Question 1

Which of the following best describes a saturated solution at a given temperature?

Accepted Answer

A solution in which the dissolved solute is in dynamic equilibrium with undissolved solute.

Question 2

Which of the following statements explains why oil and water are immiscible?

Accepted Answer

The energy required to break hydrogen bonds in water and London dispersion forces in oil is much greater than the energy released when oil and water interact.

Question 3

Which of the following best describes the process of hydration when an ionic compound dissolves in water?

Accepted Answer

Ions are surrounded by water molecules due to ion-dipole attractions.

Question 4

Given the equation $$\Delta H_{solution} = -\Delta H_{lattice} + \Delta H_{hydration}$$, what does a positive $$\Delta H_{solution}$$ indicate about the dissolution process?

Accepted Answer

The process is endothermic and the solution will feel cold.

Question 5

Which of the following compounds would be most soluble in benzene ($$C_6H_6$$)?

Accepted Answer

Iodine ($$I_2)$$

Question 6

Which of the following is the correct application of Henry’s Law for the solubility of a gas in a liquid?

Accepted Answer

$$S_{gas} = k_H P_{gas}$$

Question 7

A student adds 110 g of $$CuCl_2 to 100 mL of $$water at $$0^\circC. $$The solubility of $$CuCl_2 at $$this temperature is 70.6 g/100 mL. What type of solution is formed?

Accepted Answer

Saturated with excess solid remaining

Question 8

Which of the following factors increases the enthalpy of hydration ($$\Delta H_{hydration}) $$for an ion?

Accepted Answer

Small ionic radius and high charge

Question 9

Which of the following best explains why the solubility of $$NaNO_3 in $$water is much higher than that of $$Ca_3$$($$PO_4)_2$?

Accepted Answer

$$Ca_3$$($$PO_4)_2$ has a much higher lattice energy due to higher ionic charges.

Question 10

Which of the following statements about the effect of temperature on solubility is correct?

Accepted Answer

The solubility of most solids in water increases with increasing temperature, but the solubility of gases decreases.

Question 11

Which of the following best describes the trend in solubility of alcohols in water as the hydrocarbon chain length increases?

Accepted Answer

Solubility decreases because the molecule becomes less polar.

Question 12

A beaker containing water and ammonium nitrate ($$NH_4NO_3) $$becomes cold as the salt dissolves. What does this observation indicate?

Accepted Answer

The dissolution is endothermic.

Question 13

Which of the following is NOT a colligative property of solutions?

Accepted Answer

Color change

Question 14

Which of the following pairs will be miscible in all proportions?

Accepted Answer

Methanol and water

Question 15

Which of the following best explains why vitamin C is water-soluble but vitamin A is fat-soluble?

Accepted Answer

Vitamin C has multiple OH groups for hydrogen bonding with water, while vitamin A is mostly hydrocarbon.

Question 16

If the partial pressure of oxygen above water is 0.21 atm and $$k_H = 1.28 	imes 10$$^{-3}$$ mol L$$^{-1}$$ atm$$^{-1}$$, what is the solubility of oxygen in water at 25$$^\circ$$C?

Accepted Answer

$$2.7 	imes 10$$^{-4}$$ mol L$$^{-1}$$

Question 17

Which of the following is the best example of a solid solution?

Accepted Answer

Brass (copper and zinc)

Question 18

Which of the following statements about lattice energy is correct?

Accepted Answer

Lattice energy is more negative for ions with higher charges.

Question 19

Which of the following best describes the 'like dissolves like' rule?

Accepted Answer

Substances with similar intermolecular attractive forces dissolve in each other.

Chapter 14 lecture 1

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