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Write the disproportionation reaction of...

Write the disproportionation reaction of `H_(3)PO_(3)`

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To write the disproportionation reaction of \( H_3PO_3 \) (phosphorous acid), we need to identify the changes in oxidation states that occur during the reaction. Disproportionation reactions involve the same species being oxidized and reduced simultaneously. ### Step-by-Step Solution: 1. **Identify the Species**: We start with phosphorous acid, \( H_3PO_3 \). 2. **Determine the Oxidation States**: In \( H_3PO_3 \), phosphorus has an oxidation state of +3. In the products, we will have \( H_3PO_4 \) (where phosphorus has an oxidation state of +5) and \( PH_3 \) (where phosphorus has an oxidation state of -3). ...
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Give the disproportionation reaction of H_3PO_3 .

Write the disproportionation reaction of ClO^(-) to Cl^(-) and ClO_(3)^(-)

(a) Give reasons : (i) H_(3)PO_(3) undergoes disproportionation reaction but H_(3)PO_(4) does not . (ii) When Cl_(2) reacts with excess of F_(2), ClF_(3) is formed and not FCl_(3) . (iii) Dioxygen is a gas while Sulphur is a solid at room temperature . (b) Draw the structure of the following : (i) XeF_(4) " " (ii) HClO_(3)

Equivalent weight of H_(3)PO_(2) when it disproportionates into PH_(3) and H_(3)PO_(3) is (mol.wt. of H_(3)PO_(2)=M )

What is the basicity of H_(3)PO_(3) ?

What is the basicity of H_(3)PO_(3) ?

STATEMENT-1: In disproportionation reaction 50% of the substance is oxidised and remaining 50% is reduced. STATEMENT-2: Decomposition of H_(2)O_(2) is not a disproportionation reaction. STATEMENT-3: Both HNO_(2) & H_(3)PO_(3) can undergo disproportionation reaction.

What is the basicity of H_(3)PO_(4) ?

Equivalent mass of H_3PO_2 when it disproportionate into PH_3 and H_3PO_3 is (mol. wt. of H_3PO_2 = M ) :

Which of the following reaction does not produce H_(3)PO_(4) ?