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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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Group 1 metals and group 2 metals form positive ions by losing 1 and 2 electrons respectively. Non-metals in group 17 gain 1, group 16 gain 2 and group 15 gain 3. Elements which lose electrons form positive ions while elements that gain electrons form negative ions. 

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Write one paragraph!!!!!reasons why the minimum wage should be increased.
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Answer:

There are pros and cons, I will explain mostly pros. After all the pros outweigh the cons.

Explanation:

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Ca(s) + O₂(g) + S(s) → CaSO4(s)
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The mass of Calcium required to complete this reaction is 4.008 g.

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In the given reaction mass of product after completion of reaction is 13.614 g that means total mass of constituents before reaction should also be 13.614.

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mass of Ca + mass of O₂ + mass of S = mass of CaSO4

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Therefore, by law of conservation of mass 4.008 g of Ca is required for the completion of the reaction.

Learn more about mass conservation here:

brainly.com/question/2030891

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