Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100. g solution.

Molar Mass (g/mol)
(CH3)2CO 58.05
H2O 18.015

Density (g/mL):
(CH3)2CO 0.7899
H2O 0.9982

Name/Formula:
acetone
(CH3)2CO
water
H2O

Answered below but I forgot to add that you need to use the densities to convert grams to volume.

To calculate the volume of solute (acetone) and solvent (water) needed to prepare a solution, you need to follow these steps:

Step 1: Convert the given mass of the solution to grams.
Given mass of the solution = 1.36 kg = 1.36 * 1000 g = 1360 g

Step 2: Calculate the mass of the solute (acetone) and solvent (water) in the solution.
Mass of solute (acetone) = 25.7 g per 100 g of solution
Mass of solute (acetone) = 25.7 g * (1360 g) / (100 g) = 349.52 g

Mass of solvent (water) = Mass of solution - Mass of solute
Mass of solvent (water) = 1360 g - 349.52 g = 1010.48 g

Step 3: Convert the mass of solute and solvent to volume using their respective densities.
Volume of solute (acetone) = Mass of solute (acetone) / Density of solute (acetone)
Volume of solute (acetone) = 349.52 g / 0.7899 g/mL = 442.48 mL

Volume of solvent (water) = Mass of solvent (water) / Density of solvent (water)
Volume of solvent (water) = 1010.48 g / 0.9982 g/mL = 1,012 mL

Step 4: Convert the volume of solute and solvent from milliliters (mL) to liters (L).
Volume of solute (acetone) = 442.48 mL / 1000 mL/L = 0.4425 L
Volume of solvent (water) = 1,012 mL / 1000 mL/L = 1.012 L

Therefore, you should add approximately 0.4425 L of acetone (solute) and 1.012 L of water (solvent) to prepare 1.36 kg of a solution that is 25.7 g of acetone per 100 g of solution.