When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below. NH4+ (aq) + H₂O (1) ≥ NH3 (aq) + H3O+ (aq)
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Bronsted Lowry Base In Inorganic Chemistry
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The pKa of NH4+ is 9.25. Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Explain.
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![When ammonium (\( \text{NH}_4^+ \)) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below.
\[ \text{NH}_4^+ (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{NH}_3 (aq) + \text{H}_3\text{O}^+ (aq) \]
This chemical equation represents the equilibrium that occurs when ammonium ions interact with water. In this reaction:
- \( \text{NH}_4^+ \) (ammonium ion) and \( \text{H}_2\text{O} \) (water) are the reactants.
- \( \text{NH}_3 \) (ammonia) and \( \text{H}_3\text{O}^+ \) (hydronium ion) are the products.
The double arrow (\( \rightleftharpoons \)) indicates that the reaction is at equilibrium, meaning the forward reaction (formation of products) and the reverse reaction (formation of reactants) occur at the same rate. This balance results in constant concentrations of the reactants and products over time.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe38bcf91-c17d-45df-bac4-869cee8c9690%2Fe04483b6-7c29-46e3-9b32-c931a91d896c%2Ftfp7ofg_processed.png&w=3840&q=75)
Given,
Reaction :
pH= 7.4
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