Respuesta :
Answer : The equation that show [tex]H_2PO_4^-[/tex] act as a base with [tex]H_2O[/tex] act as an acid is:
[tex]H_2PO_4^-(aq)+H_2O(aq)\rightleftharpoons H_3PO_4(aq)+OH^-(aq)[/tex]
Explanation :
According to the Bronsted Lowry concept, Bronsted Lowry-acid is a substance that donates one or more hydrogen ion in a reaction and Bronsted Lowry-base is a substance that accepts one or more hydrogen ion in a reaction.
Or we can say that, conjugate acid is proton donor and conjugate base is proton acceptor.
The given equilibrium reaction will be,
[tex]H_2PO_4^-(aq)+H_2O(aq)\rightleftharpoons H_3PO_4(aq)+OH^-(aq)[/tex]
In this reaction, [tex]H_2O[/tex] is an acid that donate a proton or hydrogen to [tex]H_2PO_4^-[/tex] base and it forms [tex]OH^-[/tex] and [tex]H_3PO_4[/tex] are conjugate base and acid respectively.
The equation that shows how H₂PO₄⁻ can act as a base and H₂O acting as an acid is
H₂PO₄⁻ + H₂O → H₃PO₄ + OH⁻
From the question,
We are to write an equation to show how H₂PO₄⁻ can act as a base and H₂O acting as an acid
First, we will define the terms acid and base
According to Brønsted-Lowry
- An acid is any species that is capable of donating a proton (H⁺)
and
- A base is any species that is capable of accepting a proton (H⁺)
Now, the equation that shows how H₂PO₄⁻ can act as a base and H₂O acting as an acid is
H₂PO₄⁻ + H₂O → H₃PO₄ + OH⁻
In the above equation, we can observe that H₂O donated a proton and H₂PO₄⁻ accepted the proton.
This means H₂O acts as an acid while H₂PO₄⁻ acts as the base in the chemical equation.
Hence, the equation that shows how H₂PO₄⁻ can act as a base and H₂O acting as an acid is
H₂PO₄⁻ + H₂O → H₃PO₄ + OH⁻
Learn more here: https://brainly.com/question/10718267
