AP Chemistry Review Questions - Properties of Solutions
How many milliliters of 6.0 M HNO3 are needed to prepare 500 mL of 0.50 M HNO3?
0.25 mL
40 mL
15.76 mL
300 mL
None of these are correct
Which of the following compounds is expected to be the most soluble in water?
CH3-CH2-CH2-CH3
CH4
CH3-OH
CH3-CH2-O-CH2-CH3
CH3-CH2-CH2-CH2-OH
Find the mass percent of ZnSO4 in a solution whose density is 1.25 g/mL and whose molarity is 1.19 M.
15.4 %
0.2 %
23.0 %
78%
31.1%
Find the mole fraction of the ZnSO4 in a solution whose density is 1.25 g/mL and whose molarity is 1.19 M ZnSO4.
1.02
0.575
0.0199
4.09
0.174
Find the molality of a solution of ZnSO4 whose density is 1.25 g/mL and whose molarity is 1.19 M.
1.12 m
5.31 m
0.970 m
0.0571 m
None of these
Which of the following solute/solvent pairs best represents the principle of "like dissolves like"?
carbon dioxide in water
lipids (fats) in water
salt in hexane
hydrogen chloride in water
potassium iodide in benzene
The vapor pressure of water at 25.0°C is 23.8 torr. Determine the mass of sodium chloride needed to add to 400 mL of water to change the vapor pressure to 22.8 torr. Assume the density of water to be 1.0 g/mL.
0.12 g
54 g
117 g
8.15 g
None of these
Of the following compounds, which are not likely to increase in solubility as the temperature of the solution increases?
1. CH4
2. NaBr
3. CO2
4. Glucose, C6H12O6
5. CuSO4
1 and 4
2 and 3
1 and 3
4 only
5 only
At a given temperature the vapor pressure of pure liquid diethyl ether and isopropyl alcohol are 730 torr and 310 torr, respectively. A solution prepared by mixing isopropyl alcohol and diethyl ether obeys Raoult's law. At this temperature, what is the vapor pressure of diethyl ether over a solution in which its mole fraction is 0.270?
197 torr
281 torr
1040 torr
15.7 torr
0.912 torr
Which of the following properties is dependent on the amount and identity of the solute particles?
Freezing point of the solution
Boiling point of the solution
Osmotic pressure
Solution density
None of these
How many grams of Al2(SO4)3 do you need to make 87.62 g of 0.0162 m Al2(SO4)3 solution?
5.54 g
0.483 g
0.0751 g
194 g
1005 g
When 18.0 grams of a substance is dissolved in 500 grams of water, the freezing point is depressed by 0.31°. What is the molar mass of the solute?
3.0 g
108 g
216 g
54 g
1018 g
You are given the problem of lowering the freezing point of H2O from 0°C to 0°F (-17.8°C), what volume of methyl alcohol (CH3OH) should you add to 10.0 liters of H2O? The density of CH3OH is 0.787 g/mL. Assume the density of the water to be exactly 1.00 g/mL.
32.05 mL
316 mL
402 mL
4.02 L
None of these
Two sodium chloride solutions are separated by a semipermeable membrane. The concentration of solution "A" is 0.50 M and the concentration of solution "B" is 0.250 M. Over time, there will be a measurable movement of:
water from solution A to B
water from solution B to A
sodium chloride from solution A to B
sodium chloride from solution B to A
Two of these are correct
The expected (ideal) van't Hoff factor for a dilute solution of sodium sulfate is:
1
2
3
4
5
A 0.250 M solution of CaCl2 has an observed osmotic pressure of 10.1 atm at 23°C. Determine the observed van't Hoff factor for this experiment.
1.67
2.73
1.22
0.976
0.002
How many grams of calcium chloride are needed to prepare 300 mL of a 0.250 M solution?
832 g
5.66 g
566 g
112 g
8.32 g
Calculate the osmotic pressure (in torr) of 7.50 liters of an aqueous 0.210 M solution of silver nitrate at 25°C, assuming 100% dissociation.
10.3 torr
7.81 x 103 torr
0.86 torr
655 torr
1100 torr
Which of the following solutions would be expected to experience the largest deviation from the expected van't Hoff factor?
1.5 M NaCl
0.5 M CH3OH
1.0 M glucose
0.010 M NaCl
Both NaCl solutions would have the same deviation
What is the percentage by mass of ethanol (C2H5OH) in a 1.5 m solution?