What is the $pH$ of the resulting solution when equal volumes of $0.1 \ M \ NaOH$ and $0.01 \ M \ HCl$ are mixed?

Calculate the $pH$ of the following solutions:
$(a)$ $2 \,g$ of $TlOH$ dissolved in water to give $2 \,L$ of solution.
$(b)$ $0.3 \,g$ of $Ca(OH)_2$ dissolved in water to give $500 \,mL$ of solution.
$(c)$ $0.3 \,g$ of $NaOH$ dissolved in water to give $200 \,mL$ of solution.
$(d)$ $1 \,mL$ of $13.6 \,M \,HCl$ is diluted with water to give $1 \,L$ of solution.

The $pH$ of a $10^{-8} \ M \ HCl$ aqueous solution is ......

The $pH$ value of $0.1 \, M \, HCl$ is approximately $1$. What will be the approximate $pH$ value of $0.05 \, M \, H_2SO_4$?

Which of the following statements is not correct?

When a $10^{-6} \ M \ NaOH$ solution is diluted $100$ times,the $pH$ of the diluted solution will be ............ .