Question

The density of 16.0% H2SO4 is 1.11 g/mL. Calculate its molarity.
_ = M

Answer 1

The molarity of the 16.0% H2SO4 solution with a density of 1.11 g/mL is calculated to be 1.811 M by first finding the mass of H2SO4 per liter, converting that mass to moles, and then dividing by the volume in liters.

Step-by-step explanation:

To calculate the molarity of a 16.0% H2SO4 solution with a density of 1.11 g/mL, you first need to find out how many grams of H2SO4 are present in one liter of solution. Since the solution is 16.0% sulfuric acid by mass:

• Mass of H2SO4 per L of solution = volume × density × mass % = 1000 mL × 1.11 g/mL × 0.16 = 177.6 g

Next, convert the mass of H2SO4 to moles using its molar mass (98.079 g/mol for H2SO4):

• Moles of H2SO4 = mass / molar mass = 177.6 g / 98.079 g/mol = 1.811 mol

The molarity (M) is the number of moles per liter of solution:

• Molarity = moles of solute / liters of solution = 1.811 mol / 1 L = 1.811 M