Assuming complete dissociation,the $pH$ of a $0.01 \, M$ $NaOH$ solution is equal to

The $pH$ of a $H_2SO_4$ solution is $5.0$. If more $H_2SO_4$ is added to this solution,the $pH$ becomes $2.0$. The concentration of $H^{+}$ ions will become how many times the initial concentration?

Which of the following,when added to $10 \ mL$ of dilute $HCl$,will not change the $pH$ of the solution?

The $pH$ of $10^{-8} \ M$ aqueous solution of $HCl$ is

The $pH$ of $10^{-8} \ M \ HCl$ solution is

Calculate the $pH$ of $0.0035 \ M \ Ba(OH)_2$ solution.