Question 1

Which of the following best explains why NaCl does not dissolve in hexane ($$C_6H_{14}$$)?

Accepted Answer

NaCl is ionic and the ion-ion forces in the lattice are not broken by ion-nonpolar interactions.

Question 2

Which property is NOT affected by intermolecular forces?

Accepted Answer

Color

Question 3

A figure shows a cation surrounded by water molecules. What is the principal interaction between the solute and solvent?

Accepted Answer

Ion-Dipole

Question 4

Which of the following ions will have the strongest ion-dipole interaction with water?

Accepted Answer

Mg$$^{2+}$$

Question 5

Which of the following statements about the enthalpy of solution ($$\Delta H_{soln}) is $$correct?

Accepted Answer

$$\Delta H_{soln} is $$the sum of the enthalpy changes for solute separation, solvent separation, and solute-solvent interaction.

Question 6

A solution is prepared by dissolving $$\mathrm{$$NaNO_3$$} in $$water. If the lattice energy is 100 kJ/mol and the enthalpy of solution is $$-50 kJ/$$mol, what is the hydration energy? (Assume $$\Delta H_{solvent} is $$negligible.)

Accepted Answer

$$-150 kJ/$$mol

Question 7

Which of the following best describes a saturated solution?

Accepted Answer

A solution in which the rate of dissolution equals the rate of crystallization.

Question 8

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

Accepted Answer

Increasing the partial pressure of the gas above the solution

Question 9

According to Henry's Law, the solubility of a gas in a liquid is given by $$S_g = k P_g. If $$the solubility of $$N_2 in $$water at 25$$^\circC $$and 0.78 atm is $$5.3 	imes 10$$^{-4}$$ M, what is the value of k$?

Accepted Answer

$$5.3 	imes 10$$^{-4}$$ M/atm

Question 10

Which of the following is a real-world example of a solid solution?

Accepted Answer

22K gold alloy

Question 11

Which of the following statements about the dissolution of ionic compounds in water is correct?

Accepted Answer

The process involves breaking ion-ion interactions and forming ion-dipole interactions.

Question 12

A student prepares a solution by dissolving more solute than the maximum amount that can dissolve at a given temperature, then cools it slowly without agitation. What type of solution is this?

Accepted Answer

Supersaturated

Question 13

Which of the following best explains why mixing two gases is a spontaneous process?

Accepted Answer

The entropy ($$\Delta S) $$increases when the gases mix.

Question 14

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

Accepted Answer

It increases with increasing pressure above the solution.

Question 15

Which of the following is an example of a physical change involving a solution?

Accepted Answer

Evaporating water from a salt solution to recover the salt.

Question 16

Which of the following statements about miscible liquids is correct?

Accepted Answer

They mix in all proportions due to similar intermolecular forces.

Question 17

If a solution is at dynamic equilibrium with respect to the dissolved substance, which of the following is true?

Accepted Answer

The rates of dissolution and crystallization are equal.

Question 18

Which of the following best describes the driving force for the formation of a solution between two substances?

Accepted Answer

Increase in entropy ($$\Delta S)$$

Question 19

Which of the following is NOT a step in the solution formation process?

Accepted Answer

Forming covalent bonds between solute and solvent

Properties of Solutions – General Chemistry Study Notes

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