assume that you have a solution that is 5% (mol) acetone and 95% (mol) water. determine the molarity of this solution. how would you prepare a solution of this concentration in the lab? density of acetone=0.79 g/ml

To determine the molarity of the solution, we need to know the amount of solute (acetone) and the volume of the solution.

Given that the solution is 5% (mol) acetone and 95% (mol) water, we can assume a total volume of 100 mL, which means that 5 mL of the solution is acetone and 95 mL is water.

To determine the molarity, we need to convert the amount of solute (acetone) from mL to moles. We can use the density of acetone to help in this conversion.

First, let's calculate the mass of acetone:
Mass = density × volume
Mass = 0.79 g/mL × 5 mL
Mass = 3.95 g

Next, we need to convert the mass of acetone to moles using its molar mass. The molar mass of acetone (C3H6O) is 58.08 g/mol.

Moles = mass ÷ molar mass
Moles = 3.95 g ÷ 58.08 g/mol
Moles ≈ 0.068 moles

Now that we know the moles of acetone (0.068 mol) and the total volume of the solution (100 mL), we can calculate the molarity:

Molarity = moles ÷ volume
Molarity = 0.068 mol ÷ 0.1 L
Molarity = 0.68 M

Therefore, the molarity of the solution is approximately 0.68 M.

To prepare a solution of this concentration in the lab, you would measure 5 mL of acetone and add it to 95 mL of water. Make sure to mix them thoroughly to obtain a homogeneous solution.