Question

Two solutions of H2SO4 are prepared with different composition.
Solution A: 500 mL of 1 M aq. H2SO4 having density 1.2 g/mL.
Solution B: 100 mL of 2 M aq. H2SO4 having density 1.4 g/mL.
Select the correct statement.
If both solutions A and B are mixed, then molarity of final solution is 2.33 M
If both solutions A and B are mixed, then (w/w)% of H2SO4 is 10.72% in final solution
If both solutions A and B are mixed, then (w/v)% of H2SO4 is 11.43% in final solution
If both solutions A and B are mixed, then normality of final solution is 1.8 N​

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100 ml of H2SO4 having 1M and density 1.5g/ml is mixed with 400ml of water. Calculate final molarity of H2SO4 solution, if final density is 1.25g/ml

2 years ago

Answers : (1)

Dear Aman

Let's approach this two ways.

First, considering this to be a simple dilution problem:

M1V1 = M2V2

1.0 M H2SO4 X 100 mL = M2 (500 mL)

M2 = 0.20 M

Now, the initial H2SO4 solution has a volume of 100 mL and a mass of 150 g (I'm not convinced that this solution would have that high of a density, but we'll go with it for now).

The added water has a mass of 400 g, assuming a density of water of 1.00 g/mL.

So, the final solution has a mass of 550 g, and with a density of 1.25 g/mL, a volume of 440 mL.

Since this solution contains 0.100 mol H2SO4, the molarity is

0.100 mol / 0.440 L = 0.23 M

As I indicated above, the density of 1 M H2SO4 is not 1.5 g/mL, but is actually closer to 1.06 g/mL according to the MSDS sheet for 2 N H2SO4. In order to have a density of 1.5 g/mL, you would need an H2SO4 solution closer to 9 M rather than 1 M. I think so