Question

What volume of 95% H_{​​​​​​2}​_​​​​​SO_​​​4 having density 1.85g/ml and what mass of water must be taken 100 ml of 50% H_{​​​​​2}​SO₄ having density 1.10 g/ml

Answer 1

Solution:

Volume of the solution = 100 ml = 100 cm³

Density of the solution = 1.10 g/cm³

Therefore, Mass of 100 cm³ of solution = 100 x 1.10 g =110 g

The given solutions is 50%. Therefore, 100 g of solution contains 50 g of H₂SO₄

Then, mass of H₂SO₄ in 110 g of solution = 50/100 *110 = 55 gm

Mass of water in 110 g of solution = (110 - 55) g = 55 g

To obtain 100 cm³ of 50 % solution acid, we require the given information.

Mass of water = 55 g

Mass of H₂SO₄ (100% pure) = 55 g

Since, the given sulphuric acid is 95% pure, hence,

Mass of H₂SO₄ (95%) will be required = 100*55/95 = 57.895 gm = 57.9 gm

Density = 1.85 g / cm³

So volume required = Mass / density = 57.9 /1.85 = 31.3 cm³

Answer : 31.3 cm³