Download CHM 1033 Chemistry for Health Sciences

Work Assignment I
CHM 1033 Chemistry for Health Sciences
(Study and practice all questions. Select only 25 for your Home Work Assignment grade)
Assignment I
(5 points)
Due __________________
Chapter 1
1. Resolve the following operation. Round off your answer according to the data’s lowest number of
significant figures:
a)
(56.55)(0.920) =
34.2585
2. Convert into Scientific Notation:
a) 1,700 000 m =
b)
1.01 x 0.12 x 53.51 =
96
b) 0.000501 g =
3.
4.
5.
6.
7.
An engine block part displaces a volume of 4.77 L and weighs 28.4 lb. What is the density of this material?
Determine how many grams are in 63.2 ml alcohol, if the density is 0.79 g/ml
Determine the volume of 100.0 g alcohol, if the density is 0.79 g/ml
Determine the spec gravity of 500 ml alcohol if the density is 0.79 g/ml
A graduated cylinder contains 20.0 ml of water. When a 100. g solid piece of brass was added to the
graduated cylinder, the water level rose to 32.6 ml. What is the density of brass?
8. When a 0.255 lb metal was dropped into 25.0 ml of water, the level of the water rose to 27.6 ml. What is the
density of the metal?
9. Concentrated sulfuric acid has a density of 1.84 g/ml. Calculate the mass in grams of 1.00 liter sulfuric acid.
Determine its specific gravity.
10. Concentrated sulfuric acid has a density of 1.84 g/ml. Calculate the volume in ml of 1.00 Kg sulfuric acid.
Determine its specific gravity.
11. Find the density of a piece of wood that has a mass of 7.35 g and occupies a volume of 8.20 ml
12. What is the density of an unknown solution if the bottle label shows spec. gravity is 1.12?
13. A liquid has a mass of 27.45 g. When it is measured in a graduated cylinder, the meniscus shows 21.5 ml.
What is the density of the liquid? What is the specific gravity?
14. Equal quantities of olive oil and water are mixed into a glass. The mixture is stirred for a few minutes. After
settling, a separation is observed showing one liquid on top and one on the bottom. Find out the density of
each of these liquids and explain why olive oil is on the top?
15. Why would a piece of steel metal sinks in water while a piece of wood floats?
16. Calculate the density of a cylindrical metal rod that weights 2.75 lb if you know that the total rod volume is
110.3 cubic centimeters
17. Determine the mass (in grams) of 1.0 liter alcohol, if the density is 0.79 g/ml. What is the specific gravity of
the alcohol?
18. An engine part weights 0.82 lb. When measured in a graduated cylinder containing water it displaces a
volume of 125.5 ml of water. What is the density of this material?
19. (a) Carbon Dioxide gas is denser than air. If a tank containing CO2 had a leak, the gas will be found most
likely near the ceiling _______ (True or False) (Note: dAir = 0.00128 g/mL; dCO2 = 0.00198 g/mL)
(b) The density of a 45 g mercury sample at 25°C should be higher than the density of this same mercury
mass at 40°C ________ (True or False)
20. Diamonds are measured in carats and one carat equals 0.200 grams (Density of diamond = 3.51g/cm3)
What is the volume in cm3 of a 5.0 carat diamond?
(a) 3.51 cm3
(b) 3.5 cm3
(c) 1.42 cm3
(d) 0.284 cm3
(e) 0.28 cm3
21. An infant ibuprofen suspension contains 100 mg/5.0 mL suspension. The recommended dose is 10 mg/kg body
weight. How many mL of this suspension should be given to an infant weighing 18 lb? (1 lb = 453.59 g)
(a) 5.7 mL
(b) 2.0 mL
(c) 1.6 mL
(d) 3.4 mL
(e) 4.1 mL
22. A cylindrical piece of rubber has a mass of 16.0 g, a radius of 1.25 cm, and a height of 3.5 cm.
If toluene (d=0.867 g/mL), water (d=1.00 g/mL), and above piece of rubber are dropped into a cylinder, what
will be their order in the cylinder, from bottom to top (cylinder V=πr2h)
(1) Rubber, toluene, water
(2) Toluene, rubber, water
(3) Rubber, water, toluene
(4) Toluene, water, rubber
(5) Water, rubber, toluene
(6) None of the above
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 1 of 14
Work Assignment I
Chapter 2
1. Classify each type of matter as a pure substance or a mixture. If it is a pure substance, classify it as element or
Compound; if it is a mixture, classify it as homogeneous or heterogeneous.
a) a lead weight
g) oil mixed with water
d) Italian salad dressing
b) seawater
e) mercury in a thermometer
h) sand added to a glass of water
c) distilled water
f) air
i) sugar
2. Classify each of the following changes as physical or chemical:
a) Sugar turning into caramel
b) ice melting on the street
c) toasting a marshmallow
d) cutting a paper
e) iron rusting in an old car
f) burning a paper
g) tarnishing of silver
h) movement of iron particles by a magnet
i) polishing of a copper pot
j) freezing of water
k) condensation of water
l) vaporization of alcohol
3. Select the warmer temperature in each pair (Show the conversions):
a) 10°C or 10°F
b) 30°C or 15°F
c) -10°C or 32°F
d) 200°C or 200°K
4. Using the Caloric values for food:
a. Determine the total quantity of kilocalories for one serving of peanut butter if each serving
contains 6 g carbohydrate, 16 g fat and 7 g protein.
b. Convert above kilocalories to Nutritional Calories (Cal) and then to joules.
