Answer to Question #319940 in General Chemistry for jjoel

Question

A 9.168 M aqueous solution of H₂SO₄ has a density of 1.4987 g/ml at 20^∘

 C. How many grams of H₂SO₄ are in 50.0 g of this solution? 

Answer 1

Solution:

Molarity = Moles of solute / Liters of solution

Calculate the liters of solution:

Density = Mass / Volume

Therefore,

Volume = Mass / Density = (50.0 g) / (1.4987 g/ml) = 33.36 mL

Liters of solution = (33.36 mL) × (1L / 1000 mL) = 0.03336 L

Calculate the moles of solute (H₂SO₄):

Moles of H₂SO₄ = Molarity × Liters of solution = (9.168 M) × (0.03336 L) = 0.3058 mol

Calculate the mass of solute (H₂SO₄):

The molar mass of H₂SO₄ is 98.079 g/mol

Therefore,

Mass of H₂SO₄ = (0.3058 mol H₂SO₄) × (98.079 g H₂SO₄ / 1 mol H₂SO₄) = 29.99 g H₂SO₄

Mass of H₂SO₄ = 30.0 g

Answer: 30.0 grams of H₂SO₄ are in this solution