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antiseptic1488 [7]
3 years ago
8

A 0.7834 g sample of a primary standard KHP was titrated with 38.45 mL of NaOH solution to a phenolphthalein end-point. What is

the molarity of the NaOH solution?
Chemistry
1 answer:
Zinaida [17]3 years ago
6 0

Answer:

0.0998 M

Explanation:

KHP is a weak <em>monoprotic</em> acid. This means that t<u>he moles of acid are equal to the moles of OH⁻ that were added in the titration</u>.

KHP Molecular weight = 204.22 g/mol

  • moles KHP = 0.7834 g ÷ 204.22 g/mol = 3.836x10⁻³ mol KHP

So  3.836x10⁻³ moles of OH⁻ were added in the titration. With moles and volume we can <u>calculate the molarity of the NaOH solution</u>:

38.45 mL ⇒ 38.45/1000 = 0.03845 L

  • 3.836x10⁻³ mol OH⁻ / 0.03845 L = 0.0998 M
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