Q: Which equation is used to calculate the vapor pressure of a solution containing a non-volatile solute?

$$P_{solution} = \chi_{solvent} \times P$$^{\circ}$$_{solvent}$$

Question 1

Which of the following best explains why 'like dissolves like' in terms of intermolecular forces?

Accepted Answer

Because similar types of intermolecular forces between solute and solvent provide enough energy to break solute-solute and solvent-solvent interactions.

Question 2

A solution forms when the energy released from solute-solvent interactions is greater than the energy required to separate solute and solvent particles. Which equation represents the enthalpy of solution?

Accepted Answer

$$\Delta H_{solution} = \Delta H_{solute-solute} + \Delta H_{solvent-solvent} + \Delta H_{solute-solvent}$$

Question 3

Which of the following molecules would be most soluble in water?

Accepted Answer

CH$$_3OH$$

Question 4

Why can some solutions form even when the enthalpy of solution ($$\Delta H_{solution}) is $$positive?

Accepted Answer

Because the increase in entropy ($$\Delta S) $$can make the process spontaneous if $$T\Delta S \u003e \Delta H$$

Question 5

Which concentration unit is defined as moles of solute per kilogram of solvent?

Accepted Answer

Molality ($$m)$$

Question 6

A solution is prepared by mixing 1.00 g ethanol with 100.0 g of water. What is the mole fraction of ethanol in the solution? (Molar mass of ethanol = 46.07 g/mol, water = 18.02 g/mol)

Accepted Answer

$$\chi_{ethanol} = 0.00390$$

Question 7

Which of the following is a colloid rather than a solution or suspension?

Accepted Answer

Milk

Question 8

According to Henry’s Law, what happens to the solubility of a gas in a liquid as the pressure of the gas above the liquid increases?

Accepted Answer

The solubility increases proportionally.

Question 9

Which of the following best describes a supersaturated solution?

Accepted Answer

A solution that contains more solute than should be possible at a given temperature and is unstable.

Question 10

Which equation is used to calculate the vapor pressure of a solution containing a non-volatile solute?

Accepted Answer

$$P_{solution} = \chi_{solvent} 	imes P$$^{\circ}$$_{solvent}$$

Question 11

What is the Van’t Hoff factor ($$i) $$for CaCl$$_2 in an $$ideal solution?

Accepted Answer

$$i = 3$$

Question 12

Which of the following is a colligative property?

Accepted Answer

Freezing point depression

Question 13

A 0.89 m solution of CaCl$$_2 is $$prepared. What is the expected freezing point depression? ($$K_f = 1.86 \ ^\circC/m)$$

Accepted Answer

$$\Delta T_f = 4.97 \ ^\circC$

Question 14

Which of the following best explains why vapor pressure is lowered when a non-volatile solute is added to a solvent?

Accepted Answer

The solute particles reduce the number of solvent molecules at the surface, decreasing the rate of evaporation.

Question 15

A solution contains 36 g of NaCl in 100 g water at 90 °C. Is it saturated?

Accepted Answer

No

Question 16

Which process is described by the equation $$\pi = iMRT$$?

Accepted Answer

Osmotic pressure

Question 17

If a red blood cell is placed in a hypertonic solution, what will happen?

Accepted Answer

Water will leave the cell, causing it to shrink.

Question 18

Which of the following is true about the effect of temperature on the solubility of gases in water?

Accepted Answer

Solubility decreases as temperature increases.

Question 19

A solution is made by dissolving 35 g of NH$$_3 in 90.0 g of H$_2O. $$The density of the solution is 0.898 g/mL. What is the molarity of NH$$_3$$? (Molar mass NH$$_3 = 17.03 g/$$mol)

Accepted Answer

23 M

Question 20

Which of the following best describes the Tyndall effect?

Accepted Answer

Scattering of light by colloidal particles

Solutions and Their Properties (General Chemistry II, Ch. 13 Study Notes)

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