Given that the dissociation constant for $H_2O$ is $K_w = 1 \times 10^{-14} \ mol^2/L^2$. What is the $pH$ of a $0.001 \ M$ $KOH$ solution?

$1 \ L$ of $0.02 \ M$ aqueous $HCl$ is mixed with $1 \ L$ of $0.01 \ M$ aqueous $H_2SO_4$ solution. Assuming complete dissociation and no change in the volume upon mixing,the $pH$ of the resultant solution is $(\log_{10} 2 = 0.3)$.

The hydrogen ion concentration of a $10^{-8} \ M \ HCl$ aqueous solution at $298 \ K$ $(K_w = 10^{-14})$ is

What will be the $pH$ of a $10^{-8} \ M$ solution of $HCl$?

$10^{-6} \ M \ HCl$ is diluted $100$ times. Its $pH$ is

The $pH$ of $1 \ N$ $KOH$ solution is: