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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

Sagot :

Maacastrobridn

Answer:

218.7 mL

Explanation:

The reaction that takes place is:

  • HCOOH + LiOH → LiCOOH + H₂O

First we calculate how many HCOOH moles reacted, using the given volume and concentration:

  • 82.0 mL * 0.400 M = 32.8 mmol HCOOH

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

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

  • 32.8 mmol / 0.150 M = 218.7 mL
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