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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