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Question

# Solubility product (Ksp) values of the following sparingly soluble salts at 25∘C is : Salts Ksp AgCl 1.8×10−10AgI 1.1×10−16PbCrO4 1.8×10−14AgBr 3.3×10−13 The least soluble and the most soluble salts respectively are:

A
PbCrO4 and AgCl
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B
AgI and AgCl
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C
AgI and PbCrO4
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D
AgI and AgBr
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Solution

## The correct option is B AgI and AgClHere, all the salts are of AB type: The equilibrium relation of all the undissolved salts with their respective ions is of the type: AB (s)⇌A+ (aq)+B− (aq) When the stoichiometry of the precipitated salts is the same, then the salts are precipitated in the increasing order of their Ksp value. So, the least soluble salt is AgI and the most soluble is AgCl

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