To determine the concentration of a solution in mol/L (Molarity), we need to convert the given percentage by mass into molarity using the density of the solution.
Step 1: Calculate the mass of acetic acid in grams. If the solution is 7.50% by mass, it means that 7.50 g of acetic acid is present in 100 g of the solution.
Step 2: Convert the mass of acetic acid to moles. The molar mass of acetic acid (CH3COOH) is 60.052 g/mol. Moles of acetic acid = mass of acetic acid / molar mass Moles of acetic acid = 7.50 g / 60.052 g/mol
Step 3: Convert the volume of the solution to liters. Since the density is given as 1.02 g/mL, it means that 1 mL of the solution has a mass of 1.02 g. To convert grams to milliliters, we divide by the density: 100 g / 1.02 g/mL = 98.039 mL. Finally, convert milliliters to liters: 98.039 mL / 1000 mL/L = 0.098039 L.
Step 4: Calculate the concentration (Molarity). Molarity = Moles of acetic acid / Volume of solution in liters Molarity = (7.50 g / 60.052 g/mol) / 0.098039 L
Now we can calculate the concentration (Molarity): Molarity ≈ 0.204 mol/L
Therefore, the concentration of the 7.50% by mass acetic acid solution, with a density of 1.02 g/mL, is approximately 0.204 mol/L.