Question 1

Which of the following best describes the difference between acids and bases in terms of their behavior in aqueous solution?

Accepted Answer

Acids produce $$\mathrm{H^+}$$ ions, while bases produce $$\mathrm{OH^-}$$ ions.

Question 2

Which compound is classified as a base?

Accepted Answer

Ba(OH)$$_2$$

Question 3

What ions are produced when HCl is dissolved in water?

Accepted Answer

$$\mathrm{H^+}$$ and $$\mathrm{Cl^-}$$

Question 4

Which of the following best describes what happens to a base in solution?

Accepted Answer

It produces $$\mathrm{OH^-}$$ ions.

Question 5

How does the dissociation of NaOH in water appear in a chemical equation?

Accepted Answer

$$\mathrm{NaOH (aq) \rightarrow Na^+ (aq) + OH^- (aq)}$$

Question 6

A chemical in the lab reacts with a base to produce salt and water. This compound is best described as:

Accepted Answer

An acid

Question 7

A chemical in the lab feels slippery and tastes bitter. This compound is best described as:

Accepted Answer

A base

Question 8

Which of the following statements best describes a strong acid compared to a weak acid?

Accepted Answer

A strong acid completely dissociates in water, while a weak acid only partially dissociates.

Question 9

If the pH of a base is close to 14, what does this indicate about the concentration of ions in solution?

Accepted Answer

High concentration of $$\mathrm{OH^-}$$ ions

Question 10

Which definition best describes an Arrhenius acid?

Accepted Answer

A substance that produces $$\mathrm{H^+}$$ ions in solution

Question 11

Which of the following is a Bronsted-Lowry base?

Accepted Answer

A substance that accepts $$\mathrm{H^+}$$ ions

Question 12

Which of the following best describes a conjugate acid-base pair?

Accepted Answer

Two substances that differ by a $$\mathrm{H^+}$$ ion

Question 13

In the reaction $$\mathrm{$$HNO_3$$ + H_2O \rightarrow H_3O^+ + NO_3$^-}$$, which pair represents the conjugate acid-base pair?

Accepted Answer

$$\mathrm{$$HNO_3$$}$$ and $$\mathrm{NO_3$^-}$$

Question 14

What is the main difference between an Arrhenius acid/base and a Bronsted-Lowry acid/base?

Accepted Answer

Arrhenius acids/bases are defined by their behavior in water, while Bronsted-Lowry acids/bases are defined by their ability to donate or accept $$\mathrm{H^+}$$ ions.

Question 15

Which of the following is NOT an electrolyte?

Accepted Answer

Pure water

Question 16

Why is pure water NOT an electrolyte, but an acid or base is?

Accepted Answer

Pure water does not contain ions, while acids and bases produce ions in solution.

Question 17

What is the purpose of a buffer solution?

Accepted Answer

To maintain a constant pH when small amounts of acid or base are added.

Question 18

Which two components are required to make a buffer?

Accepted Answer

A weak acid and its conjugate base

Question 19

If the pH of a solution changes from 4 to 3, what happens to the hydrogen ion concentration?

Accepted Answer

It increases by a factor of 10

Question 20

Solution A has a pH of 4 and solution B has a pH of 6. How many times greater is the hydronium ion concentration in solution A than in solution B?

Accepted Answer

100 times greater

Acids and Bases Review – Step-by-Step Study Guidance

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