In a titration, 0.01M KOH was used to neutralize 18 milliliters of 2 M HBr. What was the volume of the base used?

3.60 ml

Explanation:

First of all we must put down the equation of the reaction. This will serve as a guide to our solution;

KOH(aq) + HBr(aq) > KBr(aq) + H2O(l)

The following were given in the question;

Concentration of acid CA= 2M

Volume of acid VA= 18ml

Concentration of base CB= 0.01 M

Volume of base VB=

Number of moles of acid NA= 1

Number of moles of base NB= 1

From;

CAVA/CBVB = NA/NB

CAVANB= CBVBNA

Therefore;

VB= CAVANB/CBNA

Substituting values;

VB= 2 × 18 ×1 / 0.01×1

VB= 3.60 ml

Therefore; 3.60 ml of base was used.

the answer is d. 74.02