A student weighs out 0.512g of KHP(molar mass = 204.22 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one proton.

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Jarrod RobelLv2

17 Jun 2019

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Potassium hydrogen phthalate (KHP, molar mass = 204.22 g/mol) is often used as a primary standard in acid-base titration. If 20.35 mL of NaOH is required to neutralize 0.397 g of KHP, what is the concentration of the NaOH?

A student titrate an unknown amount of potassium hydrogen phthalate (KHC8H4O4 often abbreviated KHP) with 20.46 mL of a 0.1000 M NaOH solution. KHP(molar mass= 204.22 g/mol) has one acdic hydrogen. How many grams of KHP were titrated (reacted completely) by the sodium hydroxide solution?Please answer step by step if possible.

I need the answer of #2 < #1 is answered because we need it in#2 >

1.A 0.2816g sample of KHP required 29.68 mL of sodium hydroxide toreach the phenolphthalein end point. Calculate the molarity of NaOHsolution.
#1 answer Given that mass of KHP = 0.2816 g
We know that
The molar mass of KHP = 204.22 g/mol
? Number of moles of KHP = mass / molarmass
= 0.2816 g/204.22 g/mol
= 0.00138 mol
We know that one mole of NaOH neutralizes one mole ofKHP
? The number of moles of NaOH = NUmber of molesof KHP
= 0.00138 mol
The volume of NaOH = 29.68 mL
= 0.02968 L
Hence te molarity of NaOH = moles / volume inliters
= 0.00138 mol / 0.02968 L
= 0.04646M

2. A volume of 20.22 mL of the Naoh solution described in Q.1 wasneeded to titrate 10.06 mL of acetic acid of the phenolphthaleinend point. Find the concentration of the acetic acid solution.

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A student weighs out 0.512g of KHP(molar mass = 204.22 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one proton.

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