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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