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

For a solution of $HCl$ assuming complete ionization,the $pH = 1$. Find the normality of a $H_2SO_4$ solution having the same $pH$.

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?

Millimoles of calcium hydroxide required to produce $100 \ mL$ of the aqueous solution of $pH$ $12$ is $x \times 10^{-1}$. The value of $x$ is $..............$. (Nearest integer). Assume complete dissociation.

$1.825 \ g$ of $HCl$ is dissolved in $5 \ L$ of water. What are the concentrations of $H^+$ and $OH^-$ ions?

Assuming complete dissociation,calculate the $pH$ of the following solutions:
$(i) \ 0.003 \ M \ HCl$
$(ii) \ 0.005 \ M \ NaOH$
$(iii) \ 0.002 \ M \ HBr$
$(iv) \ 0.002 \ M \ KOH$