Answer :
Answer:
The bronsted- Lowry acid is H₂PO₄⁻
Explanation:
Bronsted-Lowry acid donates a proton (H⁺)
H₂PO₄⁻ + OH⁻ → HPO₄²⁻ + H₂O
In the reaction above, H₂PO₄⁻ is donating the proton to OH⁻ resulting in H₂O and the deprotonated species. This makes it a bronsted-Lowry acid.
Answer:
[tex]H_2 PO_4^-[/tex] is the Bronsted acid.
Explanation:
An acid is a substance that can donate one or more proton
A base is a substance which can accept one or more protons
(Bronsted Acid) + (Bronsted Base) ----> Conjugate Base + Conjugate acid
[tex]H_2 PO_4^- + OH^-< -------- > HPO_4^{-2} + H_2 O[/tex]
Here we see
[tex]H_2 PO_4^-[/tex] donates or loses [tex]H^+[/tex] ion to form [tex]HPO_4^{-2}[/tex]. Hence [tex]H_2 PO_4^-[/tex] is the Bronsted acid (Answer)
Acid loses H+ (proton) to forms conjugate Base [tex](HPO_4^{-2})[/tex]
[tex]OH^-[/tex] is the bronsted Base since it gains or accepts [tex]H^+[/tex] ion to form [tex]H_2 O[/tex]
Base gains H+ (proton) to forms conjugate Acid [tex](H_2 O)[/tex]