After doing multiple titrations, your NaOH solution is determined to have a mean concentration value of 0.100 M. Given you are to assume your unknown acid is 75.0% KHP, how many grams of your unknown will you need to use 15.00 mL of your 0.100 M standardized NaOH

The mass of unknown acid needed is 0.230 grams

Explanation:

To calculate the number of moles for given molarity, we use the equation:

Molarity of NaOH solution = 0.100 M

Volume of solution = 15.00 mL = 0.015 L    (Conversion factor:  1 L = 1000 mL)

Putting values in above equation, we get:

The chemical reaction for the reaction of KHP and NaOH follows

By Stoichiometry of the reaction:

1 mole of NaOH reacts with 1 mole of KHP.

So, 0.0015 moles of NaOH will react with = of KHP

Moles of KHP = 0.0015 moles

Molar mass of KHP = 204.22 g/mol

Putting values in above equation, we get:

We are given:

Mass of unknown acid = 75 % of Mass of KHP

So, mass of unknown acid =

Hence, the mass of unknown acid needed is 0.230 grams

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