Which statement is incorrect?

Question

BlackTom AI · Accepted Answer

The question asks which statement is incorrect, and the available content provides a single option to evaluate.
Option presents: 'The molar solubility of AgI (Ksp = 8.3 × 10^(−17)) is greater than that of AgCl (Ksp = 1.8 × 10^(−10)) when saturated aqueous solutions are compared.'
To judge this, recall how molar solubility relates to Ksp for sparingly soluble salts. For AgI, the dissolution is AgI(s) ⇌ Ag+(aq) + I−(aq) with Ksp = [Ag+][I−] = s^2, so the molar solubility s_AgI = sqrt(Ksp_AgI).
Similarly, for AgCl, AgCl(s) ⇌ Ag+(aq) + Cl−(aq) with Ksp = [Ag+][Cl−] = s^2, so s_AgCl = sqrt(Ksp_AgCl).
Now plug in the numbers: s_AgI = sqrt(8.3 × 10^(−17)) ≈ 9.1 × 10^(−9) M. On the other hand, s_AgCl = sqrt(1.8 × 10^(−10)) ≈ 1.34 × 10^(−5) M.
These calculations show that the molar solubility of AgCl is far greater than that of AgI. Therefore, the claim that AgI has greater molar solubility than AgCl contradicts the derived values from the given Ksp figures.
The discrepancy arises from comparing two very different solubility magnitudes: AgCl is significantly more soluble than AgI in water, given the respective Ksp values.
Because the statement asserts the opposite relationship, it is inconsistent with the quantitative solubility implications of the provided Ksp values. If there were other options, each would similarly be weighed against the same principle: whether the stated claim aligns with (or deviates from) the Ksp-derived solubilities. In this case, the numerical comparison indicates the given claim does not hold under standard interpretation of Ksp and solubility.

Which statement is incorrect?

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