Question

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 sulfuric 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.

Answer 1

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.

Step-by-step 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 =
`(final molarity x final volume)/(initial molarity)`

putting the given values in the equation:

initial volume =
`(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.