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(C) $1.$ Orthophosphorous acid $(H_3PO_3)$: $3(+1) + x + 3(-2) = 0 \Rightarrow x = +3$ $2.$ Pyrophosphorous acid $(H_4P_2O_5)$: $4(+1) + 2x + 5(-2) =

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Orthophosphorous and pyrophosphorous acids

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(C) $1.$ Orthophosphorous acid $(H_3PO_3)$: $3(+1) + x + 3(-2) = 0 \Rightarrow x = +3$ $2.$ Pyrophosphorous acid $(H_4P_2O_5)$: $4(+1) + 2x + 5(-2) = 0$ $\Rightarrow 2x = 6$ $\Rightarrow x = +3$ $3.$ Hypophosphoric acid $(H_4P_2O_6)$: $4(+1) + 2x + 6(-2) = 0$ $\Rightarrow 2x = 8$ $\Rightarrow x = +4$ $4.$ Pyrophosphoric acid $(H_4P_2O_7)$: $4(+1) + 2x + 7(-2) = 0$ $\Rightarrow 2x = 10$ $\Rightarrow x = +5$ Therefore,the pair with $+3$ oxidation state is Orthophosphorous and pyrophosphorous acids.

The pair in which phosphorus atoms have a formal oxidation state of $+3$ is:

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