$NaOH_{(aq)}$,$HCl_{(aq)}$ and $NaCl_{(aq)}$ concentration of each is $10^{-3} \, M$. Their $pH$ will be respectively

The $pH$ value of a $\frac{N}{10} \ NaOH$ solution is:

$40 \, mg$ of pure sodium hydroxide is dissolved in $10 \, L$ of distilled water. The $pH$ of the solution is

At $27^{\circ} C$, $100 \ mL$ of $0.5 \ M$ $HCl$ is mixed with $100 \ mL$ of $0.4 \ M$ $NaOH$ solution. To this resultant solution, $800 \ mL$ of distilled water is added. What is the $pH$ of the final solution?

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.

What is the $pH$ of a $10^{-4} \ M \ OH^{-}$ solution at $330 \ K$,if $K_w$ at $330 \ K$ is $10^{-13.6}$?