Question

What is the molarity of a barium hydroxide solution if $15.48\text{mL}$ of it is required to neutralize $25\text{mL}$ of a $0.3096\text{M}HCl$ solution?

• A. $0.25\text{M}$
• B. $4.0\text{M}$
• C. $2.5\text{M}$
• D. $0.50\text{M}$

Answer 1

The correct option is A $0.25\text{M}$

Let the molarity of the $Ba(OH{)}_2$ solution be M
n-factor of $Ba(OH{)}_2=2$, and n-factor of $HCl=1$ $(n-\text{factor}\times \text{molarity}\times \text{volume}{)}_{Ba(OH{)}_2}=(n-\text{factor}\times \text{molarity}\times \text{volume}{)}_{HCl}$
$\Rightarrow 2\times M\times 15.48=1\times 0.3096\times 25$
$M=0.25\text{M}$