1. Solutions Review
Chemistry

2. Which of the following operation usually makes a substance dissolve faster in a solvent?
agitation
raising the temperature
crushing the substance into a powder
all of the above.

3. boiling point elevation molarity molality freezing point depression
Which of the following is a colligative property that explains why ice will form at higher temperatures in the Great Lakes than in the ocean.
boiling point elevation
molarity
molality
freezing point depression
mole fraction

4. What is the number of moles of solute in 250 mL of 0.4 M of solution?
A) 0.1 mol C) 0.16 mol B) 0.62 mole D) 1.6 mol E) 1 mol

5. Pressure has and influence on the solubility of:
A) liquids dissolving in liquids B) solids & liquids dissolving in liquids. C) gases dissolving in liquids. D) solids dissolving in liquids

6. Colligative properties of solutions depend on:
A) size of the solute particles. B) molecular nature of the solute particles C) charge of the solute particles. D) the number of solute particles

7. What is the maximum amount of KCl that can dissolve in 200 g of water?
(The solubility of KCl is 34 g/100 g H2O at 20C.)
a. 17 g c. 68 g
b. 34 g d g

8. Which of the following pairs of factors affects the solubility of a particular substance?
a. particle size and degree of mixing
b. temperature and degree of mixing
c. temperature and the nature of solute and solvent
d. particle size and temperature

9. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.
a. unsaturated c. an emulsion
b. saturated d. supersaturated

10. Which of the following substances is less soluble in hot water than in cold water?
a. CO2(g) c. NaNO3(s)
b. NaCl(s) d. KBr(s)

11. Which of the following occurs to most solids. as temperature increases
Which of the following occurs to most solids as temperature increases? a. Solubility decreases.
b. Solubility increases.
c. Solubility remains the same.
d. Molarity doubles.

12. In a concentrated solution there is ____.
a. no solvent c. a small amount of solute
b. no solute d. a large amount of solute

13. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
a. 6M c. 7M
b. 12M d. 3M

14. Which of the following operations yields the number of moles of solute?
molarity x moles of solution
molarity x mass of solution
molarity x liters of solution
d. moles of solution x volume of solution

15. What mass of sucrose, C12H22O11, is needed to make 500. 0 mL of a 0
What mass of sucrose, C12H22O11, is needed to make mL of a 0.200M solution?
a g c g
b. 100 g d g

17. How many mL of a 2. 0M NaBr solution are needed to make 200. 0 mL of 0
How many mL of a 2.0M NaBr solution are needed to make mL of 0.50M NaBr?
a. 25 mL c. 100 mL
b. 50. mL d. 150 mL

18. If 2. 0 mL of 6. 0M HCl is used to make a 500
If 2.0 mL of 6.0M HCl is used to make a mL aqueous solution, what is the molarity of the dilute solution?
a M c. 0.30M
b. 0.24M d. 0.83M

19. If the percent mass of solute for a solution is 4% and the mass of the solution is 200 g, what is the mass of solute in solution?
a. 8.0 g c. 80 g
b. 50 g d. 800 g

20. Which of the following is NOT a colligative property of a solution?
boiling point elevation
vapor pressure lowering
supersaturation
freezing point depression

21. What is the mole fraction of ethanol in a solution of 3
What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
a c. 1.67
b d. 15

22. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)
a. 0.67m c. 1.7m
b. 4.0m d. 0.17m

23. What is the number of kilograms of solvent in a 0
What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar mass of solute = 30 g)
a kg c kg
b. 2.4 kg d. 1.1 kg

24. To which of the following variables is change in boiling point directly proportional?
molarity of solution
percent by volume of solution
molality of solution
percent (mass/mass) of solution

25. The freezing point of a solution that contains 0
The freezing point of a solution that contains mol moles of NaI in 615 g of water is ____. (kf = 1.86C/m; molar mass of water = 18.0 g)
a. 1.66C c. 3.33C
b C d C

26. What is the boiling point of a solution that contains 3
What is the boiling point of a solution that contains 3.00 moles of KBr in mL of water? (kb = 0.512C/m; molar mass of water = 18.0 g)
a. 97.0C c C
b. 99.7C d C

27. a. 15.0 g/mol c. 150. g/mol b. 30.0 g/mol d. 300. g/mol
What is the approximate molar mass of a molecular solute if 300. g of the solute in g of water causes the solution to have a boiling point of 101C?
(kb = 0.512C/m; kf = 1.86C/m; molar mass of water = 18.0 g)
a g/mol c g/mol
b g/mol d g/mol