Given: weight of aspirin = 0.6 g
We know that, molecular weight of aspirin = 180.160 g/mol
Therefore, number of mole of aspirin present = weight/molecular weight
= 0.6/180.16 = 3.33 X 10-3.
Aspirin is a monobasic acid. Therefore, 3.33 X 10-3 mole of NaOH is required to complete neutralization of aspirin.
Given: Concentration of NaOH = 0.1 M
∴, Volume of NaOH required for complete neutralization of aspirin,
= 3.33 X 10-3 / 0.1
= 3.33 X 10-2 L
= 33.3 mL
Answer: 33.3 mL of 0.1 M NaOH would be required to neutralize 0.6 g of aspirin
