Problem on laboratory solution

Question

You are asked to make up a laboratory solution of 0.10 molar H2SO4 from concentrated (96%) H₂SO₄ at 56°F. The barometric pressure reads 750 mmHg. You look up the specific gravity of 96% H₂SO₄ and find it is listed at 1.858. Calculate:

(a) the weight of 96% acid needed per L of solution.

(b) the volume of 96% acid used per L of solution

Answer 1

Now the sp gravity data shows 96% H₂SO₄ = 1.858

Now 96% H₂SO₄ is 96g of H₂SO₄ in 100 g Solution

Since Sp gravity is 1.858 So volume of 100g is=53.82131324 CC

So 96 g H₂SO₄ [Mw=98.116g/mole] =96/98.166 Mole=0.978433691 mole Present in  53.82131324 CC

So molarity of solution =0.018179298 M

So using S₁V₁=s₂V₂

0.018179298M*xml =0.1M*1000ml

So x=5500.762ML

0.1M 1000ml H₂So₄ contains =0.1mole H₂So₄ =9.8116 g H₂So₄

Now 96 g H₂So₄ contained in 100g  H₂SO₄( 96% H₂SO₄)

So 9.8116 g H₂So₄ in =(100/96)*9.8116 g 96% H₂So₄ =10.22041667 g 96% H₂SO₄