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The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.
- a)Na2SO4 will precipitate
- b)CaSO4 will precipitate
- c)both will precipitate
- d)none will precipitat
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCa...
Ksp of CaSO4 = 2.4 x 10-5, 100 mL of 0.01M CaCl2 is mixed with 100 mL of 0.02 M Na2SO4. Concentration of Ca2+ and So42- will become Half because volume becomes double.
Kip = [Ca2+] [SO42-]
= 0.005 x 0.01 = 5 x 10-5
Kip = [Ca2+] [SO42-]
= 0.005 x 0.01 = 5 x 10-5
Kip > Ksp
Then, CaSO4 will precipitate.
Then, CaSO4 will precipitate.
Most Upvoted Answer
The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCa...
Calculation of ion concentrations:
CaCl2 dissociates into Ca2+ and 2Cl- ions.
Therefore, [Ca2+] = 0.01 M, [Cl-] = 0.02 M
Na2SO4 dissociates into 2Na+ and SO42- ions.
Therefore, [Na+] = 0.04 M, [SO42-] = 0.02 M
Calculation of ion product (Qsp):
Qsp = [Ca2+][SO42-]
= (0.01)(0.02)
= 2 x 10^-4
Comparison of Qsp with Ksp:
Ksp = 2.4 x 10^-5
Since Qsp > Ksp, the solution is supersaturated and precipitation will occur.
Explanation of the answer:
When CaCl2 and Na2SO4 are mixed, the concentrations of Ca2+ and SO42- ions increase in the solution. The ion product Qsp, which is the product of the ion concentrations, is greater than the solubility product constant Ksp of CaSO4. This means that the solution is supersaturated with respect to CaSO4 and precipitation will occur. Both CaSO4 and Na2SO4 will precipitate from the solution. Therefore, the correct answer is option C.
CaCl2 dissociates into Ca2+ and 2Cl- ions.
Therefore, [Ca2+] = 0.01 M, [Cl-] = 0.02 M
Na2SO4 dissociates into 2Na+ and SO42- ions.
Therefore, [Na+] = 0.04 M, [SO42-] = 0.02 M
Calculation of ion product (Qsp):
Qsp = [Ca2+][SO42-]
= (0.01)(0.02)
= 2 x 10^-4
Comparison of Qsp with Ksp:
Ksp = 2.4 x 10^-5
Since Qsp > Ksp, the solution is supersaturated and precipitation will occur.
Explanation of the answer:
When CaCl2 and Na2SO4 are mixed, the concentrations of Ca2+ and SO42- ions increase in the solution. The ion product Qsp, which is the product of the ion concentrations, is greater than the solubility product constant Ksp of CaSO4. This means that the solution is supersaturated with respect to CaSO4 and precipitation will occur. Both CaSO4 and Na2SO4 will precipitate from the solution. Therefore, the correct answer is option C.
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The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer?
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The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? 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 CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer?.
The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? 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 CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer?.
Solutions for The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for NEET.
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The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer?, a detailed solution for The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? has been provided alongside types of The solubility product of CaSO4 is 2.4 x 10-5. When 100 mL of 0.01 MCaCl2 and 100 mL of 0.02 M Na2SO4 are mixed, then.a)Na2SO4will precipitateb)CaSO4 will precipitatec)both will precipitated)none will precipitatCorrect answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
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