Q: A solution has a pH of 5.00. What is the $$[\mathrm{H_3O^+}]$$ concentration?

$$1.0 \times 10$$^{-5}$$\ \mathrm{M}$$

Question 1

Which of the following best describes an Arrhenius acid?

Accepted Answer

A substance that produces hydrogen ions $$\mathrm{(H^+)}$$ when dissolved in water

Question 2

Which of the following is the correct name for $$\mathrm{H_2SO_3}$$?

Accepted Answer

Sulfurous acid

Question 3

In the reaction $$\mathrm{NH_3$ + H_2O \rightleftharpoons NH_4$^+ + OH^-}$$, which species acts as the Brønsted-Lowry base?

Accepted Answer

$$\mathrm{NH_3$}$$

Question 4

Which of the following statements about strong acids is TRUE?

Accepted Answer

They completely dissociate into ions in aqueous solution

Question 5

A solution has $$[\mathrm{H_3O^+}] = 2.5 	imes 10$$^{-4}$$\ \mathrm{M}. $$What is the pH of the solution? (Report to two decimal places.)

Accepted Answer

$$3.60$$

Question 6

Which of the following is an example of an amphoteric substance?

Accepted Answer

Water ($$\mathrm{H_2O})$$

Question 7

Which of the following is the conjugate base of $$\mathrm{$$HCO_3$$^-}$$?

Accepted Answer

$$\mathrm{CO_3$^{2-}}$$

Question 8

A buffer solution is prepared using acetic acid ($$\mathrm{CH_3COOH}) $$and sodium acetate ($$\mathrm{CH_3COONa}). $$What is the main function of this buffer in a biological system?

Accepted Answer

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

Question 9

Which of the following is a characteristic property of bases?

Accepted Answer

They turn red litmus paper blue

Question 10

What is the product of the neutralization reaction between $$\mathrm{H_2SO_4}$$ and $$\mathrm{KOH}$$?

Accepted Answer

$$\mathrm{K_2SO_4}$$ and $$\mathrm{H_2O}$$

Question 11

A patient is suffering from acid reflux due to excess stomach acid ($$\mathrm{HCl}). $$Which of the following compounds would be most effective as an antacid?

Accepted Answer

Magnesium hydroxide ($$\mathrm{Mg(OH)_2})$$

Question 12

Which of the following best explains why a buffer solution resists changes in pH upon addition of small amounts of acid or base?

Accepted Answer

It contains a weak acid and its conjugate base

Question 13

If the pH of a solution changes from 3.0 to 2.0, what happens to the $$[\mathrm{H_3O^+}]$$ concentration?

Accepted Answer

It increases by a factor of 10

Question 14

Which of the following is the correct balanced equation for the neutralization of hydrochloric acid with calcium hydroxide?

Accepted Answer

$$\mathrm{2HCl + Ca(OH)_2 \rightarrow $$CaCl_2$$ + 2H_2O}$$

Question 15

Which of the following is the conjugate acid of $$\mathrm{NH_2$^-}$$?

Accepted Answer

$$\mathrm{NH_3$}$$

Question 16

A solution has a pH of 5.00. What is the $$[\mathrm{H_3O^+}]$$ concentration?

Accepted Answer

$$1.0 	imes 10$$^{-5}$$\ \mathrm{M}$$

Question 17

Which of the following statements about weak bases is correct?

Accepted Answer

They produce very few $$\mathrm{OH^-}$$ ions in solution

Question 18

Which of the following pairs are a conjugate acid-base pair?

Accepted Answer

$$\mathrm{H_2CO_3}$$ / $$\mathrm{$$HCO_3$$^-}$$

Question 19

Which of the following best describes a salt formed in a neutralization reaction?

Accepted Answer

An ionic compound that does not have $$\mathrm{H^+} as $$the cation or $$\mathrm{OH^-} as $$the anion

Question 20

A buffer in the blood helps maintain a pH close to 7.4. What could happen if the blood pH drops significantly below this value?

Accepted Answer

Cellular processes could be disrupted, affecting health

Acids and Bases: Arrhenius and Bronsted-Lowry Theories, Properties, and Nomenclature

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