Asked by Brittany
A Student Performing a lab weighed a 1.0993g sample, containing an unknown KHP, which required 18.06mL of 0.1879M NAOH to reach the phenolphtalein endpoint.
a) How many moles of base were consumed by the KHP in this sample?
b) How many grams of KHP were titrated?
c)What is the mass percent of KHP in the sample?
a) How many moles of base were consumed by the KHP in this sample?
b) How many grams of KHP were titrated?
c)What is the mass percent of KHP in the sample?
Answers
Answered by
DrBob222
mols NaOH = M x L = ?
mols KHP = same (1:1 ratio) from
KHP + NaOH ==> KNaP + H2O.
Calculate mass KHP from g = mols x molar mass.
Then %KHP = (mass KHP/mass sample)*100 = ?
mols KHP = same (1:1 ratio) from
KHP + NaOH ==> KNaP + H2O.
Calculate mass KHP from g = mols x molar mass.
Then %KHP = (mass KHP/mass sample)*100 = ?
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