Question

In a titration of hydrobromic acid (HBr) against sodium hydroxide (NaOH), 22.20 mL of 0.150 M NaOH is required to neutralize 36.60 mL of HBr. Calculate the molarity of the HBr. M1V1=M2V2

Answer 1

[HBr] = 0.0910 M

Step-by-step explanation:

NaOH → Strong base

HBr → Strong acid.

This is a titration that involves a strong acid and a strong base, so the recaction is about acid base equilibrium.

Formula for titration in the equivalence point is:

mmoles of acid = mmoles of base

M . Volume of acid = M . volume of base

We replace data:

M . 36.60 mL = 0.150 M . 22.20 mL

M = (0.150 M . 22.20 mL) / 36.60 mL

M = 0.0910 mol/L