Acid-Base Titration Quiz Online Practice Test

1. Which of the following titrations will have the equivalence point at a pH more than 8?

HCl and ammonia

Sodium hydroxide and ammonia

HCl and NaOH

Acetic acid and ammonia

2. Which of the following is used in the titration of a strong acid and a weak base?

Phenolpthalein

Thymol blue

Fluorescein

Methyl orange

3. Which of the following is used as an indicator in the titration of a weak acid and a strong base?

Bromothymol blue

Methyl orange

Methyl red

Phenolpthalein

4. The ideal indicator for titration of a strong acid and weak base should have pH range?

5-8

4-6

8-10

7-8

5. What distinguishes a strong acid from a weak acid?

Presence and absence of halogen ions

Negative and positive pH

Complete and partial ionization

Proton donation and electron acceptance

6. Which of the following is an example of a buffer solution?

NaCl + NaOH

HCl and NH4Cl

H2SO4 + CuSO4

CH3COONa + CH3COOH

7. If 20 ml of a barium hydroxide solution is titrated with 30 ml of 0.1 M HCl, what is the molarity of the barium hydroxide solution?

0.07 M

0.15 M

0.10 M

0.03 M

8. In which of the following titrations is the equivalence point expected to occur at a pH greater than 8?

HCl and NH3

CH3COOH and NH3

HCl and NaOH

CH3COOH and NaOH

9. To determine the concentration of HCl, 20 ml of 0.5 M Ca(OH)2 is needed to titrate 60 ml of HCl. What is the concentration of HCl?

0.32 M

0.17 M

0.5 M

0.05 M

10. The pH scale typically ranges from:

0 to 1

-1 to 14

0 to 7

0 to 14

11. If 20 ml of an acid requires neutralization by 10 ml of 0.2 N alkali, what is the concentration of the acid?

0.4 N

0.2 N

0.1 N

0.5 N

12. If 50 ml of a sulfuric acid solution is neutralized by 25 ml of 0.5 M Ba(OH)2 solution, what is the concentration of the sulfuric acid solution?

0.25 M

0.5 M

1 M

0.1 M

13. What is the combined concentration of H3O+ ions and OH- ions in water?

10^-28

10^-7

10.14

10^-14

14. In the given equation, how would you categorize KOH (potassium hydroxide)?
KOH(aq) —> K+(aq) + OH-(aq)

A strong base

A weak acid

A strong acid

A weak base

15. If a solution has a pH of 9, what is the concentration of OH- ions in the solution?

1 × 10^-9 M

1 × 10^9 M

9 M

1 × 10^-5 M

16. In a solution with a pH of 3, what is the ratio of the concentration of H3O+ ions to OH- ions?

1:1

1000:1

100:1

0.001:1

17. During an acid-base titration, 30 ml of 0.08 M sulfuric acid (H2SO4) is titrated with 0.15 M sodium hydroxide (NaOH). The first equivalence point is reached when 45 ml of NaOH has been added. What is the equivalent weight of sulfuric acid?

1000 g/mol

0.355556 g/mol

18 g/mol

144 g/mol

18. In an acid-base titration experiment, what effect does adding excess sodium hydroxide (NaOH) have on the calculated concentration of hydrochloric acid (HCl)?

Increases the calculated HCl concentration

Decreases the calculated HCl concentration

Has no effect on the calculated HCl concentration

Invalidates the titration results

19. In an acid-base titration, the chemist uses a strong base, sodium hydroxide (NaOH), to titrate a weak acid, acetic acid (CH3COOH). At the equivalence point, the solution's pH is measured and found to be 8.0. Which statement accurately explains this observation?

Acetic acid is a stronger acid than sodium hydroxide

The pH indicates that the solution is still acidic

Acetic acid is partially ionized, resulting in a lower pH

The equivalence point is pH-neutral, and the pH value is appropriate

20. When titrating acetic acid with NaOH using phenolphthalein as the indicator, the endpoint is pH 7.0. If the same titration is done with methyl orange as the indicator, what is the likely endpoint pH?

pH 7.0

pH 4.2

pH 2.4

pH 12.2

Test Name:	Acid-Base Titration
Subject Category:	Chemistry
Test Type:	Multiple Choice Questions
Total Score / Questions:	20 / 20
Time Allowed:	10 Min
Who Should Practice this Test:	Students, job seekers, or professionals preparing for competitive exams and interviews.