Question 1

Which of the following statements about electrolytes is TRUE?

Accepted Answer

A strong electrolyte completely dissociates into ions in solution.

Question 2

A solution contains 2.0% NaCl by mass. How much NaCl is present in 6.57 g of the solution?

Accepted Answer

$0.131\ \mathrm{g}$

Question 3

Which of the following compounds is a strong electrolyte?

Accepted Answer

NaCl

Question 4

What is the mass percent of an ammonium carbonate solution prepared by dissolving 33.2 g of solid into 395 g of water?

Accepted Answer

$7.75\%$

Question 5

What is the mass percent of a sodium fluoride solution prepared by dissolving 0.64 moles of sodium fluoride into 635 g of water? (Molar mass NaF = $41.99\ \mathrm{g/mol}$)

Accepted Answer

$4.05\%$

Question 6

A saturated solution contains the maximum amount of solute under the solution conditions. Which statement is FALSE?

Accepted Answer

A saturated solution contains less solute than an unsaturated solution.

Question 7

Calculate the amount of water (in kilograms) that must be added to 8.0 g of urea, CO(NH$_2$)$_2$, in the preparation of a 0.15% (by mass) solution. (Molar mass of urea = $60.06\ \mathrm{g/mol}$)

Accepted Answer

$5.33\ \mathrm{kg}$

Question 8

What is the concentration of a KNO$_3$ solution that is 2.58 M in nitrate ions?

Accepted Answer

$2.58\ \mathrm{M}$

Question 9

To produce a sample of silver chromate, you will need at least 2.14 g of potassium chromate to react with an excess of silver nitrate. If using a 6.00 M K$_2$CrO$_4$ solution, what volume in mL of this solution is needed for the reaction? (Molar mass K$_2$CrO$_4$ = $194.19\ \mathrm{g/mol}$)

Accepted Answer

$1.84\ \mathrm{mL}$

Question 10

There is a sample of 1.5 L of 2.00 M KNO$_3$. What is the new molarity of the solution when 1.5 L of water is added?

Accepted Answer

$1.00\ \mathrm{M}$

Question 11

Determine the volume of 0.150 M NaOH solution required to neutralize 55 mL of a 0.085 M HCl solution according to the neutralization reaction: $\mathrm{NaOH(aq) + HCl(aq) \rightarrow H_2O(l) + NaCl(aq)}$

Accepted Answer

$31.2\ \mathrm{mL}$

Question 12

Which statement best explains why ionic solutes typically dissolve in polar solvents?

Accepted Answer

The positive and negative ions are stabilized by the partial charges of the polar solvent molecules.

Question 13

A sugar solution at 13.5% percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water. What is the total mass of the solution?

Accepted Answer

$101.25\ \mathrm{g}$

Question 14

Which of the following is NOT a property of a solution?

Accepted Answer

The solute particles are visible to the naked eye.

Question 15

A student prepares a solution by dissolving 5.00 g of KCl in enough water to make 250 mL of solution. What is the molarity of the solution? (Molar mass KCl = $74.55\ \mathrm{g/mol}$)

Accepted Answer

$0.268\ \mathrm{M}$

Question 16

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

Accepted Answer

Increasing the pressure above the liquid.

Question 17

A solution is prepared by mixing 25.0 mL of 0.200 M Na$_2$SO$_4$ with 75.0 mL of water. What is the final concentration of Na$_2$SO$_4$?

Accepted Answer

$0.050\ \mathrm{M}$

Question 18

Which of the following is a real-life example of a weak electrolyte?

Accepted Answer

Acetic acid (vinegar) in water.

Solutions and Solution Chemistry (Chapter 13) – Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards