The $pH$ value of $0.1 \ M \ NaOH$ solution is (given that the ionic product of water $K_w = [H^{+}] [OH^{-}] = 10^{-15}$)

$A$ base dissolved in water yields a solution with a hydroxyl ion concentration of $0.05 \ mol \ L^{-1}$. The solution is

Which of the following will have the highest $pH$?

$600 \, mL$ of $0.01 \, M \, HCl$ is mixed with $400 \, mL$ of $0.01 \, M \, H_2SO_4$. The $pH$ of the mixture is $....... \times 10^{-2}$. (Nearest integer) [Given $\log 2 = 0.30, \quad \log 3 = 0.48, \quad \log 5 = 0.69, \quad \log 7 = 0.84, \quad \log 11 = 1.04$]

The $pH$ of a $10^{-10} \ M$ $HCl$ solution is approximately

Given below are two statements:
Statement-$I$: $pH$ of a $1.0 \times 10^{-8} \ M$ solution of $HCl$ is $8$ at $25^{\circ} C$.
Statement-$II$: $HCl$ is a strong acid and negative log of $H^{+}$ concentration is called $pH$.
In the light of the above statements,choose the most appropriate answer from the options given below: