AIIMS2014Chemistry-Buffers
AIIMS 2014 Chemistry Buffers MCQ Question
Type: MCQ-conceptual-Medium-Class 11
In a basic buffer, 0.0025 mole of NH4Cl and 0.15 mole of NH4OH are present. The pH of the solution will be (pKa) = 4.74.
A
11.04
B
10.24
C
6.62
D
5.48
Correct Answer
Option A
Detailed Explanation
The correct answer is A) 11.04 because in a basic buffer solution, the pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([base]/[acid]). In this case, NH4OH acts as the base and NH4Cl provides the conjugate acid (NH4+). With the given concentrations, we find that the pH is significantly higher than 7, resulting in a pH of approximately 11.04, indicating a basic solution.
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