Can H3PO3 act as both oxidising and reducing agent?

In H3PO2 and H3PO3 oxidation state of P is +1 and +3 respectively, which can further be oxidized to a higher oxidation state. So they can act as reducing agents.

Can act as both oxidising and reducing agent?

Hydrogen peroxide (H2O2) acts as both oxidising and reducing agent.

Why does H3PO3 act as reducing agent but H3PO4 does not?

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.

Which elements can act as both oxidizing and reducing agent?

Oxygen can reduce to -2 and oxidize to 0, so it can act as oxidizing and reducing agent both. So, the correct answer is Option C,D.

Is H3PO3 oxidising 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 does Phosphoric acid acts as reducing agent?

Phosphorus acid is H 3 PO 3 Oxidation state of P can. Therefore , P can still lose 2 electrons and reduce the other substance . Therefore , H 3 PO 3 can act as a reducing agent .

Which of the following oxide can act both as an oxidising agent as well as reducing agent?

HNO2 (oxidation number of N is +3). Highest oxidation state of N is +5. So it can undergo both oxidant and reductant.

Which act as an oxidising as well as reducing agent?

Sulphur dioxide acts as an oxidizing agent as well as a reducing agent.

Which compound acts as an oxidizing as well as a reducing agent?

H2​S acts only as reducing agent while SO2​ can act both as reducing agent and oxidising agent.

Assertion: H2​S acts as an oxidizing as well as the reducing agent.

Why H3PO4 is non oxidising?

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.So it cant be oxidized further !! & hence behaves as a non oxidizing acid.

Is H3PO3 an oxidising agent?

Which of the following oxide can act as both reducing and oxidising agent *?

Explanation: Nitric oxide acts as both an oxidising agent and a reducing agent whereas all the other oxides of nitrogen act as oxidising agents only.

Why H3PO4 is non reducing?

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.

Why is H3PO3 a better reducing agent than H3PO2 and H3PO4?

H3PO3 has more P-H bonds (just 1 more) it is a better reducing agent. In H3PO2 and H3PO3 oxidation state of P is +1 and +3 respectively, which can further be oxidized to a higher oxidation state. In H3PO4 oxidation state of P is +5, which is highest for P. H3PO3 is known as phosphorus acid and H3PO4 is known as phosphoric acid.

Is HNO3 a reducing agent or oxidising agent?

Hence, HNO3​cannot act as reducing agent. The oxidation number of nitrogen in HNO3​can only decrease; thus it acts as an oxidising agent. In HNO2​, the oxidation number of nitrogen is +3.

Is phosphorus +3 an oxidizing or reducing agent?

Phosphorus lies in Group 15 of the perodic table whose range of oxidation number is -5 to +5. So in this case +3 lies in between the range and hence it is an intermediate (i.e. it has an intermidiate oxidation number).So it can lose as well as gain electron. Thus it can act both as an oxidizing as well as reducing agent.

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.