$200 \ mL$ of $0.01 \ M \ HCl$ is mixed with $400 \ mL$ of $0.01 \ M \ H_{2}SO_{4}$. The $pH$ of the mixture is

Aqueous solution of $HCl$ has the $pH = 4$. Its molarity would be (in $, M$)

$A$ base dissolved in water yields a solution with a hydroxyl ion concentration of $0.05 \ mol \ L^{-1}$. The solution is

The $pH$ of a $10 \ mL$ aqueous solution of $HCl$ is $4$. The amount of water to be added to this solution in order to change its $pH$ from $4$ to $5$ is $..... \ mL$

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

Given below are two statements:
Statement-$I$: $pH$ of a $1.0 \times 10^{-8} \ M$ solution of $HCl$ is $8$ at $25^{\circ} C$.
Statement-$II$: $HCl$ is a strong acid and negative log of $H^{+}$ concentration is called $pH$.
In the light of the above statements,choose the most appropriate answer from the options given below: