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

`Molarity_(KOH)=0.121\ M`

Step-by-step 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 = (Mass\ taken)/(Molar\ mass)`

Thus,

`Moles= (0.566\ g)/(204.22\ g/mol)`

`Moles\= 2.7715* 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* 10^(-3)\ mol` of KHP reacts with
`2.7715* 10^(-3)\ mol` of KOH

Moles of KOH =
`2.7715* 10^(-3)\ mol`

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

`Molarity=(Moles\ of\ solute)/(Volume\ of\ the\ solution)`

`Molarity_(KOH)=(2.7715* 10^(-3))/(0.0229)`

`Molarity_(KOH)=0.121\ M`