5.
Determine the total amount of kilocalories for one cup of orange juice that contains 26 g carbohydrate,
no fat and 2 g protein.
6.
A 70.0 Kg person had a pizza slice, a glass of soda and an ice cream (Composition: Pizza slice had 13 g
protein, 10 g fat, 29 g carbohydrate; the soda drink had 51 carbohydrate, no fat, no protein; the ice cream had
8 g protein, 28 g fat and 44 g carbohydrate) What is the total amount of kilocalories obtained from this meal?
7.
Using the caloric values for food, calculate the kcal in one cup of whole milk containing 12 g carbohydrate,
9 g protein and 9 g fat
8.
Using the caloric values for food, determine how many kilocalories are in 8 oz of cream cheese if it has 5 g
of carbohydrate, 86 g of fat and 18 g of protein.
9.
Using the caloric values for food, determine how many thermal calories are in one breakfast roll if it has
30 g of carbohydrate, 15 g of fat and 5 g of protein. What is the equivalency on nutritional calories?
10. Convert 25.0º and 29.9º C temperature measurements to ºF and K.
11. Convert 155°F, 78°F and 42°F to K and ºC
12. How many calories must be added to warm 45 g of water from 12ºC to 76ºC?
See data on Reference notes (*) at the end of this section.
13. How many joules are required to heat 100 g of water from 15ºC to 95ºC?
(Note: The specific heat capacity of water is SH = 4.184 J/gºC)
14. How many joules are required to raise the temperature of 125 g copper from 22°C to 325°C.
(Note: The specific heat of copper is SH = 0.385 j/g°C)
15. How much heat in calories must be removed from 150 g of water at 0°C inside a freezer to form ice?
(assume temp remains constant at 0°C) See data on Reference notes (*) at the end of this section.
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 2 of 14
Work Assignment I
16. When steam from a pan of boiling water reaches a cool window, it condenses. How much heat in kilocalories
is released when 25 g of steam condenses at 100°C? See data on Reference notes (*) at the end of this section.
17. Calculate the kilocalories absorbed when 50.0 g of water evaporates at 100°C?
See data on Reference notes (*) at the end of this section.
18. Calculate the kilocalories released when 50.0 g of steam condenses at 100°C?
See data on Reference notes (*) at the end of this section.
19.
Calculate the heat absorbed (kcal) at 0°C to melt 65 g of ice.
See data on Reference notes (*) at the end of this section.
20.
Calculate the heat released (kcal) at 0°C to freeze 65 g of water.
See data on Reference notes (*) at the end of this section.
21.
Calculate the amount of heat energy (in joules first, then convert to calories):
See data on Reference notes (*) at the end of this section.
a. Gained when 25.0 g water temp rises from 12.5°C to 25.7°C
b. Lost when 75.0 g water cools down from 86.4°C to 2.1°C
c. Absorbed when 5.0 Kg of water warms from 22°C to 28°C?
22. How much heat is required to warm 2.00 liters of water from 25.0 °C to 95.0 °C?
(The density of water is 1.00 g/mL) See data on Reference notes (*) at the end of this section.
(a) 5.86 x 105 kJ
(b) 1.40 x 102 kJ
(c) 3.35 x 101 kJ
(d) 5.86 x 102 kJ
(e) -1.40 x 102 kJ
23. Suppose that 5.00 g of silver is initially at 27.0 °C. What is the final temperature of the sample of silver after
it has absorbed 0.75 Kj of heat? (SHAg = 0.235 J/g.°C)
(a) 938 °C
(b) 665 °C
(c) 27.6 °C
(d) 301 °C
(e) 336 °C
24. What is the temperature change in 355 mL of water upon absorption of 34 kj of heat?
(Note: Assume density of water is 1.00 g/mL) (Note: The specific heat capacity of water is 4.184 J/gºC)
25. A sample of aluminum with a mass of 53.2 g is initially at 155ºC. What’s the temperature of the aluminum
after absorbing 2.87x103 J of heat? (Note: The specific heat capacity of aluminum is SH = 0.903 J/gºC)
26. A chemistry student finds a shiny piece of metal that she suspects is gold. She weights the piece of metal on
the balance and determines that its mass is 14.3g. She then finds that the temperature of this metal rises from
25ºC to 52ºC upon absorption of 174 J of heat. Find the specific heat capacity of this piece of metal and
determine whether the value is consistent with the heat capacity of pure gold. Based on your calculation, can
this piece of metal be pure gold? (Note: The specific heat capacity of gold is 0.129 j/gºC).
