Q: Which of the following is the correct formula for calculating the molarity of a solution?

$\mathrm{M = \dfrac{\text{moles\ of\ solute}}{\text{volume\ of\ solution\ in\ liters}}}$

Question 1

Which of the following statements best describes a strong electrolyte in aqueous solution?

Accepted Answer

It dissociates completely into ions and conducts electricity well.

Question 2

A student mixes solutions of $\mathrm{AgNO_3}$ and $\mathrm{NaCl}$. Which of the following is the correct net ionic equation for the reaction that occurs?

Accepted Answer

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

Question 3

Which of the following compounds is a strong base and a strong electrolyte?

Accepted Answer

$\mathrm{KOH}$

Question 4

A solution is prepared by dissolving 11.0 g of $\mathrm{NaCl}$ (molar mass = 58.44 g/mol) in enough water to make 250 mL of solution. What is the molarity of the solution?

Accepted Answer

$0.752\ \mathrm{M}$

Question 5

Which of the following pairs will produce a precipitate when mixed in aqueous solution?

Accepted Answer

$\mathrm{Pb(NO_3)_2}$ and $\mathrm{KI}$

Question 6

Which of the following is the correct balanced net ionic equation for the neutralization of hydrochloric acid with sodium hydroxide?

Accepted Answer

$\mathrm{H^+ (aq) + OH^- (aq) \rightarrow H_2O (l)}$

Question 7

A 50.0 mL sample of 0.200 M $\mathrm{H_2SO_4}$ is titrated with 0.100 M $\mathrm{NaOH}$. What volume of $\mathrm{NaOH}$ is required to reach the equivalence point? (Balanced equation: $\mathrm{H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O}$)

Accepted Answer

$200\ \mathrm{mL}$

Question 8

Which of the following is a weak acid and a weak electrolyte?

Accepted Answer

$\mathrm{HF}$

Question 9

A solution is made by diluting 25.0 mL of 6.00 M $\mathrm{HCl}$ to a final volume of 500.0 mL. What is the final concentration?

Accepted Answer

$0.300\ \mathrm{M}$

Question 10

Which of the following best describes the role of a spectator ion in a chemical reaction?

Accepted Answer

It does not participate in the chemical change and remains unchanged in solution.

Question 11

Which of the following reactions is a gas-forming reaction?

Accepted Answer

$\mathrm{Na_2CO_3 (s) + 2HCl (aq) \rightarrow 2NaCl (aq) + CO_2 (g) + H_2O (l)}$

Question 12

Which of the following is the correct formula for calculating the molarity of a solution?

Accepted Answer

$\mathrm{M = \dfrac{	ext{moles\ of\ solute}}{	ext{volume\ of\ solution\ in\ liters}}}$

Question 13

A hospital needs to prepare 1.00 L of 0.250 M $\mathrm{KCl}$ solution for intravenous use. How many grams of $\mathrm{KCl}$ (molar mass = 74.55 g/mol) are required?

Accepted Answer

$18.6\ \mathrm{g}$

Question 14

Which of the following is a correct statement about the solubility rules for ionic compounds in water?

Accepted Answer

All compounds containing $\mathrm{Na^+}$, $\mathrm{K^+}$, or $\mathrm{NH_4^+}$ are soluble.

Question 15

A solution contains 0.75 M $\mathrm{CuCl_2}$. What are the concentrations of $\mathrm{Cu^{2+}}$ and $\mathrm{Cl^-}$ ions?

Accepted Answer

$0.75\ \mathrm{M\ Cu^{2+}},\ 1.50\ \mathrm{M\ Cl^-}$

Question 16

Which of the following is the correct dilution equation to calculate the volume of a concentrated solution needed to prepare a dilute solution?

Accepted Answer

$M_1 V_1 = M_2 V_2$

Question 17

Which of the following is a real-life application of a precipitation reaction?

Accepted Answer

Removal of heavy metal ions from wastewater by adding chemicals that form insoluble salts.

Question 18

A laboratory technician needs to neutralize 25.0 mL of 0.200 M $\mathrm{HNO_3}$ with $\mathrm{Ca(OH)_2}$ (molar mass = 74.10 g/mol). How many grams of $\mathrm{Ca(OH)_2}$ are required? (Balanced equation: $\mathrm{Ca(OH)_2 + 2HNO_3 \rightarrow Ca(NO_3)_2 + 2H_2O}$)

Accepted Answer

$0.185\ \mathrm{g}$

Chapter 4: Reactions in Aqueous Solution – Solutions and Electrolytes

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