Question

A titration is performed where 0.150M sodium hydroxide solution is added to a solution of KHP.

If 25.00mL was required to reach the end point, how many moles of KHP must have been present?

Answer 1

0.00375 moles OF KHP

Step-by-step explanation:

Equation of reaction of NaOH and KHP :

KHC₈H₄ O₄(aq) + NaOH(aq) → NaKC₈H₄O₄(aq) + H₂O(l)

the reaction required 25ml

Molarity = no of mole / volume in liters

no of moles = Molarity × volume in liters

no of moles of NaOH = 0.150 × (25/1000) = 0.00375 moles

using the balanced equation above

1 mole of NaOH requires 1 mole of KHP

therefore

0.00375 mole of NaOH will require 0.00375 mole KHP.