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1			The most significant forces between solute and solvent in an aqueous MgCl2 solution are
			A)	ion-ion interactions.
			B)	ion-dipole interactions.
			C)	dispersion forces.
			D)	hydrogen-bonding.
			E)	dipole-dipole forces.
2			Which of the following liquids would make a good solvent for bromine, Br2?
			A)	HCl
			B)	H2O
			C)	CH3OH
			D)	NH3
			E)	CS2
3			Dissolving solid of CaCl2•6H2O in a large volume of water is endothermic to the extent of 14.6 kJ/mol. Also given: CaCl2(s) + 6H2O(l)→ CaCl2•6H2O(s) ΔH = -97.0 kJ What is the heat of solution of anhydrous CaCl2 in a large volume of water?
			A)	111.6 kJ/mol
			B)	82.3 kJ/mol
			C)	-111.6 kJ/mol
			D)	-82.3 kJ/mol
			E)	none of the above
4			Considering only monatomic ions with their normal charges, which of the following ions will have the highest (most negative) heats of hydration?
			A)	ions of group 1A(1)
			B)	small ions of group 2A(2)
			C)	large ions of group 2A(2)
			D)	small ions of group 7A(17)
			E)	large ions of group 7A(17)
5			The Henry's law constant for CO2 at 20°C is kH = 3.7 X 10-2 mol/L•atm. What mass of CO2 (in grams) is present in 355 mL of a soda drink if the pressure of CO2 in the can is 2.5 atmospheres at 20°C? (Assume the solubility of CO2 in the soda is the same as in water.)
			A)	4.1 g
			B)	1.4 g
			C)	0.093 g
			D)	0.033 g
			E)	none of the above
6			If 50.0 mL of 0.150 M magnesium bromide is combined with 200 mL of 0.110 M sodium bromide what is the molarity of the bromide ion in the resulting solution? (assume volumes are additive)
			A)	0.074 M
			B)	0.26 M
			C)	0.0118 M
			D)	0.148 M
			E)	0.52 M
7			What is the molality of a solution which contains 38.0 g of cane sugar, C12H22O11, dissolved in 175 g of water?
			A)	0.514 mol/kg
			B)	635.0 mol/kg
			C)	0.217 mol/kg
			D)	0.635 mol/kg
			E)	217.0 mol/kg
8			A solute is present in aqueous solution at a concentration of 1 ppm by mass. What is this concentration in mg/L? (Assume that the solution density is 1 g/mL and that the mass of solution is equal to the mass of water present.)
			A)	1 x 10-6 mg/L
			B)	0.001 mg/L
			C)	0.1 mg/L
			D)	1 mg/L
			E)	none of the above
9			The solubility of oxygen in water is about 4.5 x 10-2 g/L. How many millimoles of O2 could dissolve in 5.0 L of water?
			A)	29 mmol
			B)	20. mmol
			C)	7.0 mmol
			D)	9.0 mmol
			E)	0.29 mmol
10			How many grams of ethanol (C2H6O) are in a 250 mL sample of a solution which is 20% ethanol by volume in water. The density of ethanol is 0.79 g/mL.
			A)	46 g
			B)	50 g
			C)	1.1 g
			D)	40. g
			E)	2.5 g
11			The freezing point of pure camphor is 178.4°C, and its molal freezing-point constant, Kf is 40.0°C/m. Find the freezing point of a solution containing 3.00 g of a compound of molar mass 125 g/mol in 45.0 g of camphor.
			A)	174.1°C
			B)	157.1°C
			C)	135.2°C
			D)	140.4°C
			E)	11.6°C
12			The molar mass of a nonvolatile solute is 176.0 g/mol. Compute the boiling point of a solution containing 68.0 g of the solute and 750.0 g of water, when the barometric pressure is such that pure water boils at 99.825°C. (Kb= 0.52°C/m)
			A)	101.2°C
			B)	100.1°C
			C)	99.8 °C
			D)	98.5°C
			E)	102.4°C
13			Which of the following is true concerning the composition of the vapor above a solution of two volatile substances?
			A)	It is independent of the composition of the solution.
			B)	It is enriched in the less volatile component.
			C)	It is enriched in the more volatile component.
			D)	It has the same composition as the solution.
			E)	It depends only on the temperature.
14			Which of the compounds listed will have the highest van't Hoff factor, i?
			A)	glucose
			B)	NaCl
			C)	MgCl2
			D)	FeCl3
			E)	CCl4
15			The dimensions of typical colloidal particles are of the order of
			A)	dm
			B)	pm
			C)	mm
			D)	mm
			E)	fm