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A solution contains 0.05 M of each of NaCl and ${Na}_{2} {CrO}_{4}$ . Solid ${AgNO}_{3}$ is gradually added to it.
Which of the following fats is true?
Given : $K_{SP} (AgCl) {= 1.7 × 10}^{-10} M^{2} {and}_{SP} ({AgCrO}_{4}) {= 1.1 × 10}^{-12}$

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${Cl}^{-}$ ions are precipitated first

${CrO}_{4}^{2-}$ ions are precipitated first

Solubility of ${Ag}_{2} {CrO}_{4}$ is > AgCl (in water when they dissolved separately)

Both ${Cl}^{-}$ and ${CrO}_{4}^{2 -}$ ions are precipitated together

answer is A, D.

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Detailed Solution

When ionic product exceed solubility product then precipitation take place

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