Q18 / 75 · JEE Main 2025 (7 Apr Shift 1) · Chemistry
An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would
(Given $\log 2=0.30)$
(Given $\log 2=0.30)$
- Areduce to $0.5$
- Correct answerBincrease to $1.3$
- Cremain same
- Dincrease to $2$
Solution
$\mathrm{HCl}_{(\mathrm{aq})} \mathrm{pH}=1 ;\left[\mathrm{H}^{+}\right]=10^{-1}$
If equal volume of water is added concentration will become half
$\begin{aligned}& {\left[\mathrm{H}^{+}\right]_{\mathrm{sol}}=\frac{10^{-1}}{2}} \\& \mathrm{pH}=1.3\end{aligned}$
If equal volume of water is added concentration will become half
$\begin{aligned}& {\left[\mathrm{H}^{+}\right]_{\mathrm{sol}}=\frac{10^{-1}}{2}} \\& \mathrm{pH}=1.3\end{aligned}$
Hence, the correct answer is option: 'B'.