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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

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3 years ago

Arun
25768 Points
```							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. RegardsArun(askIITians forum expert)
```
3 years ago
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