27. Calculate the final temperature of 32 mL of ethanol initially at 11ºC upon absorption of 562 J of heat.
(Note: Density of Ethanol is 0.789 g/mL) (Note: The specific heat capacity of Ethanol is SH = 2.42 J/gºC)
28. Calculate the final temperature of 245 mL of water initially at 32ºC upon absorption of 17 kJ of heat.
(Note: The specific heat capacity of water is SH = 4.184 J/gºC) (Note: Assume density of water is 1.00 g/mL)
Notes:
(*) Assume that the following information will always be available, if needed to resolve problems in Chapter 2.
Heat of vaporization, heat of fusion and specific heat capacity values for water.
ΔHvapor(H2O) = 540 cal/g or 2260 J/g
ΔHfusion(H2O) = 80. cal/g or 335 J/g
SH(H2O) = 1.00 cal/g C or 4.184 J/g C
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 3 of 14
Work Assignment I
Chapter 3
Given the following elements: oxygen, fluorine, sodium, silver, krypton and aluminum
1. Write their symbols. Indicate Period number and Group number within the periodic table of elements.
2. Indicate atomic number, average atomic mass and mass number of the most abundant isotope.
3. Indicate number of protons, electrons and neutrons.
4. Classify as Transition or Representative Element. Classify as metal or nonmetal
5. Indicate the number of electronic energy levels (shells).
6. If it is “Representative”, indicate the number of valence electrons (number of electrons located in the
outermost energy level).
7. Identify one alkaline metal, one halogen and one noble gas.
8. What’s the tendency of each of these elements when becoming ions (loosing or gaining electrons?)
9. Indicate in each element whether they tend to form a positive or negative charged ion
10. What’s the relationship between the Energy Levels (shells) and period numbers in the periodic table.
11. Write the electronic arrangement for the elements Na, Ca, B, Al, C, P, S, F and Ar. Indicate how many
valence electrons are in the outer energy level of each atom. Write group and period number.
12. Circle your answer accordingly to indicate the element as follows
F
or
C
 Smallest atomic size:
C or
Si
 Largest atomic size:
O
or
S
 Higher electronegativity:
Cl
or
I
 Higher electronegativity:
P
or
F
 Higher electronegativity:
13. Circle the most electronegative element below:
o Na and Cl
o S and O
o
o C and N
o Si and Cl
o
I and F
Ca and Se
o
o
F and Br
C and O
14. Using the periodic table complete the blank information below:
Name
Group
Symbol number
Period Atomic
number number
Mass
number Average Number
(of most Atomic
of
abundant
mass protons
isotope)
Total
Number
Number number
of
of
of
energy
neutrons electrons levels
Number
of
valence
electrons
Electron
dot
symbol
Lithium
13
Br
2A
4
3
8
6
15. Write the electronic distribution for each of the elements identified in above chart
16. Which group or period is described by the following elements:
a. Contains the elements C, N and O
c. The alkali metals
b. Begins with helium
d. Ends with Neon
17. Give the symbol of the element described by the following:
a. The element located in Group 2 and period 4. The only halogen in period 4.
b. An alkali metal in period 4, a metalloid in period 3, a nonmetal in period 5
c. The transition metal with the highest atomic weight in period 5
d. A noble gas in period 3, a noble gas in period 4, a noble gas in period 1
e. The most electronegative element in group 6, in group 4 and in group 7
f. The largest atomic radius (largest atom) in group 2, the smallest in group 4, the largest in period 4
and the smallest in period 2
g. Only halogen found in liquid state. Only halogen found in solid state. Only two halogens found as
gases. The most electronegative halogen.
h. The only metal found in liquid state at room temperature.
