Question 1

Which of the following best describes the pH at the equivalence point when titrating a strong acid with a strong base?

Accepted Answer

The pH will be exactly 7 because both the acid and base are strong.

Question 2

During the titration of 100 mL of 0.500 M HBr with 120 mL of 0.450 M KOH, which species will be in excess after the reaction is complete?

Accepted Answer

$$\mathrm{KOH}$$

Question 3

Which of the following combinations would result in a solution with pH = 7 at the equivalence point?

Accepted Answer

HCl and NaOH

Question 4

What is the net ionic equation for the reaction between a strong acid and a strong base?

Accepted Answer

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

Question 5

If you titrate 50.0 mL of 0.200 M HCl with 0.100 M NaOH, what volume of NaOH is required to reach the equivalence point?

Accepted Answer

$$100.0\ \mathrm{mL}$$

Question 6

Which statement best explains why the pH changes rapidly near the equivalence point in a strong acid–strong base titration?

Accepted Answer

The concentrations of acid and base are both very low, so small additions cause large pH changes.

Question 7

A student titrates 25.0 mL of 0.100 M KOH with 0.100 M HNO$$_3. $$What is the pH at the equivalence point?

Accepted Answer

$$\mathrm{pH} = 7$$

Question 8

Which of the following best describes the shape of the titration curve for a strong acid titrated with a strong base?

Accepted Answer

A sharp, nearly vertical rise in pH at the equivalence point.

Question 9

If 0.050 mol of HCl is mixed with 0.060 mol of NaOH in water, what will be the final solution's pH?

Accepted Answer

The solution will be basic because there is excess NaOH.

Question 10

Which of the following is true about the equivalence point in a titration between a strong acid and a strong base?

Accepted Answer

All the acid has been neutralized by the base.

Question 11

A titration curve for a strong base titrated with a strong acid will show:

Accepted Answer

A sharp decrease in pH at the equivalence point.

Question 12

Which indicator would be most appropriate for a strong acid–strong base titration?

Accepted Answer

Bromothymol blue (pH transition 6.0–7.6)

Question 13

If you titrate 100 mL of 0.500 M HBr with 0.450 M KOH, how many moles of KOH are required to reach the equivalence point?

Accepted Answer

$$0.0500\ \mathrm{mol}$$

Question 14

Which of the following best explains why the equivalence point for a strong acid–strong base titration is at pH 7?

Accepted Answer

The salt formed does not hydrolyze in water.

Question 15

A chemist titrates 0.0250 L of 0.200 M NaOH with 0.100 M HCl. What volume of HCl is needed to reach the equivalence point?

Accepted Answer

$$0.0500\ \mathrm{L}$$

Strong Titrant–Strong Titrant Curves in Acid-Base Titrations

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