Is H3PO3 stronger than H3PO4?

The correct acidic strength order is H3PO2>H3PO3>H3PO4.

Which is more reducing H3PO2 or H3PO4?

H3PO2 is a stronger reducing agent than H3PO4 because it has more number of P-H bond.

Is H3PO4 a strong reducing agent?

In case of phosphorous acid, the hydrogen atom is attached directly to phosphorus acid. Hence, phosphorus acid is a reducing agent. However, for phosphoric acid, the hydrogen atom is not directly attached to the phosphorus atom. Hence, phosphoric acid is not a reducing agent.

Which is stronger reducing agent H3PO3 or H3PO2?

Greater the number of element−hydrogen (E−H) bonds present in a compound, greater is the reducing nature of the compound. H3PO2has two P−H bonds while H3PO3 has one P−H bond. Thus, H3PO2 is a stronger reducing agent than H3PO3.

Why is H3PO4 a weaker acid than H3PO3?

H3PO3 is more polar, so the O-H bonds will be weaker, making the H+ easier to come off, and causing H3PO3 to be more acidic than H3PO4.

Why is H3PO3 a stronger reducing agent?

(iii) Greater the number of element−hydrogen (E−H) bonds present in a compound, greater is the reducing nature of the compound. H3PO2 has two P−H bonds while H3PO3 has one P−H bond. Thus, H3PO2 is a stronger reducing agent than H3PO3.

Is H3PO3 an oxidizing agent?

H3PO3 can act as both oxidizing and reducing agent due to the oxidation state of ‘P’ which is +3 in this case. Phosphorus lies in Group 15 of the perodic table whose range of oxidation number is -5 to +5.

Why is H3PO4 a reducing agent?

H3PO3 contains one P-H bond and hence act as a reducing agent but H3PO4 does not contain a P-H bond and hence does not act a reducing agent.

Is H3PO4 oxidising and reducing agent?

H3PO4 is a poor oxidizing agent. In H3PO2 & H3PO3 the oxidation state of P is +1 & +3 respectively, which can be further oxidized to a higher oxidation state. Moreover in H3PO4 the oxidation state of P is +5 which is highest for P.

Why H3PO2 is a good reducing agent?

Originally Answered: Why does H3PO2 behave as reducing agent? Two P – H bonds are present in the hypophosphorus acid. Hence, it behaves as a reducing agent. In presence of H3PO2, AgNO3 is reduced to silver metal.

Why H3PO2 is stronger acid than H3PO3?

Oxygen is a highly electronegative element, and so if there are more oxygen atoms present, more of the molecule’s electron density will be pulled off the O-H bond, weakening it and creating a stronger acid. By the same reasoning, H3PO3 Phosphorous acid is second, and H3PO2 Phosphinic acid is least acidic of the three.

What is the reducing property of H3PO3 and H3PO4?

The reducing property of these acids are based on the no of hydrogen atoms bonded to the central metal atom .In the case of H3PO3 there is one P-H bond which is responsible for it’s reducing character wherehas there is no such bonding in case of H3PO4. In H3PO4 there are 3 P-OH bonds and one P=O bond.

Why is H3PO3 a dibasic acid?

> For H3PO3 and H3PO4 the cor… is a dibasic acid as it has 2 number of replaceable OH groups (Dibasic) attached to phosphorous. The oxyacids of phosphorous are reducing agents. . The reducing nature of these acids is based on the no of hydrogen atoms bonded to the central metal atom.

What is the oxidation state of phosphorus in H3PO3?

in H3PO3, check the oxidation state of P…… it is +3, which can be further oxidised to higher oxidation state. Phosphoric acid, in fact, can act as an oxidising agent at very high temperatures.

Why can’t phosphoric acid act as a reducing agent?

But now lets come to the phosphoric acid or H3PO4, the oxidation state of phosphorous here is +5 that is the highest oxidation state for the P. Hence it cannot be oxidised to higher state and so it cannot act as a reducing agent Phosphoric acid, in fact, can act as an oxidising agent at very high temperatures.