Question

What is the concentration of ammonia in a solution if 23.4 mL of a 0.117 M solution of HCl are needed to titrate a 100.0 mL sample of the solution?

Answer 1

Answer: 0.0274 M

Explanation:-

The balanced chemical solution is:

$NH_4OH(aq)+HCl(aq)\rightarrow NH_4Cl(aq)+H_2O(l)$

According to the neutralization law,

$n_1M_1V_1=n_2M_2V_2$

where,

$M_1$ = molarity of $HCl$ solution = 0.117 M

$V_1$ = volume of $HCl$ solution = 23.4 ml

$M_2$ = molarity of $NH_4OH$ solution = ?

$V_2$ = volume of $NH_4OH$ solution = 100.0 ml

$n_1$ = valency of $HCl$ = 1

$n_2$ = valency of $NH_4OH$ = 1

$1\times 0.117M\times 23.4=1\times M_2\times 100.0$

$M_2=0.0274$

Therefore, the concentration of ammonia in a solution will be 0.0274 M