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MHT CET Medical202623 April 2026Evening ShiftChemistryIonic EquilibriumActual

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. [ p K_a = 3.4437 ]

Options

  1. A4.046
  2. B2.842
  3. C3.7447
  4. D3.1437

Correct answer

A. 4.046

Step-by-step solution

Using the Henderson-Hasselbalch equation for an acidic buffer: pH = p K_a + ( [ Salt ] [ Acid ] ) Given: p K_a = 3.4437 [ Salt ] = 0.02 M [ Acid ] = 0.005 M Substituting the values: pH = 3.4437 + ( 0.02 0.005 ) pH = 3.4437 + (4) pH = 3.4437 + 0.6021 pH = 4.0458 4.046 Answer: 4.046

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