Question 1

Which of the following intermolecular forces is primarily responsible for the solubility of NaCl in water?

Accepted Answer

Ion-dipole interactions

Question 2

A solution is prepared by dissolving 5.00 g of urea (CO(NH$$_2$$)$$_2) in 0.100 kg of $$water. If the vapor pressure of pure water at 25 $$^	ext{o}C is 23.7 $$torr, what is the vapor pressure of the solution? (Molar mass of urea = 60.06 g/mol)

Accepted Answer

$$23.4$$ torr

Question 3

Which of the following best describes why the solubility of gases in water decreases as temperature increases?

Accepted Answer

Gas molecules have higher kinetic energy and escape more easily from the solution.

Question 4

A 0.33 m solution of a nonvolatile solute in benzene is prepared. If the boiling point elevation constant ($$K_b) $$for benzene is $$2.53 \, ^\circ \mathrm{C} \, m$$^{-1}$$, what is the boiling point of the solution? (Boiling point of pure benzene = 80.1$$ \, ^\circ \mathrm{C}$$)

Accepted Answer

$$80.9 \, ^\circ \mathrm{C}$$

Question 5

Which of the following statements about colligative properties is correct?

Accepted Answer

They depend only on the number of solute particles, not their identity.

Question 6

A red blood cell is placed in a solution and swells until it bursts. What type of solution was it placed in?

Accepted Answer

Hypotonic

Question 7

Which of the following best explains why ethanol and water are miscible in all proportions?

Accepted Answer

Both are polar and can form hydrogen bonds with each other.

Question 8

Calculate the osmotic pressure ($$\Pi) at 37$$ $$^\circC $$for a 0.30 M glucose solution. ($$R = 0.0821 \, \mathrm{L} \, \mathrm{atm} \, \mathrm{mol}^{-1} \, \mathrm{K}^{-1})$$

Accepted Answer

$$7.6$$ atm

Question 9

Which of the following compounds will have the highest solubility in water at 18 $$^\circC $$based on the provided data?

Accepted Answer

RbF

Question 10

A solution contains 0.850 g of ammonia (NH$$_3) $$dissolved in 125 g of water. What is the mole fraction of ammonia in the solution? (Molar mass of NH$$_3 = 17.03 g/$$mol, H$$_2O = 18.02 g/$$mol)

Accepted Answer

$$7.14 	imes 10$$^{-3}$$

Question 11

Which of the following best describes the Tyndall effect?

Accepted Answer

Scattering of visible light by a colloidal dispersion

Question 12

Which of the following is a strong electrolyte?

Accepted Answer

KCl

Question 13

Which of the following best explains why the hydrated radius of Li$$^+ is $$much larger than that of Cs$$^+$$?

Accepted Answer

Li$$^+$$ has a higher charge density, attracting more water molecules.

Question 14

Which of the following best describes an ideal solution?

Accepted Answer

A solution that forms with no accompanying energy change

Question 15

Which of the following is the correct expression for Henry’s Law?

Accepted Answer

$$C_g = kP_g$$

Question 16

A solution is prepared by dissolving 4.00 g of a nonelectrolyte in 55.0 g of benzene, resulting in a freezing point of 2.32 $$^\circC. If $$the freezing point depression constant ($$K_f) $$for benzene is 5.12 $$^\circC/m$$, what is the molar mass of the solute?

Accepted Answer

$$122 g/$$mol

Question 17

Which of the following best describes a colloid?

Accepted Answer

A mixture in which relatively large solid or liquid particles are dispersed uniformly throughout a medium

Question 18

Which of the following will increase the solubility of a gas in a liquid?

Accepted Answer

Increasing the partial pressure of the gas above the liquid

Question 19

Which of the following best explains why BaSO$$_4 is $$less soluble in water than MgSO$$_4$$?

Accepted Answer

Ba$$^{2+}$$ has a lower charge density, resulting in lower hydration energy compared to Mg$$^{2+}.$$

Solutions and Their Properties: Structure, Solubility, and Colligative Effects

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