(B) The reaction is: $\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$.In this reaction,$Cl_2$ undergoes disproportionation.The products are $HOCl$

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If the product is an oxyacid with an $-ous$ suffix.

(B) The reaction is: $\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$.In this reaction,$Cl_2$ undergoes disproportionation.The products are $HOCl$ (hypochlorous acid) and $HCl$ (hydrochloric acid).$HOCl$ is an oxyacid of chlorine where the oxidation state of $Cl$ is $+1$,which corresponds to the $-ous$ suffix (hypochlorous acid).$HCl$ is a binary acid (hydrohalic acid),not an oxyacid.Therefore,the product $HOCl$ is an oxyacid with an $-ous$ suffix.

Class 11 Chemistry Redox Reactions Auto oxidation and Disproportionation

Difficult

In the following reaction,identify the nature of the product formed by the complete hydrolysis of the underlined atom at $R.T.$:
$\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$

A
If the product is an oxyacid with an $-ic$ suffix.
B
If the product is an oxyacid with an $-ous$ suffix.
C
If the products are two oxyacids,one with an $-ic$ suffix and the other with an $-ous$ suffix.
D
If the product is not an oxyacid,neither with an $-ic$ suffix nor with an $-ous$ suffix.

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Redox Reactions

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Auto oxidation and Disproportionation

Assign $A, B, C, D$ from the given type of reaction.
$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$

Medium

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In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$

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When $P_4$ reacts with caustic soda,the products are $PH_3$ and $NaH_2PO_2$. This reaction is an example of

MediumIIT 1980

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Which of the following species do not show disproportionation reaction and why?
$ClO^{-}, ClO_{2}^{-}, ClO_{3}^{-}$ and $ClO_{4}^{-}$
Also write the reaction for each of the species that disproportionates.

Medium

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Write the balanced chemical equation for the reaction of $Cl_{2}$ with hot and concentrated $NaOH$. Is this reaction a disproportionation reaction? Justify.

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In the following reaction,identify the nature of the product formed by the complete hydrolysis of the underlined atom at $R.T.$:$\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$

Similar Questions

Assign $A, B, C, D$ from the given type of reaction.$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$

In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$

When $P_4$ reacts with caustic soda,the products are $PH_3$ and $NaH_2PO_2$. This reaction is an example of

Which of the following species do not show disproportionation reaction and why?$ClO^{-}, ClO_{2}^{-}, ClO_{3}^{-}$ and $ClO_{4}^{-}$Also write the reaction for each of the species that disproportionates.

Write the balanced chemical equation for the reaction of $Cl_{2}$ with hot and concentrated $NaOH$. Is this reaction a disproportionation reaction? Justify.

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In the following reaction,identify the nature of the product formed by the complete hydrolysis of the underlined atom at $R.T.$:
$\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$

Assign $A, B, C, D$ from the given type of reaction.
$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$

In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$

Which of the following species do not show disproportionation reaction and why?
$ClO^{-}, ClO_{2}^{-}, ClO_{3}^{-}$ and $ClO_{4}^{-}$
Also write the reaction for each of the species that disproportionates.