Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side o

Question

Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of the equation below, and also designate the conjugate acid and the conjugate base on the right side. Pick the choice which gives the correct term for one of the substances found in the equation below, based on your designations.

NH3(aq) + HBr(aq)-><- NH4+(aq) + Br -(aq)

a) NH4+ is the Bronsted-Lowry acid in this reaction.

b) NH4+ is the conjugate base in this reaction.

c) NH3 is the conjugate base in this reaction.

d) HBr is the Bronsted-Lowry acid in this reaction.

e) Br - is the Bronsted-Lowry acid in this reaction.

Explanation / Answer

In the equilibrium equation, NH3(aq) is the Bronsted-Lowry base. Its conjugate acid is NH4+(aq). HBr (aq) is considered a strong acid where its conjugate base is Br-(aq). From these designations, d) is the correct choice that gives a correct term for one of the substances. A Bronsted acid donates an H+ to the conjugate base. The Bronsted base in turn accepts the ion from the acid. If you were to reverse the reaction, Br-(aq) is the base that gains a hydrogen in the product and NH4+(aq) donates a hydrogen. I hope this explanation is understandable to you.

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.