Table of Contents
- 1 Is H3PO2 a good reducing agent?
- 2 Can H3PO2 act as both oxidizing and reducing agent?
- 3 Why H3PO2 is stronger reducing agent than H3PO3?
- 4 How do you account for the reducing behavior of H3PO2 based on its structure?
- 5 How do you account for the reducing Behaviour of H3PO2?
- 6 Is H3PO2 a monobasic acid?
- 7 Can I act as both oxidising as well as reducing agent?
- 8 Which is a stronger reducing agent H3PO3 or H3PO2?
- 9 What is the difference between Hypo phosphorous acid (H3PO2) and H3PO4?
Is H3PO2 a good reducing agent?
H3PO2 is a stronger reducing agent than H3PO3 .
Can H3PO2 act as both oxidizing and reducing agent?
HNO2 can act both as a reducing agent and an oxidising agent.
Why H3PO2 is stronger reducing agent than H3PO3?
(iii) H3PO2 is a stronger reducing agent than H3PO3. (i) N atom cannot expand its covalency beyond four due to the absence of vacant d- orbitals, whereas P atom possesses vacant d- orbitals. H3PO2 has two P−H bonds while H3PO3 has one P−H bond. Thus, H3PO2 is a stronger reducing agent than H3PO3.
Why is phosphorous acid a reducing agent?
Both phosphorous acid and its deprotonated forms are good reducing agents, although not necessarily quick to react. They are oxidized to phosphoric acid or its salts. It reduces solutions of noble metal cations to the metals.
Does H3PO3 act as 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.
How do you account for the reducing behavior of H3PO2 based on its structure?
How do you account for the reducing behaviour of H3 PO2 on the basis of its structure? In H3PO2 two H atoms are bonded directly to P atom which imparts reducing character to the acid.
How do you account for the reducing Behaviour of H3PO2?
In H3PO2, two H atoms are bonded directly to P atom which imparts reducing character to the acid where as in H3PO4 all H atoms are bonded to O- atom.
Is H3PO2 a monobasic acid?
H3PO2 is a weak monobasic acid.
Can HNO2 act as oxidising and reducing agent?
HNO2 can act both as a reducing agent and an oxidising agent.
Is phosphorous acid a weak acid?
In aqueous solution, phosphoric acid behaves as a triprotic acid, having three ionizable hydrogen atoms. The hydrogen ions are lost sequentially. an extremely weak acid.
Can I act as both oxidising as well as reducing agent?
Hydrogen peroxide (H2O2) acts as both oxidising and reducing agent.
Which is a stronger reducing agent H3PO3 or H3PO2?
H3PO2 is a stronger reducing agent than H3PO3 . Give reasons. . Give reasons. 1) Reducing agents are those molecules which can donate electrons. 2) The donating elctrons are hydrogen atoms which are bonded to phosphorus atom. has more donating electrons than .
What is the difference between Hypo phosphorous acid (H3PO2) and H3PO4?
We know that In Hypo phosphorous acid (H3PO2) has two H atoms are bonded directly to P atom and In Phosphorous acid (H3PO3) has one H atom is bonded directly to P atom which imparts reducing character to the acid, whereas in H3PO4 there is no H atom bonded directly to P atom hence it does not have reducing character.
Why is p+5 a reducing agent?
The reason it’s a reducing is because that P really wants to “become” +5. Oscar Lanzi in his answer suggests that you can assume the H is H -, but this introduces a complication of this being a hydride, and these are not usually stable in solution.
What is the oxidation state of phosphorus in hypophosphorous acid?
You can do that, but then the hydrogen atoms involved have oxidation state -1 not +1. So the reducing action of hypophosphorous acid is attributed to the negative oxidation state hydrogens. The oxidation state of phosphorus in H 3 PO 4 is indeed +5, but in this case you have only 2 and not 4 oxygens. This means that your P is only +1.