Question

It has 0.7428 g of an unknown acid, H2A, which reacts with NaOH according to the balanced reaction: H2A (AC) + 2 NaOH (AC)  Na2A (AC) + 2 H2O (l) if 36.04 ML of NaOH 0.5090 M is required to hold the acid up to its equivalence point , what is the molar mass of the acid? Identifies acid

Answer 1

H2A (AC) + 2 NaOH (AC) -> Na2A (AC) + 2 H2O (l)

1 mol H2A (AC) = 2 mol NaOH (AC)

No of mol of NaOH consumed = M*V

                           = 36.04*0.5090

                           = 18.34 mmol

No of mol of H2A reacted = 18.34*(1/2) = 9.17 mmol

molarmass of H2A reacted = w/n

                          = 0.7428/(9.17*10^-3)

                          = 81 g/mol