The $pH$ of $10^{-4} \ M$ $KOH$ solution will be

$600 \, mL$ 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 $\log 2 = 0.30, \quad \log 3 = 0.48, \quad \log 5 = 0.69, \quad \log 7 = 0.84, \quad \log 11 = 1.04$]

$100 \ mL$ of $0.1 \ M$ $HCl$ is taken in a beaker and to it $100 \ mL$ of $0.1 \ M$ $NaOH$ is added in steps of $2 \ mL$ and the $pH$ is continuously measured. Which of the following graphs correctly depicts the change in $pH$?

What is the $pH$ of a solution containing $5 \times 10^{-4} \text{ M } H^+$ ions?

Which of the following solutions will have $pH$ close to $1.0$?

What will be the $pH$ of a $10^{-8} \ M \ HCl$ solution?