Calculate the molarity, molality, and density of a solution prepared by mixing equal volumes of 30% by mass of H2SO4 whose density is 1.218g/mL & by 70% mass of H2SO4 of density 1.61 g/mL so that the resulting solution is 52.83% by mass.
This doubt is from the first chapter of chemistry i e Some basic concepts of Chemistry and is from the topic concentration of solution which involves:-
1)Mass %
2)Mass/Volume%
3)Molarity
4)Molality
5)Strength
6)Mole fraction
Please answer quickly....it is really urgent..and please stick to the 11th syllabus and explain how you have done it....
This doubt is from the first chapter of chemistry i e Some basic concepts of Chemistry and is from the topic concentration of solution which involves:-
1)Mass %
2)Mass/Volume%
3)Molarity
4)Molality
5)Strength
6)Mole fraction
Please answer quickly....it is really urgent..and please stick to the 11th syllabus and explain how you have done it....
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1st H2SO4 solution has density = 1.218g/ml
thats is 1ml has 1.218g substance. So, 1litre will have 1218g substance. Now, H2SO4 in this 1 litre will be 30% by mass ie 0.3 x 1218 = 365.4g ie 365.4/98 moles H2SO4 = 3.73moles.
2nd H2SO4 solution has density = 1.61g/ml
thats is 1ml has 1.61g substance. So, 1litre will have 1610g substance. Now, H2SO4 in this 1 litre will be 70% by mass ie 0.7 x 1610 = 1127g ie 1127/98 moles H2SO4 = 11.5moles.
On mixing the solutions the total moles of H2SO4 become = 11.5 + 3.73 = 15.23 moles in 2 litres
So, Molarity = 15.23/2 = 7.615M
Now this molarity has 7.615 moles of H2SO4 in 2 litres ie 100% H2SO4. If this solution had to be 52.83% by mass then we must divide the total mass by 0.5283 ie (365.4 +1127) / 0.5283 = 2825g in 2000 ml. So in 1ml amount of substance will be 2825/2000 = 1.412 g/ml ie density of solution.
thats is 1ml has 1.218g substance. So, 1litre will have 1218g substance. Now, H2SO4 in this 1 litre will be 30% by mass ie 0.3 x 1218 = 365.4g ie 365.4/98 moles H2SO4 = 3.73moles.
2nd H2SO4 solution has density = 1.61g/ml
thats is 1ml has 1.61g substance. So, 1litre will have 1610g substance. Now, H2SO4 in this 1 litre will be 70% by mass ie 0.7 x 1610 = 1127g ie 1127/98 moles H2SO4 = 11.5moles.
On mixing the solutions the total moles of H2SO4 become = 11.5 + 3.73 = 15.23 moles in 2 litres
So, Molarity = 15.23/2 = 7.615M
Now this molarity has 7.615 moles of H2SO4 in 2 litres ie 100% H2SO4. If this solution had to be 52.83% by mass then we must divide the total mass by 0.5283 ie (365.4 +1127) / 0.5283 = 2825g in 2000 ml. So in 1ml amount of substance will be 2825/2000 = 1.412 g/ml ie density of solution.