Q: A solution has $$[\mathrm{OH^-}] = 5.0 \times 10$$^{-8}$$\ \mathrm{M}. $$What is $$[\mathrm{H_3O^+}] in $$this solution at 25°C?

$$2.0 \times 10$$^{-7}$$\ \mathrm{M}$$

Q: Which of the following solutions is basic?

$$[\mathrm{H_3O^+}] = 1 \times 10$$^{-8}$$\ \mathrm{M}$$

Question 1

Which of the following statements best describes the Brønsted–Lowry definition of acids and bases?

Accepted Answer

Acids donate H+ ions, bases accept H+ ions.

Question 2

A clinical laboratory technician is preparing a blood sample for analysis. Why is it important to understand acid–base equilibrium in this context?

Accepted Answer

Blood pH must be maintained within a narrow range for proper physiological function.

Question 3

Which acid is correctly named according to the rules for acids containing a hydrogen ion and a polyatomic ion ending in 'ate'?

Accepted Answer

H2SO4: Sulfuric acid

Question 4

Which of the following is a characteristic of Arrhenius bases?

Accepted Answer

They produce OH− ions in water.

Question 5

Given the reaction $$\mathrm{HF(aq) + H_2O(l) \rightleftharpoons F^-(aq) + H_3O^+(aq)}$$, which pair represents the conjugate acid–base pair?

Accepted Answer

HF and F−

Question 6

Which of the following acids is classified as a weak acid?

Accepted Answer

HF

Question 7

A solution has $$[\mathrm{OH^-}] = 5.0 	imes 10$$^{-8}$$\ \mathrm{M}. $$What is $$[\mathrm{H_3O^+}] in $$this solution at 25°C?

Accepted Answer

$$2.0 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 8

Which of the following solutions is basic?

Accepted Answer

$$[\mathrm{H_3O^+}] = 1 	imes 10$$^{-8}$$\ \mathrm{M}$$

Question 9

Calculate the pH of a solution with $$[\mathrm{H_3O^+}] = 4.0 	imes 10$$^{-5}$$\ \mathrm{M}.$$

Accepted Answer

pH = 4.40

Question 10

Which combination below forms a buffer solution?

Accepted Answer

H2CO3 and NaHCO3

Question 11

A titration requires 25.5 mL of 0.438 M NaOH to neutralize 0.0250 L of HCl. What is the molarity of the HCl solution?

Accepted Answer

0.447 M

Question 12

Which equation represents the net ionic equation for the neutralization of HCl and NaOH?

Accepted Answer

$$\mathrm{H^+(aq) + OH^-(aq) \rightarrow H_2O(l)}$$

Question 13

According to Le Châtelier’s principle, what happens to the equilibrium $$\mathrm{HF(aq) + H_2O(l) \rightleftharpoons F^-(aq) + H_3O^+(aq)} if $$more HF is added?

Accepted Answer

The system shifts toward the products.

Question 14

Which of the following is a correct statement about the pH scale?

Accepted Answer

A solution with pH 2 has a higher $$[\mathrm{H_3O^+}]$$ than a solution with pH 4.

Question 15

Which of the following is NOT a property of acids?

Accepted Answer

They produce OH− ions in water.

Question 16

Which of the following reactions represents the neutralization of acetic acid with sodium hydroxide?

Accepted Answer

$$\mathrm{HC_2H_3O_2(aq) + NaOH(aq) \rightarrow NaC_2H_3O_2(aq) + H_2O(l)}$$

Question 17

Which of the following statements about buffers is correct?

Accepted Answer

Buffers maintain pH by neutralizing small amounts of added acid or base.

Question 18

Which of the following is the correct formula for the ion product constant for water ($$K_w) at 25$$°C?

Accepted Answer

$$K_w = [\mathrm{H_3O^+}] 	imes [\mathrm{OH^-}]$$

Acids, Bases, and Equilibrium: Comprehensive Study Notes

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