An acetic acid solution is 6.00 M and has a density of 1.04 g/mL.What is the mass/mass percent concentration of HC₂H₃O₂ (60.06 g/mol)?

Question

Quizplus · Accepted Answer

First, we need to find the mass of acetic acid in 1 L of the solution. Since the density is 1.04 g/mL, 1 L of the solution would have a mass of:

1 L x 1.04 g/mL = 1040 g

Since the molarity of the solution is 6.00 mol/L, we can use the following formula to find the number of moles of acetic acid in 1 L of solution:

moles = Molarity x Volume
moles = 6.00 mol/L x 1 L
moles = 6.00 mol

Now, we can use the molar mass of acetic acid to find its mass in 1 L of solution:

mass = moles x molar mass
mass = 6.00 mol x 60.06 g/mol
mass = 360.36 g

Finally, we can use the mass of acetic acid and the total mass of the solution to find the mass/mass percent concentration:

mass/mass % = (mass of solute / mass of solution) x 100%
mass/mass % = (360.36 g / 1040 g) x 100%
mass/mass % = 34.7%

Therefore, the answer is C.

An Acetic Acid Solution Is 6