Answer to Question #129024 in General Chemistry for mike

Question

A 0.1216g sample of a monoprotic acid is dissolved in 25mL of water and the resulting solution is titrated with 0.1104M NaOH solution. A 12.5mL volume of the base is required to neutralise the acid. Calculate the molar mass of the acid.

Answer 1

Monoprotic Acid Is React With Strong Base Form Salt And Water .

1 mole of Acid React with 1 mol of Base

Moles Of Acid = 0.1216 / M ....................... 1 .

Where M is Molar Mass

Moles Of Base = 12.5 * 0.1104 / 1000 . ----------------2 .

eqn 1 = eqn 2 .

0.1216 / M = 12.5 * 0.1104 / 1000 .

M = 88.15 g / mol .