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Which of the following is an example of a Brønsted-Lowry acid?

A. [tex]NH _3[/tex]
B. [tex]F ^{-}[/tex]
C. [tex]NH _4{ }^{+}[/tex]
D. [tex]BF _3[/tex]

Sagot :

GinnyAnswer
To determine which of the given substances is a Brønsted-Lowry acid, we need to understand the definition of a Brønsted-Lowry acid. According to the Brønsted-Lowry theory, an acid is a substance that can donate a proton (H⁺), while a base is a substance that can accept a proton.

Let's go through each of the options:

A. NH₃ (Ammonia):
- Ammonia tends to accept a proton to form NH₄⁺ (ammonium ion), which means it behaves as a Brønsted-Lowry base.

B. F⁻ (Fluoride ion):
- The fluoride ion can accept a proton to become HF (hydrofluoric acid), meaning it acts as a Brønsted-Lowry base.

C. NH₄⁺ (Ammonium ion):
- The ammonium ion can donate a proton to form NH₃ (ammonia), indicating that it behaves as a Brønsted-Lowry acid.

D. BF₃ (Boron trifluoride):
- Boron trifluoride tends to accept pairs of electrons rather than protons, which is more aligned with the Lewis theory of acids and bases, not the Brønsted-Lowry theory.

Given this information, the correct example of a Brønsted-Lowry acid from the provided options is:
C. NH₄⁺ (Ammonium ion).
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