Question

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.

If 22.9 mL of a potassium hydroxide solution are needed to neutralize 0.566 grams of KHP, what is the molarity of the potassium hydroxide solution?
_____M

please show steps and how you started! thank you

Answer 1

Answer:

$Molarity_{KOH}=0.121\ M$

Explanation:

Moles of KHP :

Given, Mass of KHP = 0.566 g  

Molar mass of KHP = 204.22 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{0.566\ g}{204.22\ g/mol}$

$Moles\= 2.7715\times 10^{-3}\ mol$

According to the reaction shown below:

KHP + KOH ⇒ KKP + H₂O

1 mole of KHP reacts with 1 mole of KOH

So,

$2.7715\times 10^{-3}\ mol$ of KHP reacts with $2.7715\times 10^{-3}\ mol$ of KOH

Moles of KOH = $2.7715\times 10^{-3}\ mol$

Volume = 22.9 mL = 0.0229 L ( 1 mL = 0.001 L)

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity_{KOH}=\frac{2.7715\times 10^{-3}}{0.0229}$

$Molarity_{KOH}=0.121\ M$