E. there is the greatest radius of
the hydrated ion
8.28. The Schulze-Hardy rule states
that:
А. the critical concentration of
coagulation depends on the
valence of counter ions
B. the critical concentration of
coagulation does not depend
on the charge sign and valence
of coagulating ions
C. the critical concentration of
coagulation depends on the
size of coagulating ions
D. the critical concentration of
coagulation depends on the
charge sign of coagulating
ions
E. the critical concentration of
coagulation depends on the
charge sign and valence of
coagulating ions
The correct answers to test questions
1.1.
1.2.
1.3.
1.4.
1.5.
1.6.
1.7.
1.8.
1.9.
1.10.
1.11.
1.12.
1.13.
1.14.
1.15.
1.16.
1.17.
1.18.
1.19.
1.20.
1.21.
1.22.
1.23.
1.24.
1.25.
1.26.
1.27.
1.28.
1.29.
1.30.
1.31.
1.32.
1.33.
1.34.
1.35.
1.36.
1.37.
1.38.
1.39.
A
B
A
D
E
C
A
E
D
C
E
E
D
C
C
E
C
B
A
A
A
D
E
B
E
E
D
E
E
D
E
A
E
E
E
E
A
A
E
1.40.
1.41.
1.42.
1.43.
1.44.
1.45.
1.46.
1.47.
1.48.
1.49.
1.50.
1.51.
1.52.
1.53.
1.54.
2.1.
2.2.
2.3.
2.4.
2.5.
2.6.
2.7.
2.8.
2.9.
2.10.
2.11.
2.12.
2.13.
2.14.
2.15.
2.16.
2.17.
2.18.
2.19.
2.20.
2.21.
2.22.
2.23.
2.24.
D
A
E
E
D
C
B
C
D
D
A
B
A
B
C
D
E
E
B
C
D
A
E
B
E
A
C
C
A
E
E
E
D
C
C
B
B
C
D
2.25.
2.26.
2.27.
2.28.
2.29.
2.30.
2.31.
2.32.
2.33.
2.34.
2.35.
2.36.
2.37.
2.38.
2.39.
2.40.
2.41.
2.42.
2.43.
2.44.
2.45.
2.46.
2.47.
2.48.
2.49.
2.50.
2.51.
2.52.
2.53.
2.54.
2.55.
2.56.
2.57.
2.58.
2.59.
2.60.
2.61.
2.62.
2.63.
E
E
B
E
C
A
B
D
C
E
C
A
D
D
D
B
C
A
E
A
A
E
C
B
D
E
C
E
B
A
E
C
B
A
C
C
E
D
E
2.64.
3.1.
3.2.
3.3.
3.4.
3.5.
3.6.
3.7.
3.8.
3.9.
3.10.
3.11.
3.12.
3.13.
3.14.
3.15.
3.16.
3.17.
3.18.
3.19.
3.20.
3.21.
3.22.
3.23.
3.24.
3.25.
3.26.
3.27.
3.28.
3.29.
3.30.
3.31.
3.32.
3.33.
3.34.
3.35.
3.36.
3.37.
3.38.
B
E
D
A
A
C
A
A
A
C
D
E
D
D
A
B
E
C
D
D
A
C
A
C
D
D
B
A
A
B
E
E
B
A
E
C
E
E
E
3.39.
3.40.
3.41.
3.42.
3.43.
3.44.
3.45.
3.46.
3.47.
3.48.
3.49.
3.50.
3.51.
4.1.
4.2.
4.3.
4.4.
4.5.
4.6.
4.7.
4.8.
4.9.
4.10.
4.11.
4.12.
4.13.
4.14.
4.15.
4.16.
4.17.
4.18.
4.19.
4.20.
4.21.
4.22.
4.23.
4.24.
4.25.
4.26.
A
D
E
B
B
D
D
D
E
C
B
B
E
A
E
E
D
C
D
C
E
E
A
E
D
A
D
D
C
E
B
D
E
B
E
C
E
C
B
4.27.
4.28.
4.29.
4.30.
4.31.
4.32.
4.33.
4.34.
4.35.
4.36.
4.37.
4.38.
4.39.
4.40.
4.41.
4.42.
4.43.
4.44.
4.45.
4.46.
4.47.
5.1.
5.2.
5.3.
5.4.
5.5.
5.6.
5.7.
5.8.
C
D
E
C
A
A
A
E
D
B
A
B
E
E
E
B
C
D
C
C
C
B
A
E
E
D
E
E
E
5.9.
5.10.
5.11.
5.12.
5.13.
5.14.
5.15.
5.16.
5.17.
5.18.
5.19.
5.20.
5.21.
5.22.
5.23.
5.24.
5.25.
5.26.
5.27.
5.28.
5.29.
5.30.
5.31.
6.1.
6.2.
6.3.
6.4.
6.5.
6.6.
B
C
A
A
C
E
D
B
E
D
A
E
B
B
C
B
B
A
E
C
E
D
D
E
A
E
B
C
D
6.7.
6.8.
6.9.
6.10.
6.11.
6.12.
6.13.
6.14.
6.15.
6.16.
6.17.
6.18.
6.19.
6.20.
6.21.
6.22.
6.23.
6.24.
6.25.
7.1.
7.2.
7.3.
7.4.
7.5.
7.6.
7.7.
7.8.
7.9.
7.10.
C
E
D
D
A
E
D
B
B
A
B
E
E
D
A
C
B
D
D
B
A
A
B
E
B
A
B
A
C
7.11.
7.12.
7.13.
7.14.
7.15.
7.16.
7.17.
7.18.
7.19.
7.20.
7.21.
7.22.
7.23.
7.24.
7.25.
7.26.
7.27.
7.28.
7.29.
7.30.
7.31.
7.32.
7.33.
7.34.
7.35.
7.36.
8.1.
8.2.
8.3.
C
C
E
C
B
A
E
A
E
C
E
E
C
E
B
B
E
E
E
E
C
A
E
A
B
D
A
A
C
8.4.
8.5.
8.6.
8.7.
8.8.
8.9.
8.10.
8.11.
8.12.
8.13.
8.14.
8.15.
8.16.
8.17.
8.18.
8.19.
8.20.
8.21.
8.22.
8.23.
8.24.
8.25.
8.26.
8.27.
8.28.
A
D
A
C
D
D
D
E
B
D
A
E
C
B
D
E
A
D
D
E
A
A
E
D
E
CONTENTS
Chapter 1. Energetics of Chemical Reactions and Processes. Calculations
According Thermochemical Equations and Experimental
Determination of Heat Effects of Chemical Processes. Bioenergetics ......... 2
Chapter 2. Kinetics of Chemical Reactions. Chemical Equilibrium. Solubility
Product Constant........................................................................................... 8
Chapter 3. Measuring the Electromotive Forces of Galvanic Cells and
Electrode Potentials .................................................................................... 16
Chapter 4. The Reduction-Oxidation Potentials Measuring. Potentiometry
Determining of pH for Solutions and Biological Liquids.
Potentiometry Titration............................................................................... 21
Chapter 5. The Surface Tension and Surface-Active Substances. Adsorption on
the Movable Interfaces ............................................................................... 28
Chapter 6. Adsorption on the Immovable Interfaces. The Adsorptive Ability of
Activated Charcoal Studying. Ions-Exchange Adsorption and
Chromatographic Methods of Analysis ...................................................... 32
Chapter 7. Lyophobic Sols Preparation and Their Properties Studying ...................... 36
Chapter 8. The Stability of Colloidal Systems. Coagulation and Colloidal
Protection.................................................................................................... 40
The correct answers to test questions .......................................................................... 45