i. The only nonmetal found in liquid state at room temperature
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 4 of 14
Work Assignment I
Chapter 4
1. Write the chemical formula for five compounds:
a) Iron (II) bromide
b) Calcium chloride
c) Beryllium sulfide
d) Aluminum Oxide
e) Copper (II) Oxide
f) Copper (I) Oxide
g) Tin (IV) sulfate
h) Silver nitrate
i) Sodium carbonate
j) Magnesium hydroxide
k) Nickel (II) Oxide
l) Nickel (III) Oxide
m) Barium Fluoride
n)
o)
p)
q)
r)
s)
t)
u)
v)
w)
x)
y)
z)
Carbon disulfide
Carbon monoxide
Sulfur hexafluoride
Silicon dioxide
Dinitrogen monoxide
Carbon dioxide
Hydrogen Sulfide
Phosphorous trichloride
Copper (II) sulfate
Sodium phosphide
Sulfur trioxide
Diboron trioxide
Carbon tetrafluoride
2. Name five of the following compounds:
a) CS2
n) K3P
b) CO2
o) ZnCl2
c) CCl4
p) CrBr3
d) SF6
q) CuS
e) N2O
r) Cu2S
f) HNO3
s) Fe2S3
g) H2SO4
t) CaCO3
h) HCl
u) Al2(SO4)3
i) Cu2S
v) Zn3(PO4)2
j) FeCl3
w) NaHCO3
k) KOH
x) Ca3(PO4)2
l) Mg3N2
y) NH4OH
m) KI
z) KCN
3. Indicate which element is more electronegative in each case and determine if the bonds produced by the
following pairs of atoms are polar covalent, nonpolar covalent or ionic:
a) O and O
b) S and O
c) Na and N
d) Ca and N
e) P and Cl
f) H and H
g) C and O
h) Pb and F
4. Write the Lewis Electron Dot Structure Representation for the following:
a) H2S
e) CO2
i) H2O
m)
b) CCl4
f) O2
j) CS2
n)
c) Cl2
g) N2
k) F2
d) CH4
h) NH3
l) I2
Br2
SiO2
5. Write the name and classify each of the following compounds as molecular or formula unit:
a) FeCl3
b) Na3P
c) BaCl2
d) CO2
e) Zn(NO3)2
f) ZnS
g) NaOH
h) AgCl
i) Na2SO4
j) BaSO4 k) AgNO3
l) NH3 m) Na3PO4 n) Ca(NO3)2
0)
SO3
6. Write formulas for the compounds formed between the following elements and classify the chemical bond as
covalent or ionic:
a) Al & Cl
b) C & H
c) Ca & N
d) Mg & S
e) Si & O
f) S & F
7. Write the formula and ionic charge corresponding to the following polyatomic structures:
a) carbonate
b) bicarbonate
c) Sulfate
d) Nitrate
e) Phosphate
f) Cyanide
8. What is the classification of CaCO3 ?
(1) Atomic Element (2) Molecular Element (3) Molecular Compound
(4) Ionic Compound
9. Which of the following does not exist as a diatomic molecule?
(1) Nitrogen
(2) Bromine
(3) Sulfur
(4) Hydrogen
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 5 of 14
(5) Atomic Compound
(5) Oxygen
Work Assignment I
Chapter 4 Nomenclature Exercise
For the following compounds (You may select 5 random compounds):
a) Indicate whether each is ionic or covalent.
b) If the compound is ionic, show the cation and anion that make up the compound.
c) Write the formula for each compound.
NAME
FORMULA
Nickel (II) Chloride
Calcium fluoride
Tin (II) oxide
Sodium Hydroxide
Lead (II) Sulfate
Magnesium nitrate
Sulfur tetrafluoride
Phosphorus trichloride
Lithium hydroxide
Iron (III) hydroxide
Aluminum chloride
Dinitrogen pentoxide
Silicon tetrachloride
Potassium carbonate
Magnesium hydroxide
Sodium nitrate
Lithium nitride
Strontium chloride
Iron (II) fluoride
Mercury (II) sulfate
Carbon dioxide
Zinc oxide
Dinitrogen monoxide
Sodium carbonate
Potassium bicarbonate
Copper (II) sulfide
Carbon monoxide
Silver nitrate
Ammonium hydroxide
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 6 of 14
IONIC OR
COVALENT?
IF IONIC, WHAT
IS THE CATION?
IF IONIC, WHAT IS
THE ANION?
Work Assignment I
Chapter 5
Kidney stones are solid residues that form in the urinary track. Most kidney stones composition includes calcium
phosphate.
1. Using a Periodic Table:
a) Calculate the molar mass for calcium phosphate.
b) Calculate the number of moles contained in 150 g of calcium phosphate.
2. Calculate the molar mass on each of the following compounds:
C6H12O6, Mg(OH)2, KCl, NaOH, CaCO3,
Al2O3
3. Calculate the mass (in grams) contained in:
a) 2.0 moles MgCl2
b) 1.75 moles Na2O
c) 0.500 moles of NaCl
4. Calculate how many aluminum atoms are contained in a mass of 16.2 g Al (Avogadro number = 6.022 x 10²³)
5. Given a mass of 126.4 grams of glucose C6H12O6 show your calculations to answer the questions below
(Avogadro number 6.022 x 10²³)
a) Molar mass of glucose
b) Number of moles contained in 126.4 grams of glucose
c) Quantity of molecules contained in 126.4 grams of glucose
6. Calculate how many molecules are contained in a mass of 22.5 g CF4 (Avogadro number = 6.022 x 10²³)
7. Determine the number of atoms contained in a 48.3 g sample of zinc (Avogadro number = 6.022 x 10²³)
8. What is the mass of MgCl2 (grams) that would be equivalent to 0.75 moles?
9. Calculate the mass in grams of 1.75 moles of H2O
10. A box contains 737 g NaCl. How many moles of NaCl are present in the box?
11. Calculate the number of moles in 25.0 g of each of the following:
a) O2
b) Al(OH)3
c) Ga2S3
d)
HCl
e)
Ag
f) Na2O
12.
How many moles are in 180.0 g of NaOH?
13.
Balance the following equations. Select the correct coefficients from reactants to products.
