$10^{-6} \ M \ NaOH$ is diluted $100$ times. The $pH$ of the diluted base is

$0.1 \ (M) \ HCl$ and $0.1 \ (M) \ H_2SO_4$ each of volume $2 \ mL$ are mixed and the volume is made up to $6 \ mL$ by adding $2 \ mL$ of $0.01 \ (N) \ NaCl$ solution. The $pH$ of the resulting mixture is

The $pH$ values of $(i) \ 0.1 \ M \ HCl_{(aq)}$,$(ii) \ 0.1 \ M \ KOH$,$(iii)$ tomato juice,and $(iv)$ pure water follow the order.

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 $\log 2 = 0.30$):

The $pH$ of a $0.001 \, M$ solution of $HCl$ is:

Which would decrease the $pH$ of $25 \ cm^3$ of a $0.01 \ M$ solution of hydrochloric acid?