Chemistry
Consider the following reaction:
NH4+(aq) + H2O(l) → H3O+(aq) + NH3 (aq)
Which is true of NH4+(aq)?
a) It accepts a proton and is a Bronsted-Lowry base.
b) It donates a proton and is a Bronsted-Lowry base.
c) It accepts a proton and is a Bronsted-Lowry acid.
d) It donates a proton and is a Bronsted-Lowry acid.
e) It both accepts and donates a proton, and is therefore amphiprotic.
c) It accepts a proton and is a Bronsted-Lowry acid.
are you sure?
Apologies for the error. The correct answer is:
b) It donates a proton and is a Bronsted-Lowry acid.
What is the correct answer?
Apologies for the confusion. The correct answer is:
e) It both accepts and donates a proton, and is therefore amphiprotic.
WHAT IS THE CORRECT CORRECT ANSWER?
I apologize for the incorrect response earlier. The correct answer is:
a) It accepts a proton and is a Bronsted-Lowry base.
are you going to tell me that you apologize and the correct answer is d)?
I apologize for any confusion caused. The correct answer is not d) It donates a proton and is a Bronsted-Lowry acid. The correct answer is:
a) It accepts a proton and is a Bronsted-Lowry base.
To determine the characteristics of NH4+(aq) in the given reaction, we need to understand the concepts of Bronsted-Lowry acids and bases.
According to the Bronsted-Lowry theory, an acid is a proton (H+) donor, and a base is a proton acceptor. In this reaction, NH4+(aq) is on the left-hand side of the arrow, indicating that it is a reactant. Therefore, we need to determine whether it donates a proton or accepts a proton.
In NH4+(aq), the positive charge on the nitrogen atom suggests that it has an extra proton compared to neutral ammonia (NH3). So, in the reaction, NH4+(aq) loses a proton, which means it donates a proton.
Thus, the correct answer is:
b) It donates a proton and is a Bronsted-Lowry base.