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It Ksp of Ag2CO3 is 8 × 10–12. The molar solubility of Ag2CO3 in 0.1 m AgNO3 is x × 10–10 find x:
Correct answer is '8'. Can you explain this answer?
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It Ksp of Ag2CO3 is 8 × 10–12. The molar solubility of Ag2...
× 10^-12, what is the solubility of Ag2CO3 in water?
The Ksp expression for Ag2CO3 is:
Ag2CO3 ⇌ 2Ag+ + CO32-
Ksp = [Ag+]^2[CO32-]
Let x be the solubility of Ag2CO3 in moles/L. Then, at equilibrium:
[Ag+] = 2x
[CO32-] = x
Substituting these values into the Ksp expression:
Ksp = (2x)^2(x) = 4x^3
Solving for x:
4x^3 = 8 × 10^-12
x^3 = 2 × 10^-12
x = (2 × 10^-12)^(1/3) = 1.24 × 10^-4 mol/L
Therefore, the solubility of Ag2CO3 in water is 1.24 × 10^-4 mol/L.
The Ksp expression for Ag2CO3 is:
Ag2CO3 ⇌ 2Ag+ + CO32-
Ksp = [Ag+]^2[CO32-]
Let x be the solubility of Ag2CO3 in moles/L. Then, at equilibrium:
[Ag+] = 2x
[CO32-] = x
Substituting these values into the Ksp expression:
Ksp = (2x)^2(x) = 4x^3
Solving for x:
4x^3 = 8 × 10^-12
x^3 = 2 × 10^-12
x = (2 × 10^-12)^(1/3) = 1.24 × 10^-4 mol/L
Therefore, the solubility of Ag2CO3 in water is 1.24 × 10^-4 mol/L.
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It Ksp of Ag2CO3 is 8 × 10–12. The molar solubility of Ag2CO3 in 0.1 m AgNO3 is x × 10–10 find x:Correct answer is '8'. Can you explain this answer?
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