Question

An aqueous solution of barium hydroxide is standardized by titration with a 0.110 M solution of hydrochloric acid. If 29.5 mL of base are required to neutralize 14.4 mL of the acid, what is the molarity of the barium hydroxide solution

Answer 1

Answer:

0.02685 M is the molarity of the barium hydroxide solution.

Explanation:

To calculate the concentration of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $HCl$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is $Ba(OH)_2$ mm.

We are given:

$n_1=11\\M_1=0.110 M\\V_1=14.4 mL\\n_2=2\\M_2=?\\V_2=29.5 mL$

Putting values in above equation, we get:

$1\times 0.11 M\times 14.4 mL=2\times M_2\times 29.5 mL$

$M_2=\frac{1\times 0.11 M\times 14.4 mL}{2\times 29.5 mL}=0.02685 M$

0.02685 M is the molarity of the barium hydroxide solution.