What mass of water must be used to make a 1.35 m solution that contains 8.20 mol NaOH? (Show your work

The molarity (M) of a solution is defined as the number of moles of solute (NaOH in this case) divided by the volume of the solution in liters. The formula is:

M = moles of solute / liters of solution

We can rearrange this formula to solve for the volume of the solution:

liters of solution = moles of solute / M

Substituting the given values:

liters of solution = 8.20 mol NaOH / 1.35 M = 6.07 liters

Since the density of water is approximately 1 g/mL, we can convert the volume of the solution to mass. There are 1000 mL in a liter, so:

mass of water = 6.07 liters * 1000 mL/liter * 1 g/mL = 6070 g

Therefore, you would need 6070 g (or 6.07 kg) of water to make a 1.35 M solution that contains 8.20 mol NaOH.