What is the $pH$ of $1 \times 10^{-4} \ M \ H_2SO_4$ solution?

Which of the following solutions will have the maximum $pH$?

The $pH$ of a completely dissociated $0.005 \ M \ H_2SO_4$ solution is:

$0.1 \ mL$ of $0.001 \ M$ $HCl$ solution is diluted with water to form $10 \ L$. Calculate the $pH$ of the dilute solution.

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

Following solutions were prepared by mixing different volumes of $NaOH$ and $HCl$ of different concentrations:
$a. \; 60 \; mL \; \frac{M}{10} \; HCl + 40 \; mL \; \frac{M}{10} \; NaOH$
$b. \; 55 \; mL \; \frac{M}{10} \; HCl + 45 \; mL \; \frac{M}{10} \; NaOH$
$c. \; 75 \; mL \; \frac{M}{5} \; HCl + 25 \; mL \; \frac{M}{5} \; NaOH$
$d. \; 100 \; mL \; \frac{M}{10} \; HCl + 100 \; mL \; \frac{M}{10} \; NaOH$
$pH$ of which one of them will be equal to $1$?