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An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS ?
Use Ksp (ZnS) = 1.25 × 10–22 and Overall dissociation constant of H2S , KNET = K1K2 = 1 × 10–21
Use Ksp (ZnS) = 1.25 × 10–22 and Overall dissociation constant of H2S , KNET = K1K2 = 1 × 10–21
Correct answer is '0.20'. Can you explain this answer?
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An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What...
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An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What...
To determine the minimum molar concentration of H+ required to prevent the precipitation of ZnS, we need to compare the Ksp value of ZnS with the ion product (IP) of Zn2+ and HS-.
The balanced equation for the precipitation reaction of ZnS is:
Zn2+ + HS- -> ZnS
The ion product (IP) can be calculated as follows:
IP = [Zn2+][HS-]
Since the solution is saturated with H2S, the concentration of HS- is equal to the concentration of H2S, which is 0.1 M.
Let's assume the concentration of H+ is x M.
Then, the concentration of Zn2+ can be calculated as follows:
[Zn2+] = 0.05 M - x
Substituting the values into the ion product equation:
IP = (0.05 - x)(0.1)
To prevent the precipitation of ZnS, the IP should be less than or equal to the Ksp of ZnS. Therefore, we can set up the following inequality:
(0.05 - x)(0.1) ≤ 1.25
Simplifying the inequality:
0.005 - 0.1x ≤ 1.25
-0.1x ≤ 1.25 - 0.005
-0.1x ≤ 1.245
Dividing both sides by -0.1 (remember to reverse the inequality sign):
x ≥ -1.245 / -0.1
x ≥ 12.45
Therefore, the minimum molar concentration of H+ required to prevent the precipitation of ZnS is 12.45 M.
The balanced equation for the precipitation reaction of ZnS is:
Zn2+ + HS- -> ZnS
The ion product (IP) can be calculated as follows:
IP = [Zn2+][HS-]
Since the solution is saturated with H2S, the concentration of HS- is equal to the concentration of H2S, which is 0.1 M.
Let's assume the concentration of H+ is x M.
Then, the concentration of Zn2+ can be calculated as follows:
[Zn2+] = 0.05 M - x
Substituting the values into the ion product equation:
IP = (0.05 - x)(0.1)
To prevent the precipitation of ZnS, the IP should be less than or equal to the Ksp of ZnS. Therefore, we can set up the following inequality:
(0.05 - x)(0.1) ≤ 1.25
Simplifying the inequality:
0.005 - 0.1x ≤ 1.25
-0.1x ≤ 1.25 - 0.005
-0.1x ≤ 1.245
Dividing both sides by -0.1 (remember to reverse the inequality sign):
x ≥ -1.245 / -0.1
x ≥ 12.45
Therefore, the minimum molar concentration of H+ required to prevent the precipitation of ZnS is 12.45 M.
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An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS ?Use Ksp (ZnS) = 1.25 × 10–22 and Overall dissociation constant of H2S , KNET = K1K2 = 1 × 10–21Correct answer is '0.20'. Can you explain this answer?
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