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The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion?
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The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. ...
H2SO4 —> 2(H+) + (SO4)^-2
at t=0 s. 0 0
at complete dissociation
0 2s s
solubility product {ksp} = [ (Ba)^+2]×[ (SO4)^-2 ]
ksp = 10^(-9) { given }
[ (Ba)^+2 ] = 0.01 {given}
==>>>. 10^(-9) = 0.01 × s
=> s = 10^(-9) ÷ 0.01 = 10^(-7)
=> [ (SO4)^-2 ] = 10^(-7)
=> concentration of H2SO4 = 10^(-7)
at t=0 s. 0 0
at complete dissociation
0 2s s
solubility product {ksp} = [ (Ba)^+2]×[ (SO4)^-2 ]
ksp = 10^(-9) { given }
[ (Ba)^+2 ] = 0.01 {given}
==>>>. 10^(-9) = 0.01 × s
=> s = 10^(-9) ÷ 0.01 = 10^(-7)
=> [ (SO4)^-2 ] = 10^(-7)
=> concentration of H2SO4 = 10^(-7)
Community Answer
The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. ...
Introduction
To determine the concentration of H2SO4 required to precipitate BaSO4 from a 0.01 M Ba2+ solution, we need to understand the solubility product (Ksp) of BaSO4.
Ksp of BaSO4
- The solubility product constant (Ksp) of BaSO4 is given as 10^-9.
- The dissociation of BaSO4 in water can be represented as:
BaSO4 (s) ⇌ Ba2+ (aq) + SO4^2- (aq)
Relation of Ksp to Ion Concentrations
- The Ksp expression for BaSO4 is:
Ksp = [Ba2+][SO4^2-]
- For BaSO4 to start precipitating, the product of the ion concentrations must exceed Ksp.
Calculating SO4^2- Concentration
- Given that [Ba2+] = 0.01 M, we can set up the equation:
Ksp = [0.01][SO4^2-] = 10^-9
- Rearranging gives:
[SO4^2-] = Ksp / [Ba2+] = (10^-9) / (0.01) = 10^-7 M
Concentration of H2SO4 Required
- H2SO4 dissociates in solution to provide SO4^2- ions:
H2SO4 → 2H+ + SO4^2-
- Therefore, to achieve a [SO4^2-] concentration of 10^-7 M, we need the same concentration of H2SO4:
[H2SO4] = 10^-7 M
Conclusion
- To precipitate BaSO4 from a 0.01 M Ba2+ solution, the necessary concentration of H2SO4 is 10^-7 M.
To determine the concentration of H2SO4 required to precipitate BaSO4 from a 0.01 M Ba2+ solution, we need to understand the solubility product (Ksp) of BaSO4.
Ksp of BaSO4
- The solubility product constant (Ksp) of BaSO4 is given as 10^-9.
- The dissociation of BaSO4 in water can be represented as:
BaSO4 (s) ⇌ Ba2+ (aq) + SO4^2- (aq)
Relation of Ksp to Ion Concentrations
- The Ksp expression for BaSO4 is:
Ksp = [Ba2+][SO4^2-]
- For BaSO4 to start precipitating, the product of the ion concentrations must exceed Ksp.
Calculating SO4^2- Concentration
- Given that [Ba2+] = 0.01 M, we can set up the equation:
Ksp = [0.01][SO4^2-] = 10^-9
- Rearranging gives:
[SO4^2-] = Ksp / [Ba2+] = (10^-9) / (0.01) = 10^-7 M
Concentration of H2SO4 Required
- H2SO4 dissociates in solution to provide SO4^2- ions:
H2SO4 → 2H+ + SO4^2-
- Therefore, to achieve a [SO4^2-] concentration of 10^-7 M, we need the same concentration of H2SO4:
[H2SO4] = 10^-7 M
Conclusion
- To precipitate BaSO4 from a 0.01 M Ba2+ solution, the necessary concentration of H2SO4 is 10^-7 M.
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The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion?
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The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion?.
The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility product of BaSO4 at 25 degree centigrade is 10POWER-9. What should be the concentration ofH2SO4 necessary to precipitate BaSO4 solution of 0.01 M Ba 2 ion?.
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