Question

The $pH$ of $0.001M$ $Ba(OH{)}_2$ solution will be:

• A. $2$
• B. $8.4$
• C. $11.3$
• D. $2.7$

Answer 1

The correct option is C $11.3$

Barium hydroxide is a strong base.

$Ba(OH{)}_2\rightleftharpoons B{a}^{2+}+2O{H}^{-}$

$\left[O{H}^{-}\right]=2\times 0.001M$

$pOH=-log\left[OH\right]=-log(2\times {10}^{-3})=2.7$

$pOH+pH=14=14-2.7=11.3$

$\therefore pHof0.001MBa(OH{)}_{2}is11.3$