The $pH$ of $1 \ N$ $KOH$ solution is:

Water is added to $1.0 \ mL$ of $0.1 \ M$ $HCl$ solution to make the total volume $50 \ mL$. Calculate the $pH$ change of the solution.

Given $pH$ of a solution $A$ is $3$ and it is mixed with another solution $B$ having $pH$ $2$. If both are mixed in equal volumes,then the resultant $pH$ of the solution will be

When $100 \ mL$ of $0.1 \ M$ $NaOH$ is added to $50 \ mL$ of $0.2 \ M$ $HCl$ at $25 \ ^oC$,the $pH$ of the resulting solution will be:

$0.023 \ g$ of sodium metal is reacted with $100 \ cm^{3}$ of water. The $pH$ of the resulting solution is

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