If the $pH$ of a solution is $2$,find the $[H^{+}]$ of the solution.

If $pOH$ of a solution is $6.0$,then its $pH$ will be

At $90\,^oC$,the $pH$ of a $0.1\,M$ $NaCl$ aqueous solution is .......

The value of the ion product constant for water,$(K_w)$ at $60\,^{\circ}C$ is $9.6 \times 10^{-14} \,M^2$. What are the $[H_3O^{+}]$ of a neutral aqueous solution at $60\,^{\circ}C$ and the nature of an aqueous solution with a $pH = 7.0$ at $60\,^{\circ}C$,respectively?

Observe the following solutions:
$I$. Black coffee
$II$. $0.2 \ M \ NaOH$
$III$. Lemon juice
$IV$. Lime water
$V$. Human Saliva
$VI$. Tomato juice
The number of solutions with $pH$ less than $7$ is

An alcoholic drink has a $pH = 4.7$. What is the $OH^{-}$ ion concentration of this solution? (Given: $K_w = 10^{-14} \ mol^2/L^2$)