Question 1

Which of the following best describes the purpose of a strong acid-strong base titration in a laboratory setting?

Accepted Answer

To determine the unknown concentration of an acid or base by reacting it with a solution of known concentration.

Question 2

A student titrates 25.0 mL of 0.500 M HCl with 1.00 M NaOH. How many milliliters of NaOH are required to reach the equivalence point?

$$\mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{NaCl} + \mathrm{H_2O}$$

Accepted Answer

$$12.5\ \mathrm{mL}$$

Question 3

Which equation correctly represents the neutralization reaction between a strong acid and a strong base?

Accepted Answer

$$\mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{NaCl} + \mathrm{H_2O}$$

Question 4

At the equivalence point of a titration between a strong acid and a strong base, what is the expected pH of the solution?

Accepted Answer

$$\mathrm{pH} = 7$$

Question 5

If 24.9 mL of 0.100 M HNO$$_3 is $$added to 25.0 mL of 0.100 M KOH, what is the resulting solution's pH? (Assume complete reaction.)

Accepted Answer

The solution is slightly acidic, $$\mathrm{pH} \u003c 7$$

Question 6

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

Accepted Answer

The resulting solution contains only neutral ions and water.

Question 7

A titration curve for a strong acid-strong base titration shows a sharp rise in pH near the equivalence point. What does this indicate about the reaction?

Accepted Answer

The reaction between the acid and base is rapid and complete.

Question 8

Which laboratory apparatus is used to deliver a measured volume of titrant during a titration, as shown in the first image?

Accepted Answer

Buret

Question 9

During a titration, why is an indicator added to the solution in the Erlenmeyer flask?

Accepted Answer

To visually signal the endpoint of the titration by changing color.

Question 10

A student adds 25.1 mL of 0.100 M HNO$$_3 to 25.0 mL of 0.100 M $$KOH. What is the pH of the resulting solution?

Accepted Answer

The solution is slightly acidic, $$\mathrm{pH} \u003c 7$$

Question 11

Which of the following best describes what happens at the molecular level at the equivalence point in a strong acid-strong base titration?

Accepted Answer

All the H$$^+$$ ions have reacted with all the OH$$^-$$ ions to form water.

Question 12

If a student uses a buret to add NaOH to HCl in an Erlenmeyer flask, which of the following errors would cause the calculated concentration of HCl to be too high?

Accepted Answer

Recording a final buret reading that is lower than the actual value.

Question 13

Which of the following is a correct calculation for the number of moles of NaOH required to neutralize 0.0250 L of 0.500 M HCl?

Accepted Answer

$$0.0125\ \mathrm{mol}$$

Question 14

In a titration of a strong base with a strong acid, what is the pH at the equivalence point, and why?

Accepted Answer

$$\mathrm{pH} = 7$$ because the resulting solution contains only neutral ions and water.

Question 15

A titration curve for a strong acid-strong base titration is shown. What does the steep vertical region of the curve represent?

Accepted Answer

The rapid change in pH near the equivalence point.

Strong Acid-Strong Base Titrations: Principles, Calculations, and Laboratory Setup

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