20 mL of 0.1 M \(\mathrm{H_2SO_4}\) solution is added to 30 mL of of 0.2 M \(\mathrm{NH_4OH}\) solution. The pH of the resultant mixture is : [\(\mathrm{pk_b}\) of \(\mathrm{NH_4OH}\) = 4.7].
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- 5.2
- 9.0
- 5.0
- 9.4
The Correct Option is B
Solution and Explanation
\(\mathrm{NH_4OH + H^+ \rightarrow NH_4^+ + H_2O}\): remaining \(\mathrm{NH_4OH}\) = 6 - 4 = 2 mmol; \(\mathrm{NH_4^+}\) formed = 4 mmol.
This is a basic buffer: \(\mathrm{pOH = pK_b + \log\dfrac{[salt]}{[base]} = 4.7 + \log\dfrac{4}{2} = 4.7 + 0.3 = 5.0}\).
pH = 14 - 5.0 = 9.0.
Answer: (2) 9.0
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