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Ammonia molecules react with water to form a solution that contains ammonium ions and hydroxide ions. How should water be classified in this reaction?

[tex]\[ NH_3(g) + H_2O(\ell) \rightarrow NH_4^+(aq) + OH^-(aq) \][/tex]

A. As a Brønsted-Lowry acid, because it donates a proton
B. As a Brønsted-Lowry acid, because it accepts a proton
C. As a Brønsted-Lowry base, because it donates a proton
D. As a Brønsted-Lowry base, because it accepts a proton


Sagot :

To classify the role of water in the given chemical reaction:
[tex]\[ NH_3(g) + H_2O (\ell) \rightarrow NH_4^+ (aq) + OH^- (aq) \][/tex]

we need to examine how water participates in this reaction according to the Brønsted-Lowry theory. The Brønsted-Lowry definition states:

- An acid is a substance that donates a proton (H⁺).
- A base is a substance that accepts a proton (H⁺).

Let's look at what happens in the reaction:

1. Ammonia [tex]\( NH_3 \)[/tex] gains a proton (H⁺) to form ammonium [tex]\( NH_4^+ \)[/tex].
2. Water [tex]\( H_2O \)[/tex] loses a proton (H⁺) to form hydroxide ion [tex]\( OH^- \)[/tex].

In this reaction:
- Water [tex]\( H_2O \)[/tex] donates a proton to ammonia, resulting in the formation of the hydroxide ion.
- Ammonia [tex]\( NH_3 \)[/tex] accepts the proton from water, resulting in the formation of the ammonium ion.

According to the Brønsted-Lowry definition:
- Because water [tex]\( H_2O \)[/tex] donates a proton, it behaves as a Brønsted-Lowry acid in this reaction.

Therefore, the correct classification of water in this reaction is:

A. As a Brønsted-Lowry acid, because it donates a proton.
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