Question

Acetic acid (CH3CO2H) is the principal component in the vinegar. What is the molarity of an acetic acid solution if a titration of 50.00 mL of the acetic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

Answer 1

Answer : The molarity of an acetic acid solution is, 0.0338 M

Explanation :

Formula used :

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of acetic acid.

$M_2\text{ and }V_2$ are the molarity and volume of NaOH.

We are given:

$M_1=?\\V_1=50.0mL\\M_2=0.0567M\\V_2=29.80mL$

Putting values in above equation, we get:

$M_1\times 50.0mL=0.0567M\times 29.80mL\\\\M_1=0.0338M$

Hence, the molarity of an acetic acid solution is, 0.0338 M