__Fe2O3(s)
+ __C(s)
a) 2, 3, 2, 3
b) 2, 3, 4, 3
__Al(s)
+ __FeO(s)
a) 2, 3, 3, 1
b) 2, 1, 1, 1
__Al(s)
+ __H2SO4(aq)
a) 3, 2, 1, 2
b) 2, 3, 1, 3
__Fe(s)
+ __CO2(g)
c) 1, 1, 2, 3
__Fe(s)
+ __Al2O3(s)
c) 3, 3, 3, 1
__Al2(SO4)3(aq) + __H2(g)
c) 2, 3, 2, 3
14. Identify each reaction as combination, decomposition, combustion, single replacement, double replacement
or neutralization:
3Ba(s)
+
N2(g)
2Ag(s) + H2S(aq)
2C2H6(g)
+ 7O2(g)
Ba3N2(s)
Ag2S(s) + H2(g)
4CO2(g) + 6H2O(g) + Heat
PbCl2(aq) + K2SO4(aq)
2KCl(aq) + PbSO4(s)
K2CO3(s)
K2O(aq) + CO2(g)
+
Heat
Al(OH)3(aq) + 3HCl(aq)
AlCl3(aq) + 3H2O(l)
15. Balance the following chemical equations:
a) Mg(OH)2 + HCl
b) Al(OH)3 + HCl
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 7 of 14
MgCl2 + H2O
AlCl3 + H2O
Work Assignment I
16. Based on the above chemical equation, how many moles of aluminum hydroxide would be required to react
with 6 moles of hydrochloric acid?
17. Based on the above chemical equation, how many moles of magnesium hydroxide would be required to react
with 6 moles of hydrochloric acid?
18. A patient was administered a 3.0 g dosage of magnesium hydroxide antacid. How many moles of
hydrochloric acid should have been neutralized at the end of this dosage?
19. Calculate the molar mass of the following compounds:
a) Aluminum Oxide
b) Sodium hydroxide
c) Potassium Carbonate
d) Iron II Sulfate
e) Sulfur trioxide
f) Carbon tetrachloride
20. Calculate the mass in grams in each of the following:
a) 2.5 moles of MgCl2
b) 0.488 mole of C6H12O6
22. How many grams of O2 are needed to produce 45.8 grams of Fe2O3 in the following reaction?
4Fe(s) + 3O2(g)
2Fe2O3(s)
23. How many moles of Fe2O3 can form from 6.0 moles of O2? (Based on above equation)
24. How many moles of Fe are consumed in a reaction with 12.0 moles of O2? (Based on above equation)
25. Classify each equation as combination or decomposition and identify each as exothermic or endothermic
reaction:
A. N2(g) + 3H2(g)
2NH3(g) + 22 kcal
B. CaCO3(s) + 133 kcal
CaO(s) + CO2(g)
C. 2SO2(g) + O2(g)
2SO3(g) + heat
26. Calculate the mass (g) of NH3 that can be produced from 32 grams of N2.
N2(g) + 3H2(g)
2NH3(g)
28. State the effect that each factor below may have on the rate of a chemical reaction
(Write your answer as: increases, decreases, or has no effect):
A. increasing the temperature
B. removing some of the reactants
C. adding a catalyst
D. placing the reaction flask in ice
E. increasing the concentration of one of the reactants
F. using a glass rod to mix the liquid reactants
29. Calculate how much Iron (III) Sulfide (in grams) can be formed with 223.4 grams of iron based on the
following equation:
2Fe(s) + 3S(s)
Fe2S3(s)
30. Determine how much sulfur (in grams) will be required (based on above equation) for the reaction with
223.4 grams of iron
31. What are the products of a general acid-base reaction? Circle one
(1) Different acids and bases
(2) Water and ammonia
(3) Water and carbon dioxide
(4) Water and hydrogen gas
(5) Water and a salt
32. A pure titanium cube has an edge length of 0.973 ft. How many titanium atoms does it contain?
(Density of Titanium is 4.50 g/cm3).
(1) 1.22 x 1024 atoms
(2) 2.00 x 1025 atoms
(3) 1.48 x 1027 atoms
22
26
(4) 5.21x 10 atoms
(5) 3.46 x 10 atoms
(6) Insufficient information
24
33. What is the mass of 4.78 x10 molecules of NO2?
34. Calculate the number of moles of sulfur in 57.8g of sulfur.
35. How many atoms are in 107.87 g of silver?
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 8 of 14
Work Assignment I
Chapter 6
1. A sample of Helium gas has a volume of 150 ml at 750 Torr. If the volume expands to 450 ml at constant
temp, what’s the new pressure in Torr?
2. A sample of Neon gas has a volume of 5.40 L and a temp of 15ºC. Find the new volume of the gas after
the temp has been increased to 42ºC at constant pressure.
3. A balloon contains 2500 ml of helium gas at 75°C. What is the new volume of gas (assume that n and P
remain constant) when the temp changes to the following values?
a) 55°C b) 680 K
c) -25°C d) 240 K
4. In a storage area where the temp has reached 55°C the pressure of oxygen gas in a 15.0 L steel cylinder is
965 torr. To what temp would the gas have to be cooled to reduce the pressure to 850. torr?
