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?

Five solutions of $KOH$ are prepared as follows: $1st \to 0.1 \ mol$ in $1 \ L$,$2nd \to 0.2 \ mol$ in $2 \ L$,$3rd \to 0.3 \ mol$ in $3 \ L$,$4th \to 0.4 \ mol$ in $4 \ L$,$5th \to 0.5 \ mol$ in $5 \ L$. What is the $pH$ of the resulting mixture?

What is the $pH$ of $1 \times 10^{-4} \ M \ H_2SO_4$ solution?

The $pH$ of $1 \ L$ of an aqueous solution of $HCl$ is $1$. How many liters of water must be added to make the $pH$ of this solution $2$ (in $L$)?

$50 \ mL$ of water is added to $50 \ mL$ of $0.01 \ M$ $Ba(OH)_2$ solution. Calculate the $pH$ of the resulting solution.

Concentration of $H^{+}$ ions in $10^{-4} \ M \ HCl$ solution is