Question

Q8. The titration of 15.00 mL of HBr solution of unknown concentration requires 18.44 mL of a 0.100 M KOH solution to reach the equivalence point. What is the concentration of the unknown HBr solution in M? Tro, Nivaldo J.. Chemistry (p. 201). Pearson Education. Kindle Edition.

Answer 1

Answer: 0.123 M

Explanation:

According to the neutralization law:

$n_1M_1V_1=n_2M_2V_2$

where,

$M_1$ = molarity of $HBr$ solution = ?

$V_1$ = volume of $HBr$ solution = 15.00 ml

$M_2$ = molarity of $KOH$ solution = 0.100 M

$V_2$ = volume of $KOH$ solution = 18.44 ml

$n_1$ = valency of $HBr$ = 1

$n_2$ = valency of $KOH$ = 1

$1\times M_1\times 15.00=1\times 0.100\times 18.44$

$M_1=0.123$

Therefore, the concentration of the unknown HBr solution is 0.123 M