MHT CET · Chemistry · Ionic Equilibrium
What is pH of weak dibasic acid, that is \(2 \%\) dissociated in its \(\mathrm{M} / 100\) solution at 298 K ?
- A 1.699
- B 2.3979
- C 3.397
- D 4.699
Answer & Solution
Correct Answer
(C) 3.397
Step-by-step Solution
Detailed explanation
\( [H^+] = 2 \times C \times \alpha = 2 \times 0.01 \times 0.02 = 0.0004 \ M \) \( pH = -\log[H^+] = -\log(0.0004) = 3.3979 \)
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