2018年2月19日 · Why is hypophosphorous acid $(\ce{H3PO2})$ a strong reducing agent? the oxidation state of phosphorous in $\ce{H3PO2}$ is $+5$, as hydrogen and oxygen both are more electronegative than phosphorous, and phosphorous can never increase its oxidation state to more than $+5$, so how can it be a strong reducing agent?

2018年1月14日 · Acidic strength of the acids is determined on the relative tendency to donate one proton. The source where you have seen then $\mathrm{p}K_\mathrm{a}$ value has considered the tendency of first deprotonation of the acids ($\ce{H3PO2}$ deprotonates once, $\ce{H3PO3}$ can deprotonate twice and $\ce{H3PO4}$ can deprotonate thrice).

2022年5月26日 · The structure of hypophosphorous acid is $\ce{HO-PH2=O}$.The electronegativity of phosphorus is near the same as for hydrogen.

2023年10月6日 · When one mole of $\ce{H3PO2}$ is treated with excess $\ce{I2}$ in acidic solution, one mole of $\ce{I2}$ is reduced; on making the solution alkaline, a second mole of $\ce{I2}$ is consumed. I am supposed to find the reaction corresponding to the description. Here is the answer given to me by my teacher: $$\ce{H2O + H3PO2 + I2 -> H3PO3 + 2H ...

If a diazonium salt is reacted with hypophosphorous acid H3PO2 which is a reducing agent the salt is reduced to H. Benzene diazonium chloride when reacts with hypophosphorus acid produces benzene. C 6 H 5 − N + 2 C l − + H 3 P O 2 + H 2 O → C 6 H 6 + N 2 ↑ + H 3 P O 3 + H X

2016年12月26日 · I'm pretty sure it is because phosphorous acid is more polar than phosphoric acid. This is because in the phosphoric acid there are more OHs and an O, so it balances out more towards the center.

Solution for Complete the following reaction equations :(i) C6H5N2Cl + H3PO2 + H2O →(ii) C6H5NH2 + Br2 (aq) →

Solution for N*EN + H3PO2 C. Polymers are naturally occurring or synthetically produced large molecules or compounds which are made up of series of repeating units called monomers.

2019年11月24日 · In the case of $\ce{H3PO2},$ the second and third protons are bonded directly to $\ce{P},$ which is much less electronegative than $\ce{O},$ and consequently these P-H bonds are much less polarized than an $\ce{O-H}$ bond. So these protons are unable to ionize appreciably in aqueous solution.

Oxoacids of Phosphorus are hypophosphoric acid (H3PO4), metaphosphoric acid (HPO2), pyrophosphoric acid (H4P2O7), hypophosphorous acid, phosphorous acid.