5. An aerosol can has a pressure of 1.40 atm at 12°C. What’s the final pressure of the aerosol can if it is kept
in a room where the temp is 35°C?
6. A sample of Nitrogen gas has a volume of 50.0 L at a pressure of 760.0 mm Hg. What is the volume of the
gas at each of the following pressures if there is no change in temp?
a) 1500 mm Hg
b) 2.0 atm
c) 0.500 atm
d) 35 psi
7. A sample of helium gas has a volume of 6.50 L at a pressure of 845 mm Hg and a temp of 25°C. What’s
the pressure of the gas in atm when the volume and temp of the gas sample are changed to the following?
a) 1850 ml, 325 K
b) 0.55 atm, 75°C
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 9 of 14
Work Assignment I
Chapter 7
1. Show the correct link to describe the type of solution:
 Sugar completely dissolves when
 Unsaturated solution
added to hot coffee
 A layer of sugar forms on the
bottom of a glass of iced tea
 Sodium chloride crystals do not
 Saturated solution
dissolve in solution
2. Show the correct link to the experimental conditions on the right:
 Copper ions can pass through a semi-permeable membrane while
Supersaturated
starch colloidal particles are held back
 When a few crystals of potassium permanganate were added to an
undisturbed water sample, it shows a purple coloration slowly
Dialysis
expanding through water.
 Water molecules pass through a semi-permeable tissue membrane
Diffusion
from a 0.89% salt solution to a 10% salt solution
 Solution in which addition of sodium chloride crystallizes
Osmosis
3. Using your text book write a brief definition of “solution”, “colloid”, “suspension”.
4. Provide a brief experimental example of a mixture where diffusion takes place.
5. Provide an example of a mixture that represents a permanent emulsion.
6. Explain what the differences between osmosis and dialysis are.
7. Why does iodine dissolve in hexane, but not in water?
8. Why does iodine dissolve in hexane, but not in water?
9. What’s the molarity of a solution containing 15.6 g of KCl in 274 ml?
10. A solution is prepared with 70.0 g of HNO3 and 130 g H2O. It has a density of 1.21 g/ml.
a. Identify the solute and the solvent used on this solution.
b. What’s the mass % of the HNO3 solution?
c. What’s the total volume of the solution?
d. What’s the mass/volume percent?
e. What’s the molarity (M)?
11. Assuming that 15.51 g of NaCl is completely dissolved in 500 ml water at 100º F. What would be the molarity
(M) of NaCl in this solution?
12. How many liters of 5.0% (m/v) glucose solution would be required to administer a total of 75 g glucose?
13. If you were in the laboratory, how would you prepare 1.00 L of a 0.50 M KCl solution?
14. What is the molarity (M) of the solution if 180.0 g of NaOH is dissolved in 2,000 ml of water?
15. What is the molarity (M) of the solution if 40.91 g of NaCl is dissolved in 500 ml water?
16. Calculate the grams of solute needed to prepare each of the following solutions:
a) 2.0 liter of a 1.5 M NaOH solution
b) 1.5 liter of a 0.20 M KCl solution
c) 0.75 liter of a 6.0 M HCl solution
17. What’s the molarity (M) of 60.0 g of NaOH in 0.250 liter of solution?
18. What’s the mass percent of a solution prepared by dissolving 30.0 g of NaOH in 120.0 g of H2O ?
19. What’s the mass/volume percent (% m/v) of bromine (Br2) in a solution prepared by dissolving 12 g of
bromine in enough carbon tetrachloride to make 250 ml of this solution?
20. A solution is prepared by mixing 15.0 g of Na2CO3 and 235 g of H2O. Calculate the mass percent (% m/m)
of the solution.
