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Effectus [21]
2 years ago
13

In the titration of 82.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to reach the equivalence point

Chemistry
1 answer:
Igoryamba2 years ago
8 0

Answer:

218.7 mL

Explanation:

The reaction that takes place is:

  • HCOOH + LiOH → LiCOOH + H₂O

First we <u>calculate how many HCOOH moles reacted</u>, using the <em>given volume and concentration</em>:

  • 82.0 mL * 0.400 M = 32.8 mmol HCOOH

As <em>1 HCOOH mol reacts with 1 LiOH mol</em>, 32.8 mmoles of LiOH are needed to react with 32.8 mmoles of HCOOH.

Finally we <u>calculate how many mL of a 0.150 M solution would contain 32.8 mmoles</u>:

  • 32.8 mmol / 0.150 M = 218.7 mL
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