Question

If $3.65g$ $HCl$ is added to $1L$ of water at ${60}^{o}C$ and the pH of water is ${10}^{-5}$. What will be the pH of resultant solution at ${60}^{o}C$.

Answer 1

$3.65g$ of $HCl⟹0.1mol$ of $HCl$

$pH\left(H_{2}O\right)={10}^{-5}$

$H_{2}O=\left[H^{+}\right]\cong 0$

$1$ $L$ of water

$HCl+H_{2}O\leftrightharpoons H_3{O}^{+}+C{l}^{-}$

$\left[H^{+}\right]=\frac{0.1mole}{1Liter}$

$pH=-log{10}^{-1}$

$pH=1$

$pH$ of resultant solution at $60°C=1$