Calculate the $pH$ of a $4 \times 10^{-3} \ M \ Y(OH)_2$ solution. Assume $100\%$ dissociation for the first step and $50\%$ dissociation for the second step.

$2.8 \text{ g}$ of $KOH$ is dissolved in a $500 \text{ mL}$ solution at $298 \text{ K}$. What is the $pH$ of the solution? (Molar mass of $KOH = 56 \text{ g/mol}$)

What will be the resultant $pH$ when $100 \ mL$ of an aqueous solution of $HCl$ $(pH = 2)$ is mixed with $200 \ mL$ of an aqueous solution of $NaOH$ $(pH = 12)$?

Aqueous solution of $HCl$ has the $pH = 4$. Its molarity would be (in $, M$)

Calculate the volume of $0.1 \ M \ NaOH$ required to complete the neutralization of $300 \ mL$ of $HCl$ solution having $pH = 2.25$. (in $mL$)

$100 \ mL$ 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 $pH$?