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50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10
- a)2.5 X10-9M
- b)2.5 X10-7M
- c)2.5 X10-8M
- d)2.5 X10-10M
Correct answer is option 'A'. Can you explain this answer?
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Solution:
Given, volume of solution = 50 ml
Moles of Ag in 50 ml solution = 10^-3 mol
Volume of HCl solution = 50 ml
Concentration of HCl solution = 0.1 M
AgCl(s) ⇌ Ag+ (aq) + Cl- (aq)
Initial concentration of Ag+ = 10^-3 mol/100 ml = 10^-5 M
Initial concentration of Cl- = 0.1 M/100 ml = 10^-3 M
The reaction between Ag+ and Cl- ions leads to the formation of AgCl(s), therefore, the concentration of Ag+ will decrease and Cl- will increase.
Let the concentration of Ag+ at equilibrium be x.
Ksp = [Ag+][Cl-] = 1.0 × 10^-10
10^-5 - x x
10^-3 + x x
10^-10 = x^2
x = 2.5 × 10^-6 M
Therefore, [Ag+] at equilibrium = 2.5 × 10^-6 M
The amount of Ag+ remaining in solution can be calculated as follows:
Amount of Ag+ remaining = Initial amount of Ag+ - Amount of Ag+ consumed
Initial amount of Ag+ = 10^-5 M × 50 ml = 5 × 10^-4 mol
Amount of Ag+ consumed = 2.5 × 10^-6 M × 50 ml = 1.25 × 10^-7 mol
Amount of Ag+ remaining = (5 × 10^-4 - 1.25 × 10^-7) mol = 4.99875 × 10^-4 mol
Concentration of Ag+ remaining = 4.99875 × 10^-4 mol/50 ml = 9.9975 × 10^-6 M
Therefore, [Ag+] remaining in solution = 9.9975 × 10^-6 M
Hence, the correct answer is option 'A' i.e 2.5 × 10^-9 M.
Given, volume of solution = 50 ml
Moles of Ag in 50 ml solution = 10^-3 mol
Volume of HCl solution = 50 ml
Concentration of HCl solution = 0.1 M
AgCl(s) ⇌ Ag+ (aq) + Cl- (aq)
Initial concentration of Ag+ = 10^-3 mol/100 ml = 10^-5 M
Initial concentration of Cl- = 0.1 M/100 ml = 10^-3 M
The reaction between Ag+ and Cl- ions leads to the formation of AgCl(s), therefore, the concentration of Ag+ will decrease and Cl- will increase.
Let the concentration of Ag+ at equilibrium be x.
Ksp = [Ag+][Cl-] = 1.0 × 10^-10
10^-5 - x x
10^-3 + x x
10^-10 = x^2
x = 2.5 × 10^-6 M
Therefore, [Ag+] at equilibrium = 2.5 × 10^-6 M
The amount of Ag+ remaining in solution can be calculated as follows:
Amount of Ag+ remaining = Initial amount of Ag+ - Amount of Ag+ consumed
Initial amount of Ag+ = 10^-5 M × 50 ml = 5 × 10^-4 mol
Amount of Ag+ consumed = 2.5 × 10^-6 M × 50 ml = 1.25 × 10^-7 mol
Amount of Ag+ remaining = (5 × 10^-4 - 1.25 × 10^-7) mol = 4.99875 × 10^-4 mol
Concentration of Ag+ remaining = 4.99875 × 10^-4 mol/50 ml = 9.9975 × 10^-6 M
Therefore, [Ag+] remaining in solution = 9.9975 × 10^-6 M
Hence, the correct answer is option 'A' i.e 2.5 × 10^-9 M.
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50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer? for JEE 2026 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer?.
50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer? for JEE 2026 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 ml of a solution containing 10-3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. Howmuch [Ag+] remains in solution? Given: Ksp of AgCl = 10-10a)2.5 X10-9Mb)2.5 X10-7Mc)2.5 X10-8Md)2.5 X10-10MCorrect answer is option 'A'. Can you explain this answer?.
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