Question 1

A solution is prepared by combining approximately equal amounts of carbonic acid and sodium bicarbonate in water. The addition of a small amount of HCl to this buffer solution causes the pH to rise slightly. The pH does not increase drastically because the HCl reacts with the ________ present in the buffer solution.

Accepted Answer

Sodium bicarbonate

Question 2

Calculate the pH of a solution that is 0.38 M in carbonic acid ($$\mathrm{H_2CO_3}) $$and 0.18 M in sodium bicarbonate ($$\mathrm{$$NaHCO_3$$}). $$The $$K_a of $$carbonic acid is $$4.3 	imes 10$$^{-7}$$.

Accepted Answer

5.74

Question 3

What is the approximate pH at the equivalence point of a weak acid–strong base titration if 25 mL of aqueous acetic acid requires 35 mL of 0.12 M NaOH to reach the equivalence point? $$K_a = 1.8 	imes 10$$^{-5}$$ for acetic acid.

Accepted Answer

8.72

Question 4

The addition of which of the following would destroy a 1.0 L buffer solution that is 0.080 M $$\mathrm{CH_3COOH}$$ and 0.160 M $$\mathrm{CH_3COONa}$$?

Accepted Answer

Adding 0.080 mol HCl

Question 5

Calculate the volume of 0.500 M KOH required to reach the equivalence point in the titration of 50.0 mL of 0.500 M HCl.

Accepted Answer

25.0 mL

Question 6

For a titration of a weak acid with a strong base, the pH at the equivalence point is _______.

Accepted Answer

Above 7

Question 7

Which of the following acids is the strongest?

Accepted Answer

$$\mathrm{HF}$$

Question 8

Which of the following is the strongest base?

Accepted Answer

$$\mathrm{NH_2$^-}$$

Question 9

Which order correctly ranks these acids from strongest to weakest?

Accepted Answer

$$\mathrm{HI \u003e HBr \u003e HCl \u003e HF}$$

Question 10

Which pair represents a conjugate acid–base pair?

Accepted Answer

Question 11

Which statement is correct?

Accepted Answer

Strong acids have weak conjugate bases

Question 12

Adding $$\mathrm{NH_4Cl} to a $$solution of $$\mathrm{NH_3$}$$ will:

Accepted Answer

Decrease pH

Question 13

What happens when NaF is added to a solution of HF?

Accepted Answer

pH increases

Question 14

What is the pH of a solution of NaF?

Accepted Answer

Basic

Question 15

Which salt will produce a basic solution?

Accepted Answer

$$\mathrm{CH_3COONa}$$

Question 16

Given the following reaction, identify the Brønsted-Lowry acid and its conjugate base.

$$\mathrm{$$HCHO_2$$ (aq) + H_2O (l) \rightleftharpoons H_3O^+ (aq) + $$CHO_2$$^- (aq)}$$

Accepted Answer

$$\mathrm{$$HCHO_2$$ / $$CHO_2$$^-}$$

Question 17

A weak unknown monoprotic acid is titrated with a strong base. The titration curve is shown. Find $$K_a$$ for the unknown acid.

Accepted Answer

$$2.5 	imes 10$$^{-5}$$

Question 18

A buffer solution is made by mixing equal concentrations of a weak acid and its conjugate base. If a small amount of strong base is added, what will happen to the pH?

Accepted Answer

The pH will increase slightly

Question 19

Which of the following best explains why the pH at the equivalence point in the titration of a weak acid with a strong base is greater than 7?

Accepted Answer

The conjugate base of the weak acid hydrolyzes to produce $$\mathrm{OH^-}$$ ions

Acids, Bases, Buffers, and Titration – Step-by-Step Study Guidance

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