Question

Calculate the molarity ( m ) of 157.3 g of H₂SO₄ in 1.390 L of solution.

Answer 1

The molarity of 157.3 g of H₂SO₄ in 1.390 L of solution is calculated by first finding the molar mass of H₂SO₄, then converting mass to moles, and finally dividing by the volume in liters. The resulting molarity is 1.153 M.

Step-by-step explanation:

To calculate the molarity of 157.3 g of H₂SO₄ in 1.390 L of solution, we need to follow these steps:

• First, determine the molar mass of H₂SO₄, which is 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol.
• Then, convert the mass of H₂SO₄ into moles by dividing 157.3 g by the molar mass (98.09 g/mol).
• Finally, divide the number of moles by the volume of the solution in liters to find the molarity.

Now, let's perform the calculations:

1. Moles of H₂SO₄ = 157.3 g ÷ 98.09 g/mol
2. Moles of H₂SO₄ = 1.603 mol (2 decimal places)
3. Molarity (M) = Moles of solute ÷ Volume of solution in liters
4. Molarity (M) = 1.603 mol ÷ 1.390 L
5. Molarity (M) = 1.153 M (3 decimal places)

The molarity of the H₂SO₄ solution is 1.153 M.