UNIT 7 | STUDY GUIDE
LIQUIDS, SOLIDS, AND SOLUTIONS
liquids and solids
answers to selected problems
12-1, 12-2 | Section Reviews
Chapter 13 Review:
kinetic molecular theory of liquids
properties of liquids
kinetic molecular theory of solids
properties of solids
phase changes
solutions
13-1, 13-2, 13-3, 14-2 | Section Reviews
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solute & solvent
suspension
colloid
solution
electrolytes vs. nonelectrolytes
miscible vs. immiscible
gas solubility
o Henry’s Law
rate of dissolution
solubility values & solubility curves
unsaturated, saturated, supersaturated
solution concentrations
o molality
o molarity
dilutions
colligative properties
o vapor pressure
o boiling point
o boiling point elevation
o freezing point depression
solution stoichiometry
Chapter 13 Review: 1, 2, 4, 5, 6, 7, 8, 9, 11, 13,
14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25,
26, 27, 28, 30, 31, 33
Chapter 14 Review: 8, 11, 13, 19, 20, 21, 22, 25,
26, 42
Solubility of AgNO₃
grams solute per 100 g H₂O
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800
700
600
500
400
300
200
100
0
y = 6.3329x + 73.967
0
20
40
60
80
100
120
temperature (°C)
13) a: increases // b:
549 g
100 g H2 O
296 g
100 g H2 O
,
422 g
100 g H2 O
,
// c: 32°C // d: unsaturated,
saturated with 29 g undissolved
14) 74 g KNO3
15) a: (1) convert grams NaOH to moles
NaOH (2) 39.997 g/mol (3) 0.167 M
NaOH // b: 0.953 M NH4Br
16) a: (1) sulfuric acid, H2SO4 (2) water, H2O
(3) 343 g H2SO4 // b: 1140 g Ba(NO3)2
17) 0.143 mol NaOH
18) a: 132.140 g/mol // b: NH41+, SO42- //
c: 3.999 M (NH4)2SO4
19) a: convert grams AgNO3 to moles AgNO3
// b: 169.872 g/mol // c: 1000 mL soln
20) a: 2, 3, 1, 6 // b: 700 g Ca3(PO4)2,
240 g H2O
21) 52.1 mL
22) 0.0309 M AgNO3
23) a: (1) sulfuric acid, H2SO4 (2) water, H2O
(3) 3.001 m H2SO4 // b: 4.00 m HNO3
24) a: 441 g H2SO4 // b: 126 g HNO3
25) a: 342.297 g/mol // b: 0.182 m
C12H22O11
26) 0.920 kg H2O 27) 20.2 g C2H5OH
28) a: 142.042 g/mol // b: 0.113 M Na2SO4
30) a: 74.551 g/mol // b: mass of KCl would
be unaffected // c: 160 g KCl
31) a: 39.997 g/mol // b: 2 Na + 2 H2O →
2 NaOH + 1 H2 // c: 0.250 M NaOH
33) Table 1: 1 – solution, 2 – suspension,
3 – colloid, 4 – colloid // Table 2:
1 – solution, 2 – colloid, 3 – colloid,
4 – solution
CHEMISTRY MYP | KHAN
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UNIT 7 | STUDY GUIDE
LIQUIDS, SOLIDS, AND SOLUTIONS
Chapter 14 Review
13) a: 1 KI → 1 K1+ + 1 I1- // b: 1 NaNO3 → 1 Na1+ + 1 NO31- // c: 1 MgCl2 → 1 Mg2+ + 2 Cl1- //
d: 1 Na2SO4 → 2 Na1+ + 1 SO4219) a: -2.79°C // b: -0.929°C // c: -1.05°C
21) a: -0.826°C // b: -0.826°C
25) a: 1.3°C // b: 0.00906°C //c: 0.0596°C
42) 101.79°C
20) a: 0.500 m // b: 2.00 m // c: 4.50 m
22) 334 g C2H4(OH)2
26) a: 0.49 m // b: 3.00 m // c: 5.500 m
Solution Stoichiometry
1) How many milliliters of 0.200 M phosphoric acid, H3PO4, are needed to react with 100. mL of 0.100
M sodium hydroxide if the products are sodium phosphate and water?
2) Phosphoric acid, H3PO4, reacts with sodium hydroxide to produce sodium phosphate and water. If
36.0 mL of phosphoric acid react with exactly 80.0 mL of 0.500 M sodium hydroxide, what is the
molarity of the phosphoric acid?
3) Iron metal reacts with aqueous gold(III) nitrate through single replacement to produce iron(II) nitrate
and gold metal. How many liters of 0.500 M of gold(III) nitrate react with 224 grams of iron metal?
4) How many milliliters of 18.0 M sulfuric acid, H2SO4, are required to react with 250. mL of 2.50 M
aluminum hydroxide if the products are aluminum sulfate and water?
5) 75.0 mL of a silver(I) nitrate solution react with enough copper metal to produce 0.250 g of silver
metal by single replacement. What is the molarity of the initial silver(I) nitrate solution if copper(II)
nitrate is the other product?
6) What mass of each product results if 750. mL of 6.00 M phosphoric acid, H3PO4, react with excess
calcium hydroxide if the products are calcium phosphate and water?
7) Calcium carbonate reacts with hydrochloric acid, HCl, to yield calcium chloride, carbon dioxide, and
water. What volume, in liters, of 0.80 M hydrochloric acid is needed to react with 4.0 grams of
calcium carbonate?
8) Vinegar that is 5.00% acetic acid, HC2H3O2, has a molarity of 0.873 M. Baking soda is sodium
bicarbonate. These two chemicals react to produce sodium acetate, carbon dioxide, and water. If
30.0 mL of vinegar react with 5.00 g of baking soda, what is the limiting reactant? How many grams
of carbon dioxide are produced?
9) When 25 mL of 4.0 M HCl is used to produce hydrogen gas, how many grams of zinc does it react
with through single replacement? What volume of hydrogen gas is produced at standard
temperature and pressure?
10) Sea water is about 0.500 M sodium chloride. To produce chlorine gas, a company evaporates sea
water, melts the sodium chloride, and runs electricity through it to produce elemental sodium and
chlorine gas. How many liters of sea water are needed to fill a tank car with 1,120,000 liters of
chlorine gas at standard temperature and pressure?
answers: 1) 16.7 mL H3PO4 // 2) 0.370 M H3PO4 // 3) 5.35 L Au(NO3)3 // 4) 52.1 mL H2SO4 //
5) 0.0309 M AgNO3 // 6) 698 g Ca3(PO4)2 and 243 g H2O // 7) 0.10 L HCl // 8) vinegar is the
limiting reactant; 1.15 g CO2 are produced // 9) 3.3 g Zn; 1.1 L H2 // 10) 2.00 x 105 L sea water
CHEMISTRY MYP | KHAN
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