Q: A solution is prepared by dissolving 20.0 g of NaOH in 80.0 g of water. What is the mass percent ($$\% m/m) of $$NaOH in the solution?

$$\displaystyle \frac{20.0}{100.0} \times 100\% = 20.0\%$$

Question 1

Which of the following best describes a solution?

Accepted Answer

A homogeneous mixture of two or more substances

Question 2

Which of the following statements about solutes and solvents is correct?

Accepted Answer

The solvent is present in a larger amount, and the solute is present in a smaller amount

Question 3

Which of the following substances would most likely dissolve in hexane ($$\mathrm{C_6H_{14}}$$), a nonpolar solvent?

Accepted Answer

Octane ($$\mathrm{C_8H_{18}})$$

Question 4

Which type of intermolecular force is primarily responsible for the dissolution of sodium chloride ($$\mathrm{NaCl}) in $$water?

Accepted Answer

Ion-dipole interactions

Question 5

Which of the following compounds is a strong electrolyte when dissolved in water?

Accepted Answer

Potassium bromide ($$\mathrm{KBr})$$

Question 6

A solution is prepared by dissolving 20.0 g of NaOH in 80.0 g of water. What is the mass percent ($$\% m/m) of $$NaOH in the solution?

Accepted Answer

$$\displaystyle \frac{20.0}{100.0} 	imes 100\% = 20.0\%$$

Question 7

Which of the following best explains why oil does not dissolve in water?

Accepted Answer

There are no significant intermolecular forces between nonpolar oil molecules and polar water molecules

Question 8

Which of the following reactions represents the dissociation of a strong electrolyte in water?

Accepted Answer

$$\mathrm{Na_2SO_4(s) \rightarrow 2Na^+(aq) + SO_4$^{2-}(aq)}$$

Question 9

A solution contains 60 g of KBr in 100 g of water at 40$$^\circC. If $$the solubility of KBr at this temperature is 80 g per 100 g water, the solution is:

Accepted Answer

Unsaturated

Question 10

Which of the following best describes a saturated solution?

Accepted Answer

A solution that contains the maximum amount of solute that can dissolve at a specific temperature

Question 11

Which of the following compounds will be insoluble in water according to solubility rules?

Accepted Answer

Calcium carbonate ($$\mathrm{$$CaCO_3$$})$$

Question 12

Which of the following best explains why methanol ($$\mathrm{CH_3OH}) is $$soluble in water?

Accepted Answer

Methanol forms hydrogen bonds with water due to its $$-\mathrm{OH}$$ group

Question 13

Which of the following is the correct net ionic equation for the reaction between aqueous solutions of NaCl and AgNO$$_3$$?

Accepted Answer

$$\mathrm{Ag^+(aq) + Cl^-(aq) \rightarrow AgCl(s)}$$

Question 14

Which of the following best describes the role of water in an aqueous solution of NaCl?

Accepted Answer

Water is the solvent

Question 15

Which of the following statements about electrolytes is true?

Accepted Answer

Electrolytes dissociate into ions when dissolved in water

Question 16

Which of the following best explains why $$\mathrm{NaCl} is $$classified as a strong electrolyte?

Accepted Answer

$$\mathrm{NaCl}$$ dissociates completely into ions in water

Question 17

Which of the following is a correct example of a polar solute dissolving in a polar solvent?

Accepted Answer

Methanol ($$\mathrm{CH_3OH}) $$dissolving in water ($$\mathrm{H_2O})$$

Question 18

Which of the following best describes the effect of increasing temperature on the solubility of most solid solutes in water?

Accepted Answer

Solubility increases with increasing temperature

Question 19

Which of the following best describes the effect of increasing pressure on the solubility of a gas in a liquid?

Accepted Answer

Solubility increases with increasing pressure

Solutions: Properties, Types, and Solubility (Chapter 9 Study Notes)

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