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.

Be sure to include:

1. The calculations determining the amount of stock needed to make the 3M solution.

2. The steps the teacher needs to take in order to prepare the solution.

25 mL

Explanation:

PART 1:

12.0 M * V = .1 L * 3 M

12 * V = .3

V = .025 L OR 25 mL

The moles of the acid in your final solution have to equal the moles that you add from your stock solution. Since molarity (M) = moles/volume, that means moles = M*V. Therefore, to find the volume, set M*V for the stock solution equal to M*V for your final solution.

PART 2:

To make this diluted solution, add the 25 mL of stock solution to a small amount of pure solvent. Then fill the graduated cylinder to the 100 mL mark with solvent.

answer: mole of the gas

answer: mole of the gasexplanation: