For each question, choose answer "e" if no correct answer is found.

MULTIPLE CHOICE

1. In a solution, the solvent is:
a) the substance being dissolved
b) always a liquid
c) the substance present in the greatest amount
d) always water

2. In a solution, solutes:
a) must be liquids
b) can be liquids or gases
c) cannot be solids
d) can be solids, liquids or gases

3. A solution is always characterized by each of the following except one. The
exception is:

a) homogeneity
b) variable composition
c) absence of settling
d) liquid state

4. A crystal of solid NaCl is placed into an aqueous NaCl solution. It is observed
that most, but not all, of the crystal dissolves. The original solution was

a) unstable
b) unsaturated
c) slightly saturated
d) saturated

5. Which type of compound is not likely to dissolve in water?

a) one with hydrogen bonds
b) a nonpolar compound
c) a salt
d) a highly polar compound

6. Salts incorporating all but one of the following ions are usually soluble in
water. Which ion is the exception?

a) nitrate ion
b) carbonate ion
c) sodium ion
d) ammonium ion

7. In which of the following pairs of ionic compounds are both members of the pair
insoluble in water?

a) sodium carbonate and barium carbonate
b) calcium sulfate and calcium nitrate
c) silver chloride and lead chloride
d) beryllium nitrate and beryllium phosphate

8. Which of the following percentage concentration units is most frequently used by
chemists? Note: m denotes mass and v denotes volume.

a) %(m/m)
b) %(m/v)
c) %(v/v)
d) %(v/m)

9. Which of the following gives the correct defining expression for molarity?

a) moles of solute/liter of solution
b) moles of solute/kilogram of solvent
c) moles of solute/liter of solute
d) moles of solute/liter of solvent

10. An aqueous solution contains 17 g NH₃ per 100 mL of solution. This solution is

a) 1.0 M NH₃
b) 1.7 M NH₃
c) 10.0 M NH₃
d) 17.0 M NH₃

11. The maximum solubility of NaCl is 36.0 g NaCl/100g H2O at 20^oC, therefore a solution at 20^oC containing 45 g NaCl/150 g H2O would be:

a. Dilute      b. Saturated      c. Supersaturated         d. Unsaturated
 

12. A solution is made by dissolving 0.40 mole of NaOH in enough water to give a final
volume of 250.0 mL. What is the molarity of the solution?

a) 0.1 M     b. 0.8 M     c. 1.6 M     d. 2.5 M

13. Molarity could be used as a conversion factor between

a) grams of solute and moles of solvent
b) moles of solute and volume of solution
c) grams of solute and volume of solution
d) moles of solute and kilograms of solute
 

14. A student wishes to prepare 180 mL of 0.20 M NaOH from 6.0 M NaOH. What volume of
the 6.0 M NaOH should he/she start with?

a) 6.0 mL
b) 18 mL
c) 3 mL
d) 9 mL
 

15. If 5.00 g NaCl are dissolved in 25.0 g of water, the percentage of NaCl be weight is:

a. 16.7     b. 20.0     c. 0.200      d. 0.166
 
 

16. What mass of 9.0% AgNO3 solution contains 5.3 g AgNO3?

a. 47.7 g     b. 0.58 g     c. 59 g     d. No correct answer given.
 
 

17. What mass of BaCl2 (FW = 208.25) will be required to prepare 200. mL of 0.150 M solution?

a. 0.750     b. 156 g     c. 6.25 g     d. 31.2 g
 

Problems 18-20, all refer to the following equation.

2HCl + CaCO3 ---> H2O + CO2 + CaCl2
 

18. What volume of 6.00 M HCl will be needed to react with 0.350 mole of CaCO3?

a. 42.0 mL     b. 1.17 L     c. 117 mL     d. 583 mL
 

19. If 400 mL of 2.0 M HCl react with excess CaCO3, the volume of CO2 produced, measured at STP, is:

a. 18 L     b. 5.6 L     c. 9.0 L     d. 56 L
 

20.   5.3 g of CaCl2 (FW = 110.99) were made by reacting 25 mL of HCl solution and excess CaCO3. What was the molarity of the HCl solution?

 a. 3.8 M     b. 0.19 M     c. 0.38 M     d. 0.42M