How many grams of sulfuric acid, H2SO4, are required to make 2.0 L of a 3.0 M solution?Group of answer choices65.0 g46.0 g294 g588 g98.0 g

To solve this problem, we need to use the formula for molarity which is:

Molarity (M) = moles of solute / liters of solution

We know the molarity (3.0 M) and the volume of the solution (2.0 L), and we need to find the amount of sulfuric acid in grams.

First, we need to find the number of moles of sulfuric acid. We can rearrange the formula to find moles:

moles of solute = Molarity (M) * liters of solution moles of solute = 3.0 M * 2.0 L = 6.0 moles

Next, we need to convert moles to grams. The molar mass of sulfuric acid (H2SO4) is approximately 98.08 g/mol.

grams of solute = moles of solute * molar mass grams of solute = 6.0 moles * 98.08 g/mol = 588.48 g

So, we need approximately 588 g of sulfuric acid to make 2.0 L of a 3.0 M solution. The closest answer choice is 588 g.