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AIIMS2018Chemistry-Acid-Base Equilibria

AIIMS 2018 Chemistry Buffer Solutions MCQ Question

Type: MCQ-numerical-Medium-Class 11

20 mL20\text{ mL} of 0.1 M0.1\text{ M} acetic acid is mixed in a solution of NaOH\text{NaOH}. If 10 mL10\text{ mL} of 0.1 M0.1\text{ M} NaOH\text{NaOH} is present, then H+\text{H}^+ concentration in the resulting solution is (Ka of acetic acid=1.7×10−5\text{K}_\text{a}\text{ of acetic acid} = 1.7 \times 10^{-5})

A

3.4×10−53.4 \times 10^{-5}

B

1.7×10−21.7 \times 10^{-2}

C

1.7×10−51.7 \times 10^{-5}

D

1.7×10−71.7 \times 10^{-7}

Correct Answer

Option C

Detailed Explanation

In the given reaction, acetic acid (CH₃COOH) reacts with sodium hydroxide (NaOH) to form sodium acetate (CH₃COONa) and water (H₂O). The pOH equation provided indicates that the pOH is influenced by the concentration of the salt (CH₃COONa) and the acid (CH₃COOH), which allows for the calculation of pH based on the dissociation constant (Kₐ) of acetic acid, given as 1.7 × 10⁻⁵ M. Option C correctly applies the Henderson-Hasselbalch equation to determine the pH of the solution, while other options may misinterpret the relationship between pH, pOH, and the concentrations of the acid and its conjugate base.

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