Calculate the mass of KHP (molar mass 204.44 g/mol) that reacts with 15.0 mL of the 0.15 M NaOH solution (molar mass 40.00 g/mol) required for standardization of the NaOH solution. Show your work.
This done the same way as you other acid/NaOH problem. The only difference is in this problem the acid is given a name and they want grams and not M.
KHP + NaOH ==> NaKP
mols NaOH = M x L = ?
mols KHP = mols NaOH
Then mols KHP = grams KHP/molar mass KHP. You know molar mass and mols, solve for grams.
To calculate the mass of KHP that reacts with the NaOH solution, we need to use the balanced chemical equation and stoichiometry.
The balanced chemical equation for the reaction between NaOH and KHP is:
NaOH + KHC8H4O4 → KNaC8H4O4 + H2O
The molar ratio between NaOH and KHP in the balanced equation is 1:1. This means that one mole of NaOH reacts with one mole of KHP.
First, let's find the number of moles of NaOH that reacted. We are given the volume of NaOH solution (15.0 mL) and its concentration (0.15 M). We can use the formula:
moles of NaOH = concentration × volume (in liters)
Since the volume is given in milliliters, we need to convert it to liters:
15 mL = 15/1000 L = 0.015 L
moles of NaOH = 0.15 M × 0.015 L = 0.00225 moles
Since the molar ratio between NaOH and KHP is 1:1, the number of moles of KHP that reacted is also 0.00225 moles.
To calculate the mass of KHP, we can use its molar mass.
mass of KHP = moles of KHP × molar mass of KHP
mass of KHP = 0.00225 moles × 204.44 g/mol = 0.46095 grams
Therefore, the mass of KHP that reacts with the NaOH solution is approximately 0.461 grams.