Answer to Question #332614 in General Chemistry for Ivan Ackerman

Question

A 0.415 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. 

Calculate the volume of NaOH that should neutralize the KHP sample.

Answer 1

Solution:

The molar mass of KHP is 204.22 g mol^−1

Balanced chemical equation:

KHP(aq) + NaOH(aq) → KNaP(aq) + H₂O(l)

According to stoichiometry:

Moles of KHP = Moles of NaOH

or:

Mass of KHP / Molar mass of KHP = Molarity of NaOH × Volume of NaOH

Therefore,

Volume of NaOH = (Mass of KHP) / (Molarity of NaOH × Molar mass of KHP)

Volume of NaOH = (0.415 g) / (0.100 M × 204.22 g mol^−1) = 0.0203 L = 20.3 mL

Volume of NaOH = 20.3 mL

Answer: 20.3 milliliters of NaOH solution