Question

What volume of a 0.155 M potassium hydroxide solution is required to neutralize 25.7 mL of a 0.388 M hydrobromic acid solution

Answer 1

Answer: Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

$n_1M_1V_1=n_2M_2V_2$

where,

$M_1$ = molarity of $HBr$ solution = 0.338 M

$V_1$ = volume of $HBr$ solution = 25.7 ml

$M_2$ = molarity of $KOH$ solution = 0.155 M

$V_2$ = volume of $KOH$ solution = ?

$n_1$ = valency of $HBr$ = 1

$n_2$ = valency of $KOH$ = 1

$1\times 0.338\times 25.7=1\times 0.155\times V_2$

$V_2=56.0ml$

Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml