Q: In the titration of $H_2SO_4$ with $NaOH$, what is the stoichiometric relationship at the equivalence point?

$2\ \text{mol}\ NaOH = 1\ \text{mol}\ H_2SO_4$

Question 1

During an acid-base titration, what is the equivalence point?

Accepted Answer

The point where the moles of acid equal the moles of base.

Question 2

Which formula is used to calculate the volume of titrant required to reach the equivalence point in a titration?

Accepted Answer

$M_1V_1/n_1 = M_2V_2/n_2$

Question 3

A student titrates 40.0 mL of 0.0500 M HCl with 0.100 M NaOH. How many milliliters of NaOH are required to reach the equivalence point?

Accepted Answer

$20.0\ 	ext{mL}$

Question 4

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

Accepted Answer

A sharp vertical rise in pH near the equivalence point.

Question 5

In a titration of 100.0 mL of 0.40 M HCl with 0.40 M NaOH, what volume of NaOH is needed to reach the equivalence point?

Accepted Answer

$100.0\ 	ext{mL}$

Question 6

If a titration curve shows a pH jump from 3 to 11 at the equivalence point, which combination of titrant and analyte is most likely?

Accepted Answer

Strong acid titrated with strong base

Question 7

Which of the following is a correct application of the equivalence point volume formula for a diprotic acid titrated with a monoprotic base?

Accepted Answer

$M_1V_1/2 = M_2V_2$

Question 8

A titration curve for a strong acid-strong base titration typically has which key feature?

Accepted Answer

A steep vertical section at the equivalence point.

Question 9

In the titration of $H_2SO_4$ with $NaOH$, what is the stoichiometric relationship at the equivalence point?

Accepted Answer

$2\ 	ext{mol}\ NaOH = 1\ 	ext{mol}\ H_2SO_4$

Question 10

Which of the following statements about acid-base titration curves is correct?

Accepted Answer

The shape of the curve depends on both the strength and type of acid and base.

Question 11

A student is titrating 50.0 mL of 0.100 M $CH_3COOH$ (acetic acid) with 0.100 M $NaOH$. What is the volume of $NaOH$ required to reach the equivalence point?

Accepted Answer

$50.0\ 	ext{mL}$

Question 12

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

Accepted Answer

Phenolphthalein

Question 13

If 0.100 M $NaOH$ is used to titrate 0.0500 M $HCl$, and 40.0 mL of $HCl$ is present, what is the number of moles of $NaOH$ required at the equivalence point?

Accepted Answer

$0.00200\ 	ext{mol}$

Question 14

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

Accepted Answer

The resulting solution contains only water and neutral salt.

Question 15

A titration curve for a weak acid titrated with a strong base will have which distinguishing feature?

Accepted Answer

A buffer region before the equivalence point.

Question 16

In a titration, what is the primary purpose of using an indicator?

Accepted Answer

To visually signal the approach or arrival at the equivalence point.

Question 17

A student titrates 25.0 mL of 0.200 M $H_2SO_4$ with 0.100 M $NaOH$. What volume of $NaOH$ is required to reach the equivalence point?

Accepted Answer

$100.0\ 	ext{mL}$

Question 18

Which of the following is NOT a factor that affects the shape of a titration curve?

Accepted Answer

Color of the indicator

Question 19

In a titration experiment, why is it important to add the titrant slowly near the equivalence point?

Accepted Answer

To avoid overshooting the equivalence point due to rapid pH change.

Question 20

Which of the following best describes the equivalence point in the titration of a diprotic acid with a monoprotic base?

Accepted Answer

It occurs when twice as many moles of base have been added as acid.

Acid-Base Titration Curves and Equivalence Point Calculations

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