Question

A 0.826 g sample of a diprotic acid is dissolved in water and titrated with 0.110 M NaOH. What is the molar mass of the acid if 36.5 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol Não

Answer 1

Diprotic Acid vs NaOH M,via = M2 V₂ & 2 wereren M = Molarity, V= Volume , X=n-factor 1, x = M₂ V2 R2 : n= mxv] molo - 2ши ман 0.826x2 = 0.110 x 36.5x1 Molarmas n = mole м 0.826 x 2 x 1000 M M= 411.459/mol 0.110 x 36.5 → [M= 41.15g/mol , CScanned with CamScanner