Question

How much volume of decamolar solution of H.So, is required to prepare

500ml of solution with density 1.03g/ml and having mass percentage equal to
40% ? Also calculate the molarity of the resulting solution.

Answer 1

To prepare 500 ml of a 40% mass/volume sulfuric acid solution with a density of 1.03 g/ml, you would need 210 ml of a decamolar (10 M) H₂SO₄ solution. The molarity of the prepared solution is 4.2 M.

Step-by-step explanation:

To calculate the volume of a decamolar (10 M) sulfuric acid solution, H₂SO₄, that is required to prepare 500 ml of a 40% mass/volume solution with a density of 1.03 g/ml, we need to use the definition of mass percentage and molarity.

First, calculate the mass of H₂SO₄ in the final solution using the mass percentage and the density:

Mass of H₂SO₄ = Volume × Density × Mass percentage
= 500 ml × 1.03 g/ml × 40%
= 206 g

Next, calculate the volume of the initial decamolar solution needed:

Volume of decamolar solution = Mass of solute / (Molarity × Molar mass of solute)
= 206 g / (10 mol/L × 98.079 g/mol)
= 0.210 L or 210 ml

Now, we can calculate the molarity of the resulting solution:

Molarity = Moles of solute / Volume of the solution
= (206 g / 98.079 g/mol) / 0.5 L
= 4.2 M

Therefore, 210 ml of a decamolar solution of H₂SO₄ is required, and the molarity of the prepared solution is 4.2 M.