Solutions to Bronsted-Lowry Exercises

Exercises

Exercise 1. What is the conjugate base for each of the following?

a) NH₄⁺ NH₃
b) HClO₄ ClO^–
c) HSO₄^– SO₄^2-
d) H₂O OH^–

Exercise 2. What is the conjugate acid for each of the following?

a) HCO₃^– CO₃^2-
b) H₂O H₃O⁺
c) NO₂^– HNO₃
d) CN^– HCN
e) CH₃NH₂ CH₃NH₃⁺

Exercise 3. Write a balanced equation for the dissociation of HCO₃^– in water. Label the conjugate acid-base pairs.

HCO₃^– (aq) + H₂O (l) ⇄ CO₃^2- (aq) + H₃O⁺ (aq)

The two conjugate acid-base pairs are HCO₃^–/CO₃^2- and H₃O⁺/H₂O

Exercise 4. Write a balanced equation for the dissociation of HF in water. Label the conjugate acid-base pairs.

HF (aq) + H₂O (l) ⇄ F^– (aq) + H₃O⁺ (aq)

The conjugate acid-base pairs are HF/F^– and H₃O⁺/H₂O

Back to Bronsted-Lowry Theory

Exercise 5. Write a balanced chemical equation for the reaction of CH₃NH₂ with water. Label the conjugate acid-base pairs.

CH₃NH₂ (aq) + H₂O (l) ⇄ CH₃NH₃⁺ (aq) + OH^– (aq)

The conjugate acid-base pairs are CH₃NH₃⁺/CH₃NH₂ and H₂O/OH^–