Question

A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....?
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP,
with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and a final
buret reading of 31.32 mL.
“KHP” is shorthand for a certain acid. It contains NO phosphorus.

•Write the reaction equation for the acid-base neutralization.
I got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct?

•Name the secondary standard used in the titration of the unknown KHP mixture.


• Calculate the amount of NaOH (in millimoles) delivered in the titration.


• Find the mass of KHP neutralized in the reaction.


• Calculate the mass percent of KHP in the original sample.

Answer 1

got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct?
<b>yes</b>

•Name the secondary standard used in the titration of the unknown KHP mixture.
<b>NaOH</b>

• Calculate the amount of NaOH (in millimoles) delivered in the titration.
<b>
mL x M = millimols</b>

• Find the mass of KHP neutralized in the reaction.

<b>millimoles KHP = millimoles NaOH
g KHP = (millimoles/1000)*molar mass</b>

• Calculate the mass percent of KHP in the original sample.

<b>%KHP in sample = (grams KHP/mass sample)*100 = ?</b>