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natka813 [3]
3 years ago
14

In order to complete a lab, your teacher needs a 3.0 M solution of sulfuric acid, but only has a 12.0 M stock solution of sulfur

ic acid in the chemical store room. Calculate and describe the steps the teacher needs to take in order to make 100 mL of the 3.0 M solution of sulfuric acid.
Chemistry
1 answer:
Dimas [21]3 years ago
4 0

25 ml of the 12M solution will be diluted with water till volume made upto 100 ml to get a solution of 3M sulphuric acid.

Explanation:

Data given:

stock solution molarity (initial) = 12 M

Required molarity  (final)= 3M

Required volume (final)= 100ml

final volume = ?

So the formula used for dilution is:

Initial molarity X Initial volume = final molarity x final volume

initial volume = \frac{final molarity x final volume}{initial molarity}

putting the given values in the equation:

initial volume = \frac{3X100}{12}

                       = 25 ml

so, 25 ml of the original solution that is of 12 M will be diluted with water and volume made to 100ml will give a solution of 3M.

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The answer to your question is: C₄H₁₀O

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Data

          CxHyOz

mass sample : 1.376 g

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                      CxHyOz  + O₂ ⇒   CO₂  +  H₂O

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