General Chemistry 1 Practice Questions (Set 13)

1. What volume of a 0.771 M solution of CaCl2 contains 1.28 g of solute?
A) 66.8 mL
B) 15.0 mL
C) 1.66 mL
D) 8.89 mL
E) 85.0 mL

2. Determine the molarity of a solution containing 6.76 g BaCl2 in 750.0 mL of solution.
A) 3.25 x 10–2 M
B) 2.44 x 10–2 M
C) 9.01 x 10–3 M
D) 4.33 x 10–2 M
E) 9.01 M

3. A solution containing 292 g of Mg(NO3)2 per liter has a density of 1.108 g/mL. The molality of the solution is:
A) 2.00 m
B) 2.41 m
C) 1.77 m
D) 6.39 m
E) none of these

4. A 20.0-g sample of methyl alcohol (CH3OH, molar mass = 32.04 g/mol) was dissolved in 43.3 g of water. The mole fraction of CH3OH is:
A) 0.260
B) 0.624
C) 0.316
D) 4.85
E) 0.206

5. The term “proof” is defined as twice the percent by volume of pure ethanol in solution. Thus, a solution that is 95% (by volume) ethanol is 190 proof. What is the molarity of ethanol in a 92 proof ethanol/water solution?

density of ethanol
= 0.80 g/cm3

density of water
= 1.0 g/cm3

mol. wt. of ethanol
= 46 g/mol

A) 0.46 M
B) 0.80 M
C) 0.92 M
D) 8.0 M
E) 17 M

6. Rank the following compounds according to increasing solubility in water.
I.
CH3–CH2–CH2–CH3
II.
CH3–CH2–O–CH2–CH3
III.
CH3–CH2–OH
IV.
CH3–OH

A) I < III < IV < II
B) I < II < IV < III
C) III < IV < II < I
D) I < II < III < IV
E) None of these (A-D) is correct.

7. When solid Ca(CH3COO)2 is dissolved in a nearly saturated solution of Ca(CH3COO)2, the solution becomes warmer. This information indicates that if the temperature of a solution is decreased:
A) dH will become negative.
B) dH will become zero.
C) The solubility of Ca(CH3COO)2 will decrease.
D) The solubility of Ca(CH3COO)2 will increase.
E) The solubility of Ca(CH3COO)2 will not change.

8. The solubility of O2 in water is 0.590 g/L at an oxygen pressure of around 14.5 atm. What is the Henry’s law constant for O2 (in units of mol/L·atm)?
A) 4.07 x 10–2
B) 1.27 x 10–3
C) 7.86 x 102
D) 2.67 x 10–1
E) None of the above are within 5% of the correct answer.

9. A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution
A) increases over time
B) decreases over time
C) stays the same over time
D) need to know which salt is in the solution to answer this
E) need to know the temperature and pressure to answer this

10. What is reverse osmosis?
A) the application, to a concentrated solution, of a pressure that is greater than the osmotic pressure, such that solvent flows from the concentrated solution to the dilute solution
B) the application, to a dilute solution, of a pressure that is greater than the osmotic pressure, such that solvent flows from the concentrated solution to the dilute solution
C) the application, to a concentrated solution, of a pressure that is greater than the osmotic pressure, such that solute flows from the concentrated solution to the dilute solution
D) the application, to a dilute solution, of a pressure that is greater than the osmotic pressure, such that solute flows from the concentrated solution to the dilute solution
E) the application, to a concentrated solution, of a pressure that is greater than the osmotic pressure, such that solvent flows from the dilute solution to the concentrated solution

11) Describe what happens when seawater is consumed to quench thirst.
A) Seawater can quench thirst once it is boiled.
B) Seawater quenches thirst when directly ingested.
C) Seawater draws water out of the body resulting in further dehydration and diarrhea.
D) Seawater helps diarrhea.
E) Seawater must be ingested at twice the volume to quench thirst.

12) Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?
A) trimethylamine (N(CH3)3)
B) acetone (CH3COCH3)
C) ethylene glycol (HOCH2CH2OH)
D) hexane (CH3CH2CH2CH2CH2CH3)
E) None of these compounds should be soluble in ethanol.

13) Which of the following compounds is most soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?
A) methanol
B) ethanol
C) 1-propanol
D) 1-butanol
E) 1-pentanol

14) If two substances are soluble in all proportions then they are ________ in each other.
A) miscible
B) nonpolar
C) immiscible
D) neutral
E) polar

15) A solution containing less than the equilibrium solute amount is called
A) an unsaturated solution.
B) a dilute solution.
C) a supersaturated solution.
D) a concentrated solution.
E) a saturated solution.

16) A solution containing more than the equilibrium amount is called
A) an unsaturated solution.
B) a dilute solution.
C) a supersaturated solution.
D) a concentrated solution.
E) a saturated solution.

17) What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?
A) 2.02 g
B) 4.94 g
C) 1.19 g
D) 8.42 g
E) 1.90 g

18) Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH
(d = 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d = 0.811 g/mL).
A) 0.630 m
B) 0.812 m
C) 1.57 m
D) 2.01 m
E) 4.98 m

19) A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.
A) 4.09 ? 10-3
B) 7.80 ? 10-2
C) 1.28 ? 10-3
D) 7.23 ? 10-2
E) 2.45 ? 10-3

20) A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.
A) 6.04 ? 10-3
B) 1.65 ? 10-2
C) 1.40 ? 10-3
D) 1.32 ? 10-2
E) 8.84 ? 10-2

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