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A $0.1\; M$ solution of a certain cation will form a precipitate with $0.1\; M$ solution of all these anions ;

$OH^{-},CO_{3}^{-2},Cl-,SO_{4}-2$ , Which cation fits in the description?
Option: 1
$Ba^{+2}$

Option: 2
$Fe^{+2}$

Option: 3
$Mg^{+2}$

Option: 4
$Pb^{+2}$

Answers (1)

best_answer

Test of Lead(2+) ion -

$PbCl_{2}$ is soluble in hot water but very much less soluble in cold water.
$Pb^{2+}{+} SO^{2-}_{4}\rightarrow PbSO_{4}$

$Pb^{2+}{+} CrO^{2-}_{4}\rightarrow PbCrO_{4}$

$Pb^{2+}{+} 2I^{-}\rightarrow PbI_{2}$

- wherein

$PbSO_{4}\:is\:white\: ppt$

$PbCrO_{4}\:is\:yellow\: ppt$

$PbI_{2}\:is\:yellow\: ppt$

$Pb^{2+}+OH^{-}\; \; \rightarrow \; Pb\left ( OH \right )_{2}\downarrow\left ( white \right );$

$Pb^{2+}+CO_{3}^{2-}\; \; \rightarrow \; PbCO_{3}\downarrow\left ( white \right );$

$Pb^{2+}+2Cl^{-}\; \; \; \rightarrow \; PbCl_{2}\downarrow\left ( white \right );$

$Pb^{2+}\left ( aq. \right )+SO_{_{4}}^{2-}\; \; \rightarrow \; PbSO_{4}\downarrow\left ( white \right );$

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Ritika Harsh

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