Which of the following shows a Bronsted-Lowry acid reacting?
A. [tex]$CO + NO _2 \rightarrow CO _2+ NO$[/tex]
B. [tex]$NH _3+ H ^{+} \rightarrow NH _4{ }^{+}$[/tex]
C. [tex]$CO _3^{2-}+ H ^{+} \rightarrow HCO _3^{-}$[/tex]
D. [tex]$HCl + H _2 O \rightarrow H _3 O ^{+}+ Cl ^{-}$[/tex]
Answer (2)
A Bronsted-Lowry acid donates a proton.
Examine each reaction for proton donation.
H Cl donates a proton in the reaction H Cl + H 2 O → H 3 O + + C l − .
The reaction showing a Bronsted-Lowry acid is H Cl + H 2 O → H 3 O + + C l − .
Explanation
Understanding Bronsted-Lowry Acids A Bronsted-Lowry acid is a substance that donates a proton (H+) in a chemical reaction. We need to identify the reaction where a species donates a proton.
Analyzing Each Reaction Let's examine each reaction to see if a species is donating a proton (H+):
CO + N O 2 → C O 2 + NO : In this reaction, there is no proton transfer.
N H 3 + H + → N H 4 + : In this reaction, H + is reacting with N H 3 , so H + is the acid.
C O 3 2 − + H + → H C O 3 − : In this reaction, H + is reacting with C O 3 2 − , so H + is the acid.
H Cl + H 2 O → H 3 O + + C l − : In this reaction, H Cl donates a proton to H 2 O to form H 3 O + and C l − . Thus, H Cl is acting as a Bronsted-Lowry acid.
Identifying the Correct Reaction Therefore, the reaction that shows a Bronsted-Lowry acid reacting is H Cl + H 2 O → H 3 O + + C l − .
Examples
Bronsted-Lowry acids are crucial in many chemical processes, including industrial production and biological reactions. For example, in the human body, hydrochloric acid (HCl) in the stomach helps digest food by donating protons to break down complex molecules. Similarly, in the production of fertilizers, ammonia (NH3) reacts with sulfuric acid (H2SO4), where sulfuric acid acts as a Bronsted-Lowry acid by donating protons to ammonia, forming ammonium sulfate, a key ingredient in fertilizers. Understanding Bronsted-Lowry acids helps us comprehend and control these essential chemical reactions.
The reaction that shows a Bronsted-Lowry acid is H Cl + H 2 O → H 3 O + + C l − because HCl donates a proton to water. In other options, either no proton is transferred or the acid is not the one donating the proton. Understanding this concept is crucial as it helps frame chemical reactions appropriately in the context of acid-base chemistry.
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