Acid-Base Titration MCQs

Acid-base titration involves a neutralization reaction where an acid or base of known concentration is used to determine the concentration of an unknown acid or base. During the titration, a few drops of an indicator are added, which changes color to signal the endpoint. The indicator reacts to changes in the pH of the solution. To accurately determine the equivalence point and minimize errors, it is essential to choose an appropriate indicator.

The ideal indicator for the titration of strong acid and weak base should have pH range between

(a) 5-8
(b) 4-6
(c) 8-10
(d) 7-8

(b) 4-6

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

(a) Phenolphthalein
(b) Thymol blue
(c) Fluorescein
(d) Methyl orange

(d) Methyl orange

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

(a) HCl and NH3
(b) CH3COOH and NH3
(c) HCl and NaOH
(d) CH3COOH and NaOH

(d) CH3COOH and NaOH

What is the molarity of the solution of barium hydroxide, if 35 ml of 0.1 M HCl is used in the titration of 25 ml of the barium hydroxide solution?

(a) 0.35
(b) 0.07
(c) 0.28
(d) 0.14

(b) 0.07

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

(a) Bromothymol blue (6 to 7.5)
(b) Methyl orange (3 to 4)
(c) Methyl red (5 to 6)
(d) Phenolphthalein (8 to 9.6)

(d) Phenolphthalein (8 to 9.6)

What is the concentration of the sulphuric acid solution, if 100 ml of the solution is neutralised by 50 ml of 0.5 M Ba(OH)2 solution?

(a) 0.25 M
(b) 50 M
(c) 0.5 M
(d) 100 M

(a) 0.25 M

A difference between strong and weak acid is

(a) presence and absence of halogen ions
(b) negative and positive pH
(c) complete and partial ionisation
(d) proton donation and electron acceptance

(c) complete and partial ionisation

Which of the following is a buffer solution?

(a) H2SO4 + CuSO4
(b) CH3COOH + CH3COONH4
(c) NaCl + NaOH
(d) CH3COONa + CH3COOH

(d) CH3COONa + CH3COOH

If 30 ml of acid is neutralised by 15 ml of 0.2 N alkali, then the concentration of acid is

(a) 0.4 N
(b) 0.1 N
(c) 0.3 N
(d) 0.15 N

(b) 0.1 N

Find the concentration of HCl, if 10 ml of 0.5 M Ca(OH)2 is required to titrate 50 ml of HCl.

(a) 5 M
(b) 1/10 M
(c) 10 M
(d) 1/5 M

(d) 1/5 M