In the following reaction, which substance is acting as the Brønsted-Lowry acid?
NH3 + H2O NH4+ + OH
Where is the arrow?
NH3 + HOH ==> NH4^+ + OH^-
Remember the Bronsted-Lowry theory says that the acid is the molecule that donates a proton. Which molecule on the left has one less H^+ on the right? The molecule on the left then is the acid. The other molecule is the base.
In the given reaction, NH3 (ammonia) is acting as the Brønsted-Lowry acid.
To determine which substance is acting as the Brønsted-Lowry acid in the reaction NH3 + H2O -> NH4+ + OH-, we need to identify the species that donates a proton (H+) in the reaction.
In this case, NH3 (ammonia) donates a proton while forming the NH4+ (ammonium ion). The H2O (water) acts as the Brønsted-Lowry base, accepting the proton to form OH- (hydroxide ion).
To summarize:
- The Brønsted-Lowry acid is NH3 (ammonia), as it donates a proton (H+).
- The Brønsted-Lowry base is H2O (water), as it accepts the proton to form OH- (hydroxide ion).
Note: In Brønsted-Lowry acid-base theory, acids are defined as substances that donate protons (H+ ions), while bases are defined as substances that accept protons.
Aha! Homework dumping, I see.
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