$0.837 \ g$ of $Ba(OH)_2$ is dissolved in $100 \ mL$ of solution. Calculate the $pH$ of the solution. (Atomic masses: $Ba = 137, O = 16, H = 1$)

Millimoles of calcium hydroxide required to produce $100 \ mL$ of the aqueous solution of $pH$ $12$ is $x \times 10^{-1}$. The value of $x$ is $..............$. (Nearest integer). Assume complete dissociation.

Calculate the $pOH$ of a $0.01 \text{ M}$ monobasic acid solution that is completely dissociated at $298 \text{ K}$.

Concentration of $H^{+}$ ions in $10^{-4} \ M \ HCl$ solution is

Which of the following,when added to $10 \ mL$ of dilute $HCl$,will not change the $pH$ of the solution?

$50 \ mL$ of $H_2O$ is added to $50 \ mL$ of $1 \times 10^{-3} \ M$ barium hydroxide solution. What is the $pH$ of the resulting solution?