Q: What is the pH of a solution with [H$$_3O$^+$$] = $$5.0 \times 10$$^{-3}$$ M?

$$pH = -\log(5.0 \times 10$$^{-3}$$) = 2.30$$

Q: What is the pH of a solution with [OH$$^-$$] = $$3.0 \times 10$$^{-8}$$ M?

$$pOH = -\log(3.0 \times 10$$^{-8}$$) = 7.52$$, $$pH = 14 - 7.52 = 6.48$$

Q: A titration requires 23.50 mL of 0.10 M NaOH to neutralize 50.00 mL of HCl. What is the molarity of the HCl solution?

$$M_{HCl} = \frac{0.02350 \times 0.10}{0.05000} = 0.047 M$$

Question 1

Which of the following best describes a Brønsted-Lowry acid?

Accepted Answer

A substance that donates a proton (H$$^+) to $$another species

Question 2

Which hydrogen in acetic acid (CH$$_3$$COOH) is considered acidic?

Accepted Answer

The hydrogen attached to the oxygen atom in the carboxyl group

Question 3

Which of the following is a correct conjugate acid-base pair?

Accepted Answer

NH$$_3$$ and NH$$_4^+$$

Question 4

What is the pH of a solution with [H$$_3O$^+$$] = $$5.0 	imes 10$$^{-3}$$ M?

Accepted Answer

$$pH = -\log(5.0 	imes 10$$^{-3}$$) = 2.30$$

Question 5

Which of the following combinations will produce a buffer solution?

Accepted Answer

H$$_2CO$_3$$ and NaHCO$$_3$$

Question 6

A 0.15 M solution of H$$^+$$ has a pH of:

Accepted Answer

$$pH = -\log(0.15) = 0.82$$

Question 7

Which of the following acids is triprotic?

Accepted Answer

H$$_3PO$_4$$

Question 8

What is the pH of a solution with [OH$$^-$$] = $$3.0 	imes 10$$^{-8}$$ M?

Accepted Answer

$$pOH = -\log(3.0 	imes 10$$^{-8}$$) = 7.52$$, $$pH = 14 - 7.52 = 6.48$$

Question 9

Which of the following is a strong base?

Accepted Answer

NaOH

Question 10

In the reaction: $$2K(s) + 2HCl(aq) \rightarrow 2KCl(aq) + H_2$(g)$$, what is the role of HCl?

Accepted Answer

It acts as an acid, donating protons to potassium

Question 11

Which of the following best describes the effect of adding more HF to the equilibrium: $$HF(aq) + H_2O(l) \rightleftharpoons F^-(aq) + H_3O^+(aq)$$?

Accepted Answer

The rate of the forward reaction increases

Question 12

A titration requires 23.50 mL of 0.10 M NaOH to neutralize 50.00 mL of HCl. What is the molarity of the HCl solution?

Accepted Answer

$$M_{HCl} = \frac{0.02350 	imes 0.10}{0.05000} = 0.047 M$$

Question 13

Which of the following is the correct name for HClO$$_3$$?

Accepted Answer

Chloric acid

Question 14

Which of the following statements about buffer solutions is correct?

Accepted Answer

Buffers resist changes in pH when small amounts of acid or base are added

Question 15

How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H$$_2SO$_4$$? (Assume complete neutralization.)

Accepted Answer

80.0 mL

Question 16

Which of the following is the correct expression for the self-ionization constant of water ($$K_w$$)?

Accepted Answer

$$K_w = [H_3O^+][OH^-]$$

Question 17

Which of the following is a weak acid?

Accepted Answer

HF

Question 18

A buffer solution is prepared by mixing acetic acid and sodium acetate. What happens when a small amount of HCl is added to this buffer?

Accepted Answer

The added H$$^+ is $$neutralized by the acetate ion, so the pH changes only slightly

Question 19

Which of the following best describes the effect of removing some F$$^-$$ from the equilibrium: $$HF(aq) + H_2O(l) \rightleftharpoons F^-(aq) + H_3O^+(aq)$$?

Accepted Answer

The equilibrium shifts to the right, producing more F$$^-$$ and H$$_3O$^+$$

Acids, Bases, and Equilibrium: Study Notes for General Chemistry

Study Guide - Practice Questions

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