With respect to hypochlorite, chlorate and perchlorate ions, choose the correct statement(s).

The hypochlorite ion is the strongest conjugate base.

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The hypochlorite and chlorate ions disproportionate to give rise to an identical set of ions

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The molecular shape of only chlorate ion is influenced by the lone pair of electrons of

C l

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The hypochlorite ion oxidizes the sulfite ion.

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Solution

The correct option is D The hypochlorite ion oxidizes the sulfite ion.
Hypochlorite ion $\to C l O^{-}$
Chlorate ion $\to C l {O_{3}}^{-}$
Perchlorate ion $\to C l {O_{4}}^{-}$
(a) Acidic strength of oxoacids of chlorine depends upon the oxidation state on chlorine.
Acidic nature $H + 1 C l O < H + 5 C l O_{3} < H + 7 C l O_{4}$
Conjugate Base order $C l O^{-} > C l {O_{3}}^{-} C l O_{4}^{-}$

(c) $(+ 1) 3 O C l h o t - - \to (- 1) 2 C l^{-} + (+ 5) C l O_{3}^{-}$ $4 (+ 5) C l O_{3}^{-} a b s e n c e o f c a t a l y s t - ----------- \to l o w e r t e m p e r a t u r e + 7 3 C l O_{4}^{-} + (- 1) C l^{-}$

(d) Lower oxyacids are good oxidizing agents.
$C l O + S O_{3}^{-} \to C l^{-} + S O_{4}^{2 -}$

Suggest Corrections

Similar questions

2 C l O_{3}^{-} ⇌ C l O_{2}^{-} + C l O_{4}^{-}

0.1 M

298 K

E_{C l O_{4}^{-} | C l O_{3}^{-}}^{\circ} = 0.36 V a n d E_{C l O_{3}^{-} | C l O_{2}^{-}}^{\circ} = 0.33 V a t 298 K

2 C l O_{3}^{-} ⇌ C l O_{2}^{-} + C l O_{4}^{-}

0.1 M

298

x

\frac{1}{x}

E_{C l O_{4}^{-} | C l O_{3}^{-}} = 0.36 V a n d E_{C l O_{3}^{-} | C l O_{2}^{-}}^{\circ} = 0.33. V A t 298 K \frac{R T}{F} = 0.06 V \sqrt{10} = 3.16

Three moles of hypochlorite gives 2 moles of chloride and one mole of chlorate. This is:

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