Your teacher needs a 3.0M solution acid, but only has a 12.0M stock solution of sulfuric acid in the chemical store room. Calculate and describe the steps the teacher needs to take in order to make 100mL of the 3.0M solution of sulfuric acid.

The calculations are in the explanation below.

The steps are:

Explanation:

To make 100 mililiter of the 3.0M solution of sulfuric acid, first you must calculate the volume of the 12.0M stock solution that contains the same number of moles as the diluted solution.

For that, you use the dilution formula:

Then, the steps are:

1. Using a graduated pipette, accurately take 25mL of the 12.0M stock solution.

2. Pour the 25mL of stock solution into a 100 mL volumetric flask

3. Add distilled water up to the mark

4. Cap the flask with the stopper

5. Stirr by gently rotating the flask.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.