WBJEE · Chemistry · Ionic Equilibrium
\(0.1(\mathrm{M}) \mathrm{HCI}\) and \(0.1(\mathrm{M}) \mathrm{H}_2 \mathrm{SO}_4\) each of volume \(2 \mathrm{ml}\) are mixed and the volume is made up to \(6 \mathrm{ml}\) by adding \(2 \mathrm{ml}\) of \(0.01(\mathrm{~N}) \mathrm{NaCl}\) solution. The \(\mathrm{pH}\) of the resulting mixture is
- A 1.17
- B 1
- C 0.3
- D \(\log 2-\log 3\)
Answer & Solution
Correct Answer
(B) 1
Step-by-step Solution
Detailed explanation
Hints: Mili moles of \(\mathrm{H}^{+}=0.1 \times 2+0.1 \times 2 \times 2=0.6\) Total volume in \(\mathrm{ml}=6\) \[ \mathrm{pH}=-\log _{10}\left[\mathrm{H}^{+}\right]=-\log \left(\frac{0.6}{6}\right)=-\log 0.1=1 \]
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