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The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6?
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The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What wo...
Solution:
Calculating the concentration of SO42- ions:
BaSO4 ⇌ Ba2+ + SO42-
Let the concentration of SO42- ions be x M.
Since the reaction equation is 1:1, the concentration of Ba2+ ions will also be x M.
Using the solubility product expression:
Ksp = [Ba2+][SO42-] = 10^-9
Substituting the values, we get:
10^-9 = x * x
x = [SO42-] = [Ba2+] = 10^-4 M
Thus, the concentration of SO42- ions in the solution is 10^-4 M.
Calculating the concentration of H2SO4 required:
H2SO4 + Ba2+ → BaSO4 + 2H+
The balanced chemical equation shows that for every one Ba2+ ion, two H+ ions are required. Therefore, the concentration of H2SO4 required will be twice the concentration of Ba2+ ions.
Concentration of Ba2+ ions = 0.01 M
Concentration of H2SO4 required = 2 * 0.01 M = 0.02 M
Therefore, the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba2+ ions is 0.02 M.
Answer: D) 10^-6
Calculating the concentration of SO42- ions:
BaSO4 ⇌ Ba2+ + SO42-
Let the concentration of SO42- ions be x M.
Since the reaction equation is 1:1, the concentration of Ba2+ ions will also be x M.
Using the solubility product expression:
Ksp = [Ba2+][SO42-] = 10^-9
Substituting the values, we get:
10^-9 = x * x
x = [SO42-] = [Ba2+] = 10^-4 M
Thus, the concentration of SO42- ions in the solution is 10^-4 M.
Calculating the concentration of H2SO4 required:
H2SO4 + Ba2+ → BaSO4 + 2H+
The balanced chemical equation shows that for every one Ba2+ ion, two H+ ions are required. Therefore, the concentration of H2SO4 required will be twice the concentration of Ba2+ ions.
Concentration of Ba2+ ions = 0.01 M
Concentration of H2SO4 required = 2 * 0.01 M = 0.02 M
Therefore, the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba2+ ions is 0.02 M.
Answer: D) 10^-6
Community Answer
The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What wo...
Ksp=[Ba2+][SO42-].10^-9=[0.01][SO42-].[SO42-]=10^-7. therefore 10^-7 is the concentration of H2SO4 required to precipitate BaSO4 solution.
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The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6?
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The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6? 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 Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6? 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 Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6?.
The solubility product of BaSO4 at 25 degree Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6? 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 Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6? 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 Celsius is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01M Ba2 ions A) 10^-9 B) 10^-8 C) 10^-7 D) 10^-6?.
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