AP EAMCET · Chemistry · Ionic Equilibrium

The solubility products of three sparingly soluble salts \(A B, A_2 B\) and \(A B_3\) are respectively \(4.0 \times 10^{-20}, 3.2 \times 10^{-11}\) and \(2.7 \times 10^{-31}\).
The increasing order of their solubility is

A \(A B < A B_3 < A_2 B\)
B \(A B_3 < A B < A_2 B\)
C \(A_2 B < A B_3 < A B\)
D \(A_2 B < A B < A B_3\)

Verified Solution

Answer & Solution

Correct Answer

(A) \(A B < A B_3 < A_2 B\)

Step-by-step Solution

Detailed explanation

The solubility product is defined as the product of concentrations of the ions raised to a power equal to the number of times the ions occur in the equation representing the dissociation of electrolyte at given temperature. (When the solution is saturated.) (i) Electrolyte of…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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The solubility products of three sparingly soluble salts \(A B, A_2 B\) and \(A B_3\) are respectively \(4.0 \times 10^{-20}, 3.2 \times 10^{-11}\) and \(2.7 \times 10^{-31}\).The increasing order of their solubility is

Step-by-step Solution

The solubility products of three sparingly soluble salts \(A B, A_2 B\) and \(A B_3\) are respectively \(4.0 \times 10^{-20}, 3.2 \times 10^{-11}\) and \(2.7 \times 10^{-31}\).
The increasing order of their solubility is