TS EAMCET · Chemistry · Ionic Equilibrium
The \(\mathrm{pH}\) of \(0.01 \mathrm{M}\) solution of acetic acid is 5.0. What are the values of \(\left[\mathrm{H}^{+}\right]\)and \(K_a\) respectively?
- A \(1 \times 10^{-5} \mathrm{M}, 1 \times 10^{-8}\)
- B \(1 \times 10^{-5} \mathrm{M}, 1 \times 10^{-9}\)
- C \(1 \times 10^{-4} \mathrm{M}, 1 \times 10^{-8}\)
- D \(1 \times 10^{-3} \mathrm{M}, 1 \times 10^{-8}\)
Answer & Solution
Correct Answer
(A) \(1 \times 10^{-5} \mathrm{M}, 1 \times 10^{-8}\)
Step-by-step Solution
Detailed explanation
Given, \(\mathrm{pH}\) of \(0.01 \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}\) solution \(=5.0\) Concentration, \(C\) of the solution \(=0.01 \mathrm{M}\) \(\left[\mathrm{H}^{+}\right]=1 \times 10^{-\mathrm{pH}}\)…
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