With respect to hypochlorite,chlorate,and per | vedclass

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Question

(B) Hypochlorite ion: $ClO^{-}$Chlorate ion: $ClO_{3}^{-}$Perchlorate ion: $ClO_{4}^{-}$$A.$ Acidic strength order: $HClO < HClO_{3} < HClO_{4}$. Ther

Vedclass · Accepted Answer

$A, B, D$

Vedclass · Answer

(B) Hypochlorite ion: $ClO^{-}$Chlorate ion: $ClO_{3}^{-}$Perchlorate ion: $ClO_{4}^{-}$$A.$ Acidic strength order: $HClO  ClO_{3}^{-} > ClO_{4}^{-}$. Thus,$A$ is correct.$B.$ Hypochlorite ion $(ClO^{-})$: Linear shape. Chlorate ion $(ClO_{3}^{-})$: Trigonal pyramidal shape due to the lone pair on $Cl$. Perchlorate ion $(ClO_{4}^{-})$: Tetrahedral shape. Only the chlorate ion's shape is significantly distorted by a lone pair. Thus,$B$ is correct.$C.$ Disproportionation reactions:$I.$ $3ClO^{-} \rightarrow 2Cl^{-} + ClO_{3}^{-}$$II.$ $4ClO_{3}^{-} \rightarrow 3ClO_{4}^{-} + Cl^{-}$The products are different. Thus,$C$ is incorrect.$D.$ Hypochlorite is a strong oxidizing agent and oxidizes sulfite $(SO_{3}^{2-})$ to sulfate $(SO_{4}^{2-})$: $ClO^{-} + SO_{3}^{2-} \rightarrow Cl^{-} + SO_{4}^{2-}$. Thus,$D$ is correct.Correct statements are $A, B, D$.

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