Question

What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4

Answer 1

The molarity of H2SO4 is the number of moles in 1 L of solution.
The molarity is 2.0 mol/L
This means that there should be 2 moles in a 1 L solution to make up this molarity.
In this case we need to make up a 5 L solutions with that molarity. Then the amount of moles required are - 2 mol/L x 5 L = 10 mol

Answer 2

The total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4 is 10 moles.

MOLARITY:

• The molarity of a solution can be calculated by dividing the number of moles in the substance by its volume. That is;

• Molarity = no. of moles ÷ volume

• This means that the number of moles in the solution can be calculated by multiplying the volume by its molarity.

Therefore, the number of moles in needed to prepare 5.0 liters of a 2.0 M solution of H2SO4 is as follows:

5 liters× 2M = 10 moles

Learn more about Molarity at: brainly.com/question/12127540