Identify conjugate acid and conjugate base in the following reaction. H2PO4− (aq) + H2O (l) ⇌ HPO42− (aq) + H3O+ (aq)a) HPO42− (conjugate acid), H3O+ (conjugate base) b) HPO42− (conjugate base), H3O+ (conjugate acid)c) H2PO4− (conjugate acid), H2O (conjugate base)d) H2PO4− (conjugate base), H2O (conjugate acid)

HPO 4 2− (conjugate base), H 3 O + (conjugate acid)

Identify conjugate acid and conjugate base in the following reaction. H 2 PO 4 − (aq) + H 2 O (l) ⇌ HPO 4 2 − (aq) + H 3 O + (aq) a) HPO 4 2 − (conjugate acid), H 3 O + (conjugate base) b) HPO 4 2 − (conjugate base), H 3 O + (conjugate acid) c) H 2 PO 4 − (conjugate acid), H 2 O (conjugate base) d) H 2 PO 4 − (conjugate base), H 2 O (conjugate acid)

Here we have to identify the conjugate acid and conjugate base in the following reaction. Now first of all when we refer to conjugate acids and bases those are the products. So basically we have to see how have things changed from going to the react from the reactant side to the product side. If we take a look we have H 2 PO 4 minuteus, and all of a sudden it becomes HPO 42 minuteus. We should notice that we've lost an H plus. We went from water as a liquid to H three zero plus, so we gained an H plus. So what must have happened here is that this, dihydrogen phosphate or bihydrogen phosphate gave an h plus away. So it acts as the acid, water as the base. It lost an h plus to create a conjugate base. So this is the conjugate base. This is the form after you've lost an h plus. Water gained an H+ and became H three 0+, so this is our conjugate acid. So based on that, remember when referring to conjugates we're referring to the products, so it's either A or B. And then we're gonna say hydrogen phosphate here, HPO4-two- is the conjugate base, and then the hydronium ion was the conjugate acid. So option B is our correct choice.

Identify conjugate acid and conjugate base in the following reaction. H 2 PO 4 − (aq) + H 2 O (l) ⇌ HPO 4 2 − (aq) + H 3 O + (aq) a) HPO 4 2 − (conjugate acid), H 3 O + (conjugate base) b) HPO 4 2 − (conjugate base), H 3 O + (conjugate acid) c) H 2 PO 4 − (conjugate acid), H 2 O (conjugate base) d) H 2 PO 4 − (conjugate base), H 2 O (conjugate acid)

HPO 4 2− (conjugate base), H 3 O + (conjugate acid)

HPO 4 2− (conjugate acid), H 3 O + (conjugate base)

H 2 PO 4 − (conjugate acid), H 2 O (conjugate base)

H 2 PO 4 − (conjugate base), H 2 O (conjugate acid)

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
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13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
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21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

17. Acid and Base Equilibrium

Bronsted-Lowry Acids and Bases

General Chemistry

17. Acid and Base Equilibrium

Bronsted-Lowry Acids and Bases

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Multiple Choice

Identify conjugate acid and conjugate base in the following reaction.
H₂PO₄⁻ (aq) + H₂O (l) ⇌ HPO₄²⁻ (aq) + H₃O⁺ (aq)
a) HPO₄²⁻ (conjugate acid), H₃O⁺ (conjugate base)
b) HPO₄²⁻ (conjugate base), H₃O⁺ (conjugate acid)
c) H₂PO₄⁻ (conjugate acid), H₂O (conjugate base)
d) H₂PO₄⁻ (conjugate base), H₂O (conjugate acid)

HPO₄²⁻ (conjugate acid), H₃O⁺ (conjugate base)

HPO₄²⁻ (conjugate base), H₃O⁺ (conjugate acid)

H₂PO₄⁻ (conjugate acid), H₂O (conjugate base)

H₂PO₄⁻ (conjugate base), H₂O (conjugate acid)

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Verified step by step guidance

Understand the concept of conjugate acid-base pairs: In a chemical reaction, a conjugate acid is formed when a base gains a proton (H⁺), and a conjugate base is formed when an acid loses a proton.

Identify the acid and base in the reactants: In the given reaction, H₂PO₄⁻ acts as an acid because it donates a proton, and H₂O acts as a base because it accepts a proton.

Determine the conjugate base: When H₂PO₄⁻ donates a proton, it forms HPO₄²⁻. Therefore, HPO₄²⁻ is the conjugate base of H₂PO₄⁻.

Determine the conjugate acid: When H₂O accepts a proton, it forms H₃O⁺. Therefore, H₃O⁺ is the conjugate acid of H₂O.

Match the identified conjugate acid and base with the options provided: The correct identification is HPO₄²⁻ as the conjugate base and H₃O⁺ as the conjugate acid.