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Given Ksp(AgCl) = 1.8x 10-10 and Ksp(Ag) = 8.3x10-17, provide a plausible reason why I would severely interfere with the Cl-

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Answer #1

The solubility of AgI in water is much less than that of AgCl in water.

The solubility product of AgCl = [Ag+][Cl-] = 1.8×10-10

Where [Ag+] = [Cl-]

Therefore, [Ag+] = (1.8×10-10)1/2 = 1.34×10-5 M

Now, the solubility product of AgI = [Ag+][I-]

i.e. 8.3×10-17 = 1.34×10-5 [I-]

i.e. [I-] = 6.2×10-12 M

Hence, even though I- is in low concentrations, it will severely interfere with the Cl- electrode immersed in the corresponding solution and here, the Cl- electrode forms the corresponding I- electrode.

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