Question 1

Which of the following best describes a solution?

Accepted Answer

A homogeneous mixture consisting of a solute dissolved in a solvent

Question 2

According to Henry's Law, what is the relationship between the solubility of a gas in a liquid and the partial pressure of the gas above the liquid?

Accepted Answer

The solubility is directly proportional to the partial pressure, as given by $$C_g = k_H P_g$$

Question 3

A solution is prepared by dissolving 5.65 g of an unknown compound in 100.0 g of benzene, lowering the freezing point from 5.45°C to 4.39°C. If the freezing point depression constant $$K_f$$ for benzene is $$5.12 \ \mathrm{°C \ kg \ $$mol^{-1}$$}$$, what is the molar mass of the unknown compound?

Accepted Answer

246.5 g/mol

Question 4

Which concentration unit is best suited for calculations involving colligative properties because it does not vary with temperature?

Accepted Answer

Molality ($$m)$$

Question 5

What is the effect of adding a nonvolatile solute to a volatile solvent on the vapor pressure of the solution?

Accepted Answer

The vapor pressure of the solution decreases, as described by $$P_{solution} = X_{solvent} P_{solvent}$$

Question 6

A 0.556 M aqueous solution of glucose (density = 1.00 g/mL, molar mass = 180.2 g/mol) is prepared. What is the molality of glucose in this solution?

Accepted Answer

0.60 mol/kg

Question 7

Which of the following statements about electrolytes is correct?

Accepted Answer

Nonelectrolytes do not dissociate into ions in water

Question 8

Which equation correctly expresses the osmotic pressure ($$\pi) of a $$dilute solution?

Accepted Answer

$$\pi = M R T$$

Question 9

A solution is made by dissolving 10.0 g of hemoglobin in enough water to make 1.00 L of solution. The osmotic pressure is measured to be 5.9 torr at 22°C. What is the molar mass of hemoglobin? (Use $$\pi = M R T$$, $$R = 0.0821 \ \mathrm{L \ atm \ $$mol^{-1}$$ \ K$$^{-1}$$}$$, $$T = 295 \ \mathrm{K}$$, $$1 \ \mathrm{atm} = 760 \ \mathrm{torr})$$

Accepted Answer

6.8 x $$10^4 g/$$mol

Question 10

Which of the following best explains why the solubility of gases in liquids decreases with increasing temperature?

Accepted Answer

Higher temperature increases the kinetic energy, causing gas molecules to escape from the solution

Question 11

Which of the following is a colligative property?

Accepted Answer

Boiling point elevation

Question 12

If 1.0 mol of NaCl is dissolved in water, what is the expected van't Hoff factor ($$i) $$for this strong electrolyte?

Accepted Answer

$$i = 2$$

Question 13

Which of the following pairs will form a miscible solution?

Accepted Answer

Ethanol and water

Question 14

A solution is prepared by dissolving 30 mol NaCl in 10 kg H$$_2O. $$What is the mole fraction of NaCl in the solution?

Accepted Answer

0.05

Question 15

Which of the following statements about colligative properties is true?

Accepted Answer

They depend only on the number of solute particles present

Question 16

Which formula is used to calculate the boiling point elevation of a solution?

Accepted Answer

$$\Delta T_b = K_b m$$

Question 17

Which of the following is NOT a strong electrolyte?

Accepted Answer

CH$$_3$$COOH

Question 18

If a solution is supersaturated, which of the following is true?

Accepted Answer

It contains more solute than required for saturation

Question 19

Which of the following best describes the process of osmosis?

Accepted Answer

Solvent molecules move across a membrane from low to high solute concentration

Solutions and Colligative Properties: Study Notes for General Chemistry

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