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Problem on laboratory solution

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

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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

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