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MHT CET 202623 AprilEvening Shift
Exam
MHT CET
Year
2026
Date
23 April
Shift
Evening Shift
Subject
Chemistry
Chapter
Ionic Equilibrium

MHT CET 2026 · 23 April · Evening Shift · Chemistry · Ionic Equilibrium

Calculate the pH of the buffer solution consists of 0.005 M weak...

Calculate the pH of the buffer solution consists of 0.005 M weak acid and 0.02 M of its salt with strong base BA. [pKa=3.4437\text{p}K_a = 3.4437]

Options

  1. A4.0464.046
  2. B2.8422.842
  3. C3.74473.7447
  4. D3.14373.1437

Correct answer

A. 4.0464.046

Step-by-step solution

Using the Henderson-Hasselbalch equation for an acidic buffer:

pH=pKa+log⁡([Salt][Acid])<br><br>Given:<br><br>p\text{pH} = \text{p}K_a + \log \left(\dfrac{[\text{Salt}]}{[\text{Acid}]}\right)<br><br>Given:<br><br>\text{p} K_a = 3.4437<br><br><br><br>[Salt]=0.02 M<br><br>\text{Salt}] =0.02 \text{ M}<br><br>[Acid]=0.005 M<br><br>Substitutingthevalues:<br><br>pH=3.4437+log⁡(0.020.005)\text{Acid}] =0.005 \text{ M}<br><br>Substituting the values:<br><br>\text{pH} =3.4437 + \log \left(\dfrac{0.02}{0.005}\right)

pH=3.4437+log⁡(4)\text{pH} = 3.4437 + \log(4)

pH=3.4437+0.6021\text{pH} = 3.4437 + 0.6021

pH=4.0458≈4.046\text{pH} = 4.0458 \approx 4.046

Answer: 4.0464.046
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