The $pH$ of a $0.02 \, M$ solution of hydrochloric acid is

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 $L$)?

Calculate the $pH$ of the following solutions:
$(a)$ $0.1 \ M \ HCl$
$(b)$ $0.1 \ M \ H_2SO_4$
$(c)$ $0.1 \ M \ HNO_3$
$(d)$ $0.1 \ M \ NaOH$
$(e)$ $0.1 \ M \ KOH$
$(f)$ $0.1 \ M \ Ba(OH)_2$

$50 \ mL$ of $H_2O$ is added to $50 \ mL$ of $1 \times 10^{-3} \ M$ barium hydroxide solution. What is the $pH$ of the resulting solution?

How many liters of water must be added to $1 \ L$ of an aqueous $HCl$ solution with $pH = 1$ to make the $pH$ of the resulting solution equal to $2$ (in $L$)?

$10^{-6} \ M \ NaOH$ is diluted $100$ times. The $pH$ of the diluted base is