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Effectus [21]
3 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:
Igoryamba3 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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Answer:

0.1105 moles per 130 ml

Explanation:

For  1 L (1000) of solution, no of moles are =  0.85

For 1 ml of solution, no of moles are = 0.85/1000 moles

For 130 ml of solution, no of moles are=  0.85/1000 x 130

                                                                = 0.1105 moles per 130 ml

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What happens to a reaction at equilibrium when a reactant is removed from the reaction system
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The speed of a wave in the string is 16.2ms. The mass per unit length of the string is 0.3ms calculate tension in the string
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Answer:

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Explanation:

The tension in the string can be determined from the expression;

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