21. What is the molarity of 0.225 L of a KNO3 solution containing 34.8 g of KNO3?
22. How many grams of AlCl3 are needed to prepare 125 mL of a 0.150 M solution?
23. Calculate the molarity of 15.2 mg KI in 102 mL of solution.
(a) 8.98 x 10-7 M
(b) 1.49 x 10-4 M
(c) 0.898 M
(d) 8.98 x 10-4 M
(e) 1.49 x 10-7 M
24. A chemist wants to make 5500 mL of a 0.300 M CaCl2. What mass (in g) of CaCl2 should the chemist use?
(a) 1.8 x 102 g
(b) 2.0 x 106 g
(c) 1.8 x 105 g
(d) 1.5 x 10-2 g
(e) 2.0 x 103 g
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 10 of 14
Work Assignment I
25. An isotonic solution exerts the same osmotic pressure as body fluids (between red blood cells and their
surrounding environment). Solutions of 5.0% (m/v) glucose or 0.90% (m/v) NaCl are typical isotonic
solutions Indicate if each of the following solutions is: A) isotonic B) hypotonic C) hypertonic
1. ____ 2% NaCl solution
2. ____ 1% glucose solution
3. ____ 0.5% NaCl solution
4. ____ 5% glucose solution
26. Indicate if each statement below is True or False:
(a) In an isotonic solution, a red blood cell retains its normal volume ________
(b) Hemolysis: In a hypotonic solution, water flows into a red blood cell by osmosis,
causing it to swell and burst ________
(c) Crenation: In a hypertonic solution, water goes out of the red blood cell by osmosis,
causing it to shrink ________
27. When placed in each of the following solutions, indicate if a red blood cell:
A) will not change
B) will undergo hemolysis
C) will undergo crenation
1.____ 5% glucose solution
2.____ 1% glucose solution
3.____ 0.5% NaCl solution
4.____ 2% NaCl solution
28. Show the correct link according to description shown on the right:
 Small molecules and ions pass through a semi-permeable
Solubility
membrane while large macromolecules are held back
 Heterogeneous mixture with very large and heavy particles that
Diffusion
tend to settle down on the bottom of the container.
 Maximum amount of solute that can be dissolved in a given
Suspension
amount of solvent
 When a few crystals of potassium permanganate are added to an
undisturbed water sample, it shows a purple coloration slowly
Osmosis
expanding through water.
 A homogeneous mixture where the solute is made up of very
Dialysis
small size molecules or ions.
 Passage of water molecules through a semi-permeable
Solution
membrane from a solution containing a lower salt concentration
to a solution containing a higher salt concentration
29. Indicate the correct answer below:
a) solution
b) colloid
c) suspension
1) A mixture that has solute particles that do not settle out but are too large to pass through a
semipermeable membrane is called a ________________
2) A transparent mixture that has very small solute particles, ions or molecules that do not separate,
cannot be filtered out and pass through semipermeable membranes is called a _______________
3) A mixture that has have very large particles, settle out on the bottom of the container, can be filtered
and must be stirred to stay suspended is called a __________________
30. Calculate the molarity of a solution prepared by dissolving 180g of NaOH in 2000. ml of water.
31. What is the mass in grams of NaCl needed to prepare 0.50 L of a 0.20 M solution?
32. What is the % (v/v) of a solution prepared by adding 250 mL ethanol to 1.0 liter of water?
33. The density of a 40.0% by mass ethylene glycol (C2H6O2) solution in water is 1.11 g/mL.
Find the molarity of the solution.
34. (Part 1) If 3.5 liters of a 1.1 M CaCl2 aqueous solution is diluted by adding 500.0 mL of water, what is the
molarity of the diluted solution?
(Part 2) If 3.5 liters of a 1.1 M CaCl2 aqueous solution is slowly evaporated by heat until a final volume of
500.0 mL is obtained, what is the molarity of the resulting solution?
Circle your answers:
(a) 3.5 M
(b) 0.96 M
(c) 4.0 M
(d) 1.9 M
(e) 7.7 M
35. If 0.123 L of a 1.6 M fructose solution is diluted to 428.0 mL, what is the molarity of the diluted solution?
(a) 0.46 M
(b) 5570.0 M
(c) 5.57 M
(d) 3.92 M
(e) 0.00046 M
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 11 of 14
Work Assignment I
Chapter 8
1. The following chemical equations include antacid formulations which are used to neutralize
excess stomach acid:
a)
b)
c)
d)
e)
Mg(OH)2 +
CaCO3 +
NaHCO3 +
KHCO3 +
Al(OH)3 +
HCl
HCl
HCl
HCl
HCl
MgCl2 + H2O
CaCl2 + H2O + CO2
NaCl + H2O + CO2
KCl + H2O + CO2
AlCl3 + H2O
a. Write the appropriate coefficients to balance each of the above equations.
b. Identify the acid and the base within some of the above reactants
2. Given the following neutralization reactions:
a) Al(OH)3 + HNO3
b) LiOH +
c) Ca(OH)2 + H3PO4
d)
+ HCl
+ H2O
Li2SO4 + H2O
Ca3(PO4)2 +
NaCl + H2O
a. Fill the appropriate chemical formulation in each blank square
b. Write the name of each of the reactants and products.
