Asked by Mandy
What volume of 5.0 M H2SO4 should be diluted to 100mL to prepare a 0.25 M H2SO4 M solution?
I know the molar mass of H2SO4 is 98g but I'm not sure where exactly that fits in and how I'm supposed to get it to be diluted.
Thank you!
I know the molar mass of H2SO4 is 98g but I'm not sure where exactly that fits in and how I'm supposed to get it to be diluted.
Thank you!
Answers
Answered by
herp_derp
The general formula for a dilution is
M₁V₁=M₂V₂
Look familiar? Notice how MV is the number of moles. The number of moles of H₂SO₄ solution do not change.
So, all we have to do now is plug in what we know, and solve for the unknown, which is V₁.
(5.0 M)V₁ = (0.25 M)(100 mL)
V₁ = 5.0 mL
Therefore, 5.0 mL of the 5.0 M solution of H₂SO₄ should be diluted to get 100 mL of a 0.25 M solution of H₂SO₄.
M₁V₁=M₂V₂
Look familiar? Notice how MV is the number of moles. The number of moles of H₂SO₄ solution do not change.
So, all we have to do now is plug in what we know, and solve for the unknown, which is V₁.
(5.0 M)V₁ = (0.25 M)(100 mL)
V₁ = 5.0 mL
Therefore, 5.0 mL of the 5.0 M solution of H₂SO₄ should be diluted to get 100 mL of a 0.25 M solution of H₂SO₄.
Answered by
bobpursley
another way.
You want to dilute it 5/.25 or 20 times.
That means 19 parts water, one part stock acid. so you need 1/20 *100ml of stock solution. or 5 ml.
You want to dilute it 5/.25 or 20 times.
That means 19 parts water, one part stock acid. so you need 1/20 *100ml of stock solution. or 5 ml.
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