What is the $pH$ of a solution in which $25.0 \ mL$ of $0.1 \ M \ NaOH$ is added to $25 \ mL$ of $0.08 \ M \ HCl$ and the final solution is diluted to $500 \ mL$?

What is the $pH$ of $0.005 \ M \ H_2SO_4$ solution?

$A$ solution with $pH = 5.0$ is diluted $100$ times. Calculate the $pH$ of the diluted solution.

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

Calculate the $pH$ of $1.36 \times 10^{-2} \ M$ solution of perchloric acid.

An aqueous solution of $HCl$ with $pH \ 1.0$ is diluted by adding an equal volume of water (ignoring the dissociation of water). The $pH$ of the $HCl$ solution would be (Given $\log 2 = 0.30$):