Q: Which of the following is the correct calculation for the number of moles in 1.5 L of a 3.5 M solution?

$3.5\ \mathrm{mol/L} \times 1.5\ \mathrm{L} = 5.25\ \mathrm{mol}$

Question 1

Which of the following best describes a neutralization reaction?

Accepted Answer

A reaction in which an acid and a base combine to form water and an ionic salt.

Question 2

What is the balanced chemical equation for the neutralization of acetic acid ($\mathrm{CH_3COOH}$) with ammonia ($\mathrm{NH_3}$)?

Accepted Answer

$\mathrm{CH_3COOH_{(aq)} + NH_3_{(aq)} \rightarrow H_2O_{(l)} + NH_4CH_3COO_{(aq)}}$

Question 3

Which statement about acids and bases is correct?

Accepted Answer

Acids have a higher concentration of $\mathrm{H^+}$ ions, while bases have a higher concentration of $\mathrm{OH^-}$ ions.

Question 4

What is the molarity of a solution prepared by dissolving 23.4 g of $\mathrm{Na_2SO_4}$ in enough water to make 125 mL of solution? (Molar mass of $\mathrm{Na_2SO_4}$ = 142.042 g/mol)

Accepted Answer

$1.32\ \mathrm{M}$

Question 5

A student wants to prepare 1.5 L of a 3.5 M NaOH solution. How many grams of NaOH are required? (Molar mass of NaOH = 39.997 g/mol)

Accepted Answer

$210\ \mathrm{g}$

Question 6

Which of the following is a product of the reaction between hydrochloric acid ($\mathrm{HCl}$) and sodium hydroxide ($\mathrm{NaOH}$)?

Accepted Answer

Both $\mathrm{NaCl}$ and $\mathrm{H_2O}$

Question 7

If 0.250 mol of solute is dissolved in 500 mL of solution, what is the molarity?

Accepted Answer

$0.50\ \mathrm{M}$

Question 8

Which of the following best explains why pure water is considered neutral?

Accepted Answer

It contains equal concentrations of $\mathrm{H^+}$ and $\mathrm{OH^-}$ ions.

Question 9

A solution is prepared by dissolving 10.0 g of NaCl (molar mass = 58.44 g/mol) in enough water to make 250 mL of solution. What is the molarity?

Accepted Answer

$0.684\ \mathrm{M}$

Question 10

Which of the following is true about the pH scale?

Accepted Answer

It ranks the acidity or basicity of a solution based on the concentration of $\mathrm{H^+}$ ions.

Question 11

Which of the following is a correct expression for molarity?

Accepted Answer

$\mathrm{Molarity = \frac{moles\ of\ solute}{volume\ of\ solution\ in\ Liters}}$

Question 12

A chemist mixes 0.50 mol of HCl with 0.50 mol of NaOH in 1.0 L of water. What is the concentration of NaCl formed?

Accepted Answer

$0.50\ \mathrm{M}$

Question 13

Which of the following is a double displacement reaction?

Accepted Answer

$\mathrm{HCl_{(aq)} + NaOH_{(aq)} \rightarrow H_2O_{(l)} + NaCl_{(aq)}}$

Question 14

If you have 0.16474 mol of $\mathrm{Na_2SO_4}$ dissolved in 0.125 L of solution, what is the molarity?

Accepted Answer

$1.32\ \mathrm{M}$

Question 15

Which of the following would NOT result from a neutralization reaction?

Accepted Answer

Increase in $\mathrm{OH^-}$ ion concentration

Question 16

A solution contains 0.75 mol of solute in 2.5 L of solution. What is its molarity?

Accepted Answer

$0.30\ \mathrm{M}$

Question 17

Which of the following is the correct calculation for the number of moles in 1.5 L of a 3.5 M solution?

Accepted Answer

$3.5\ \mathrm{mol/L} 	imes 1.5\ \mathrm{L} = 5.25\ \mathrm{mol}$

Question 18

Which of the following best describes the role of water in a neutralization reaction?

Accepted Answer

Water is formed when $\mathrm{H^+}$ ions from the acid react with $\mathrm{OH^-}$ ions from the base.

Acid-Base Neutralization Reactions and Solution Concentrations

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