The dibasic oxoacid of phosphorus on disproportionation gives two products $A$ and $B$. $A$ and $B$ are respectively
- A$HPO_3, PH_3$
- B$H_3PO_2, H_2O$
- C$H_3PO_4, PH_3$
- D$H_4P_2O_6, H_3PO_2$
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Similar Questions
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.
$ClO^{-}, ClO_{2}^{-}, ClO_{3}^{-}$ and $ClO_{4}^{-}$
Also write the reaction for each of the species that disproportionates.
Medium
View SolutionWhat is meant by 'disproportionation' of an oxidation state? Give an example.
Easy
View SolutionWhich one of the following is a disproportionation reaction?
In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$
Difficult
View SolutionAssign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$
$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$
Medium
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