Honors Chemistry – Chapter 15 and 16 Review Packet
Name: _____________________________
Chapter 15 and 16: Water and Solutions
Section 1: Properties of Solutions
1. Define the following:
a. Solute the substance being dissolved
b. Solvent the substance doing the dissolving
c. Solvation the process of dissolving
2. What are the four factors that affect solution formation? How and why do they have an effect?
a. Composition of solute and solvent – polarity and attraction
b. Stirring – agitating the particles for more contact
c. Temperature – increased temp = increased kinetic energy = increased collisions = dissolve
d. Surface Area – increased surface area means more area for interaction/collisions
3. Dissolving involves an exchange process between two processes: Solvation and Crystallization
4. What are the three types of solutions and how are they different?
a. Unsaturated – less than maximum amount of solute
b. Saturated – maximum amount of solute
c. Supersaturated – more than maximum amount of solute
5. Oil and water are examples of two miscible
immiscible liquids. (Circle one)
6. Temperature increases the solubility of solids and decreases the solubility of gases.
7. How does pressure affect the solubility of solids? Of gases? No effect on solids, increase pressure to
increase gas solubility
8. What is Henry’s law? S1 / P1 = S2 / P2
9. The solubility of a gas at 12 atm is 1.23 g/L. What is the solubility of this gas at 5 atm? 0.513 g/L
10. The solubility of a gas at 740 mmHg is 0.97 g/L. What pressure produces a solubility of 2.1 g/L? 1602
mmHg
11. What is the general solubility rule? Like dissolves like
Honors Chemistry – Chapter 15 and 16 Review Packet Name: _____________________________
12. Use the solubility curve to answer the questions below:
a. Determine the solubility of the following substances:
i. SO2 at 40˚C in 100 g of water 5g
ii. NH3 at 90˚C in 100 g of water 10 g
b. Determine how much undissolved solute is present in each of the following:
i. 110 g NaNO3 at 10˚C in 100 g of water 30 g
ii. 140 g KNO3 at 50˚C in 100 g of water 55 g
iii. 60 g NaCl at 0˚C in 100 g of water 22 g
c. Which of the substances on the chart are likely gases? HCl, NH3, SO2
Section 2: Concentrations of Solutions
1. Molarity = moles solute / liters solution Unit: M (Molar)
2. How many grams of potassium nitrate are required to prepare 0.250 L of a 0.700 M solution? 17.6 g
Honors Chemistry – Chapter 15 and 16 Review Packet Name: _____________________________
3. What is the molarity of a solution of HNO3 that contains 12.6 g of nitric acid in 1.0 L of solution? 0.2 M
4. How many moles of sucrose are dissolved in 250 mL of solution if the concentration is 0.150 M? 0.038
mol
5. To make 1249 mL of a 4.00 M solution, how many moles of solute will be needed? 4.996 mol
6. How many liters of solution can be produced from 2.5 moles of solute if s 2.0 M solution is needed?
1.25 L
7. What is the concentration of a solution with a volume of 2.5 L containing 660 g of calcium phosphate?
0.8516 M
8. How would you prepare 250 mL of 0.67 M AlBr3 from a stock solution with a concentration of 5 M?
(Provide the volume of stock solution and the volume of water required). 33.5 mL stock, 216.5 mL
water
9. How would you prepare a 1.2 L solution of 3 M HCl from a stock solution with a concentration of 18
M? (Provide the volume of stock solution and the volume of water required). 0.2 L stock, 1.0 L water
10. What is the (%v/v) ethanol in a mixture containing 42 mL of ethanol in a 652 mL solution? 6.44%
11. What is the (%m/m) baking soda (sodium hydrogen carbonate) in a mixture containing 2.3 moles of
baking soda in a 510 g solution? 37.9%
Section 3 and 4: Colligative Properties
1. Molality = moles solute / kg solvent Unit: m (Molal)
2. How many grams of AgNO3 are needed to prepare a 0.125 m solution in 250 grams of water? 5.31 g
3. What mass in grams of sucrose, C6H12O6, must be dissolved in 2000 grams of water to make a 0.1 molal
solution? 36 g
4. Determine the molality (m) of a solution containing 42 grams of glycerin, C3H5(OH)3 in 750 grams of
water. 0.609 m
5. A solution contains 85.0 grams of methanol, CH3OH, in 3000 grams of water. Calculate the molality of
the solution. 0.8867 m
6. Calculate the mole fraction of each component of a solution containing 1.89 moles of lithium hydroxide
dissolved in 7.21 moles of water. LiOH = 0.208 and water = 0.792
7. Calculate the mole fraction of each component of a solution containing 10 g of lithium dissolved in 19 g
of hydrobromic acid. Li = 0.859 and HBr = 0.140
8. What does a colligative property depend on? Number of particles
9. Vapor Pressure Lowering
a. Summary: The more solute particles you have, the lower the vapor pressure.
b. Why? Solvent particles have to overcome attractive forces of other solvent particles and
new solute particles, it is harder to overcome and become a gas
c. Assume each of the solutions below contains 1 mole of solute in 1 L of solution. Which solution
in each group would have the lowest vapor pressure? (Circle one)
i.
NaCl
CaCl2
ii.
Aluminum bromide
Ammonia
iii.
Pure water (no solute)
Glucose
iv.
Aluminum sulfate
Barium carbonate
Lithium hydroxide
Honors Chemistry – Chapter 15 and 16 Review Packet Name: _____________________________
10. Boiling Point Elevation
a. Summary: The more solute particles you have, the higher the boiling point.
b. Why? Solvent particles entering the gas phase must overcome attractions from solvent and
new solute particles, which requires more energy – thus a higher temperature to boil.
c. Assume each of the solutions below contains 1 mole of solute in 1 L of solution. Which solution
in each group would have the highest boiling pressure? (Circle one)
i.
Magnesium oxide
Barium chloride
ii.
Lead (IV) sulfide
Aluminum phosphide
11. Freezing Point Depression
a. Summary: The more solute particles you have, the lower the freezing point.
b. Why? Solute particles interrupt crystal formation and more energy must be given off in
order to freeze, therefore the freezing point is lower.
c. Assume each of the solutions below contains 1 mole of solute in 1 L of solution. Which solution
in each group would have the lowest freezing point? (Circle one)
i.
Lithium oxide
Barium oxide
ii.
Rubidium nitrate Magnesium acetate
Aluminum oxide
12. A solution contains 15 grams of sucrose, C12H22O11, in 250 grams of water. What is the freezing point
and boiling point of the solution? FP = -0.326 C and BP = 100.0898 C
13. Calculate the boiling point and freezing point of a solution that contains 3.0 grams of sodium acetate,
NaC2H3O2, dissolved in 250 grams of water. FP = -0.5952 C
14. Calculate the freezing point of a solution containing 5.70 grams of sugar, C12H22O11, in 50 grams of
water. FP = -0.62 C
15. Calculate the boiling point of a solution containing 60.0 grams of NaOH in 500 grams of water.
BP = 103.072C
16. How many grams of glucose, C6H12O6, must be dissolved in 500 grams of water to lower the freezing
point to -6.51oC? 315 g