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LiRa [457]
3 years ago
12

An aqueous solution of sodium hydroxide is standardized by titration with a 0.170 M solution of perchloric acid. If 28.5 mL of b

ase are required to neutralize 16.0 mL of the acid, what is the molarity of the sodium hydroxide solution?
Chemistry
1 answer:
Ray Of Light [21]3 years ago
4 0

Answer:

0.095M

Explanation:

HClO4 + NaOH = NaClO4 + H2O

Concentration of acid CA= 0.170M

Concentration of base CB= ???

Volume of base VB= 28.5ml

Volume of acid VA= 16.0ml

Number of moles of acid nA= 1

Number of moles of base nB= 1

From

CAVA/CBVB= nA/nB

CB= CAVAnB/VBnA

CB= 0.170×16.0×1/28.5×1

CB= 0.095M

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<u>Explanation:</u>

Every balanced chemical equation follows law of conservation of mass.

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