Chem 1405 homework of chap7
1. Which of the following statements about the solubility of a solute in a solvent is correct? (Section 7.3)
a. The solubility of a solute in a particular solvent is temperature-dependent.
b. When the solubility limit of a solute in a particular solvent has been reached, that solution is said to
be unsaturated.
c. All solutes that are soluble have unlimited values for solubility at a given temperature.
2. Which of the following salts would be classified as soluble in water? (Section 7.3)
a. BaSO4
b. BaCl2
c. Ca(OH)2
3. Vinegar is 5.00% (v/v) acetic acid. How many milliliters of acetic acid are in 25.0 mL of vinegar?
(Section 7.5)
a. 1.25 mL
b. 0.0125 mL
c. 0.200 mL
4. An intravenous solution of sodium chloride is 0.900% (w/v). How many milliliters of solution would be
required to deliver a 5.00-mg dose of sodium chloride? (Section 7.5)
a. 556 mL
b. 0.556 mL
c. 0.045 mL
5. How many grams of KCl would be required to prepare 100. mL of a 0.250-M KCl solution? (Section
7.6)
a. 1.86 g
b. 29.8 g
c. 3.35 × 10-4 g
6. What volume of 0.50 M AgNO3 solution would be required to obtain 0.2 moles of AgNO3? (Section
7.6)
a. 0.1 L
b. 0.4 L
c. 0.3
7. You require 200 mL of 20-mM MgCl2 for your experiment. However, you can find only 1.0 L of a 1.0M MgCl2 stock solution in the lab. How much stock solution is required to prepare the MgCl2 solution
required for your experiment? (Section 7.7)
a. 4000 mL
b. 4 mL
c. 10,000 mL
8. 300. mL of a 1.5-M solution of potassium chromate is diluted to 0.10 M for an experiment. What is
the final volume after dilution? (Section 7.7)
a. 4500 mL
b. 20 mL
c. 5 × 10-4 mL
9.What is the concentration in ppm of a solution that contains 0.147 g of glucose in 105 mL?
a. 75 ppm
b. 133 ppm
c. 1400ppm
10. Which of the following equations is the complete ionic equation for the reaction of NaCl and PbBr2?
(Section 7.10)
a. 2NaCl(aq) + PbBr2(s)  2NaBr(aq) + PbCl2(s)
b. 2Na+(aq) + 2Cl-(aq) + PbBr2(s)  2Na+(aq) + 2Br-(aq) + PbCl2(s)
c. 2Na+(aq) + 2Cl-(aq) + Pb2+ (s) + 2Br-(s)  2Na+(aq) + 2Br-(aq) + Pb2+ (s) + 2Cl-(s)
11. Calculate the osmolarity of 0.2 M Na2SO4. (Section 7.14)
a. 0.2 M
b. 0.4 M
c. 0.6 M
12. Calculate the osmolarity of 0.2 M glucose. (Section 7.14)
a. 0.2 M
b. 0.4 M
c. 0.6 M
13. If a cell comes into contact with a hypertonic solution, what will happen to the cell? (Section 7.15)
a. The cell will swell with water and burst.
b. The cell will lose water and shrink.
c. There will be no change in the volume of the cell.