Question

A 0.1516g sample of a solid weak acid was dissolved in 25.00 mL of distilled water and titrated with 0.1120 M sodium hydroxide solution. Calculate the FORMULA WEIGHT of the weak acid.

Answer 1

Molarity (concentration) will changes upon dilution, but number of moles won't change.

There is no data about weak acid? Ka (dissociation constant), concentration, is this a complete neutralization (equivalence point)?

Assuming this is for complete neutralization values and also as a monoprotic acid.

moles NaOH reacted = moles weak acid completely neutralized = 0.112 moles

molar mass or formula weight = mass of acid / moles of acid

Formula weight = 0.1516 g / 0.112 mol = 1.35 g/mol

Formula weight = 1.35 g/mol

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