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What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1 x Ka2 = 10-20 .
Correct answer is '1'. Can you explain this answer?
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To determine the minimum pH required to prevent the precipitation of ZnS, we need to consider the solubility product constant (Ksp) of ZnS and the effect of pH on the concentration of H2S.
The balanced chemical equation for the precipitation reaction is:
Zn2+ + S2- -> ZnS
The solubility product constant (Ksp) expression for ZnS is:
Ksp = [Zn2+][S2-]
Given that Ksp = 10, we can assume that the concentration of Zn2+ is equal to the concentration of S2- in the saturated solution.
Let's assume x is the concentration of Zn2+ (or S2-) in the saturated solution.
So, [Zn2+] = [S2-] = x
The concentration of Zn2+ in the solution is given as 0.01 M (0.01 mol/L).
Therefore, we have:
0.01 = x
The concentration of H2S is given as 0.10 M (0.10 mol/L).
H2S is a weak acid and can dissociate in water as follows:
H2S ⇌ H+ + HS-
HS- ⇌ H+ + S2-
The equilibrium constant expression for the dissociation of H2S is:
Ka = [H+][HS-]/[H2S]
Given that the concentration of H2S is 0.10 M and the concentration of HS- is x (since [HS-] = [Zn2+] = [S2-]), we can write:
Ka = [H+][x]/[0.10]
The pH is defined as the negative logarithm of the hydrogen ion concentration (pH = -log[H+]).
To prevent the precipitation of ZnS, the concentration of H+ should be sufficient to keep the concentration of S2- (or [Zn2+]) below the solubility product constant (Ksp = 10).
Therefore, we have:
[H+][S2-] < />
[H+][x] < />
Substituting the values, we get:
[H+][0.01] < />
[H+] < />
[H+] < />
Taking the negative logarithm of both sides to find the pH, we have:
-pH < />
pH > -log(1000)
pH > 3
Therefore, the minimum pH required to prevent the precipitation of ZnS is pH > 3.
The balanced chemical equation for the precipitation reaction is:
Zn2+ + S2- -> ZnS
The solubility product constant (Ksp) expression for ZnS is:
Ksp = [Zn2+][S2-]
Given that Ksp = 10, we can assume that the concentration of Zn2+ is equal to the concentration of S2- in the saturated solution.
Let's assume x is the concentration of Zn2+ (or S2-) in the saturated solution.
So, [Zn2+] = [S2-] = x
The concentration of Zn2+ in the solution is given as 0.01 M (0.01 mol/L).
Therefore, we have:
0.01 = x
The concentration of H2S is given as 0.10 M (0.10 mol/L).
H2S is a weak acid and can dissociate in water as follows:
H2S ⇌ H+ + HS-
HS- ⇌ H+ + S2-
The equilibrium constant expression for the dissociation of H2S is:
Ka = [H+][HS-]/[H2S]
Given that the concentration of H2S is 0.10 M and the concentration of HS- is x (since [HS-] = [Zn2+] = [S2-]), we can write:
Ka = [H+][x]/[0.10]
The pH is defined as the negative logarithm of the hydrogen ion concentration (pH = -log[H+]).
To prevent the precipitation of ZnS, the concentration of H+ should be sufficient to keep the concentration of S2- (or [Zn2+]) below the solubility product constant (Ksp = 10).
Therefore, we have:
[H+][S2-] < />
[H+][x] < />
Substituting the values, we get:
[H+][0.01] < />
[H+] < />
[H+] < />
Taking the negative logarithm of both sides to find the pH, we have:
-pH < />
pH > -log(1000)
pH > 3
Therefore, the minimum pH required to prevent the precipitation of ZnS is pH > 3.
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What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer?
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What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer?.
What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 0.10 M H2S ? Given Ksp of ZnS = 10–21, for H2S Ka1x Ka2= 10-20.Correct answer is '1'. Can you explain this answer?.
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