3. Indicate if each of the following characteristics corresponds to an acid or base:
a) Sour taste
b) Produces H+ ions in water
c) Neutralizes bases
d) Potassium hydroxide
e) Neutralizes acids
f) Soapy feel
g) Produces OH- ions in water
h) Turns litmus red
i) pH measures 4.8
4. Write the chemical formula of the following compounds and classify them as acid or base:
a) Magnesium hydroxide
b) Aluminum hydroxide
c) Hydrochloric acid
d) Sulfuric acid
e) Nitric acid
f) Calcium hydroxide
g) Potassium hydroxide
h) Phosphoric acid
i) Sodium hydroxide
j) Boric acid
5. Explain briefly the main difference between a “weak” and a “strong” acid.
6. Is gastric “juice” acidic, basic or neutral? What color should Gastric juice turn litmus paper?
7. Is Mylanta antacid acidic, basic or neutral? What color should hydroxides turn litmus paper?
8. For a substance to be considered an acid or a basic, what should the pH value be in each case?
(pH above 7, pH below 7)
9. Regarding buffer solutions:
a) Briefly explain how is a buffer solution made
b) What is the purpose of the buffer system
c) Provide an example of a chemical buffer system in human blood
10. State whether each of the following solutions is acidic, basic or neutral:
a) blood, pH 7.38
b) drain cleaner, pH 11.2
c) Vinegar, pH 2.8
d) Coffee, pH 5.5
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 12 of 14
Work Assignment I
11. Determine the pH for the following solutions:
a) [H3O+] = 0.000010 M
b) [H3O+] = 0.00000005 M
12. Write the conjugate base of each of the following:
A.
HBr
B.
H2S
C.
H2CO3
13. Write the conjugate acid of each of the following:
A.
NO2
B.
NH3
C. OH
14. The conjugate base of HCO3 is a) CO32
b) HCO3
c) H2CO3

2
15. The conjugate acid of HCO3 is a) CO3
b) HCO3
c) H2CO3

16. The conjugate base of H2O is
a) OH
b) H2O
c) H3O+
17. The conjugate acid of H2O is
a) OH
b) H2O
c) H3O+

2
18. The [OH ] of an ammonia solution is 4.0  10 M. What is the [H3O+] of the solution?
19. If lemon juice has [H3O+] of 2  103 M, what is the [OH] of the solution?
20. What is the [H3O+] of a solution if [OH] is 5.0  108 M?
21. Find the pH of a solution with a [H3O+] of 1.0  103
22. Determine the pH of a solution with a [OH] = 3  1010
23. Determine the pH of a solution with a [H3O+] = 5  1012
24. Determine the pH of a solution with a [OH-] = 1  109
25. Determine the pH of a solution with a [H3O+] = 1  108
26. What is the pH of coffee if the [H3O+] is 1  105 M?
27. The [H3O+] of tomato juice is 2  104 M. What is the pH of the solution?
28. Select the correct set of coefficients for each of the following neutralization equations:
A)
HCl(aq) + Al(OH)3(aq)
a) 1, 3, 3, 1
AlCl3(aq) + H2O(l)
b) 3, 1, 1, 1
c) 3, 1, 1, 3
B)
Ba(OH)2(aq) + H3PO4(aq)
a) 3, 2, 2, 2
Ba3(PO4)2(s) + H2O(l)
b) 3, 2, 1, 6
c) 2, 3, 1, 6
29. A buffer consists of a weak acid and its conjugate base. Which of the following combinations make a
buffer solution?
a) HCl and Cl 
b) H2CO3 and HCO3
c) H3PO4 and NaCl
d) CH3COOH and CH3COO
30. Identify each solution as acidic, basic, or neutral:
A. ___ HCl with a pH = 1.5
B. ___ pancreatic fluid, [H3O+] = 1  108 M
C. ___ Sprite soft drink, pH = 3.0
D. ___ pH = 7.0
31. Indicate if each statement below is true or false
a) A buffered solution shows minimum or no pH change when acid is added
b) The pH of a HCl solution with a 0.050 M acid concentration is 1.3
c) Strong bases dissociate 100% in water releasing OH (-) Hydroxide ions
d) A solution with a pH = 9.0 is considered a basic solution
e) The higher the pH value, the higher the acid concentration in solution
f) A solution of Mg(OH)2 is considered an acid solution
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 13 of 14
Work Assignment I
Chapter 9
1. Show the correct link to describe the type of nuclear radiation:
 Alpha emission



 Beta emission





Gamma
emission





Positron
emission






Represented by Symbol β
High energy emission that can travel great distances through the air and
can penetrate body tissues.
They travel only short centimeters distance (paper or clothing shielding is
OK for protection)
Similar than an electron with mass=0, except charge is +1
Heavy clothes, lab coats and gloves needed for shield protection.
Mass number 4, charge = +2
Produced by an unstable nucleus when a neutron is transformed into a
proton and an electron
These are the heaviest radiation particles (2 protons + 2 neutrons).
Heavy dense leaded shield protection required.
Represented by symbol α
Produced by an unstable nucleus when a proton is transformed into a
neutron and a positron
Represented by symbol β+
Mass=0, charge = -1
High energy electron particle radiation that can penetrate body tissues.
mass=0, charge =0
Formed by collision between electron and positron particles
Represented by symbol γ
2. Complete each of the following nuclear equations:
a) 241/95Am --------> ? + 4/2He
b) 60/27Co ---------> ? + 0/-1e
c) 66/30Zn + 1/1H--------> ?
d) 28/13Al ---------> ? + 0/1e
e) ? ----------> 86/36Kr + 1/0n
f) 66/29Cu --------> 66/30Zn + ?
Professor Ralph Duarte
CHM1033 Chemistry for Health Sciences
Page 14 of 14