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A. using the five-step method, predict the predominant Bronsted-Lowry acid base reaction when solutions of ammonium chloride and sodium hydrogen carbonate are combined.
Accepted Answer
Step 1. Write the balanced chemical equation for the reaction.
NH₄Cl(aq) + NaHCO₃(aq) → NH₄HCO₃(aq) + NaCl(aq)
Step 2. Identify the Bronsted-Lowry acid and base.
The Bronsted-Lowry acid is the species that donates a proton (H⁺), and the Bronsted-Lowry base is the species that accepts a proton.
In this reaction, NH₄⁺ is the Bronsted-Lowry acid and HCO₃⁻ is the Bronsted-Lowry base.
Step 3. Write the conjugate acid-base pairs.
The conjugate acid of the Bronsted-Lowry base is the species that is formed when the base accepts a proton.
The conjugate base of the Bronsted-Lowry acid is the species that is formed when the acid donates a proton.
In this reaction, the conjugate acid of HCO₃⁻ is H₂CO₃, and the conjugate base of NH₄⁺ is NH₃.
Step 4. Determine the relative strengths of the acids and bases.
The stronger acid is the one that donates protons more readily. The stronger base is the one that accepts protons more readily.
In this reaction, H₂CO₃ is a stronger acid than NH₄⁺, and NH₃ is a stronger base than HCO₃⁻.
Step 5. Predict the direction of the reaction.
The reaction will proceed in the direction that favors the formation of the weaker acid and the weaker base.
In this reaction, the weaker acid is NH₄⁺ and the weaker base is HCO₃⁻. Therefore, the reaction will proceed in the direction of the formation of NH₄HCO₃ and NaCl.
Conclusion:
The predominant Bronsted-Lowry acid-base reaction when solutions of ammonium chloride and sodium hydrogen carbonate are combined is the formation of ammonium hydrogen carbonate and sodium chloride.
NH₄Cl(aq) + NaHCO₃(aq) → NH₄HCO₃(aq) + NaCl(aq)
Step 2. Identify the Bronsted-Lowry acid and base.
The Bronsted-Lowry acid is the species that donates a proton (H⁺), and the Bronsted-Lowry base is the species that accepts a proton.
In this reaction, NH₄⁺ is the Bronsted-Lowry acid and HCO₃⁻ is the Bronsted-Lowry base.
Step 3. Write the conjugate acid-base pairs.
The conjugate acid of the Bronsted-Lowry base is the species that is formed when the base accepts a proton.
The conjugate base of the Bronsted-Lowry acid is the species that is formed when the acid donates a proton.
In this reaction, the conjugate acid of HCO₃⁻ is H₂CO₃, and the conjugate base of NH₄⁺ is NH₃.
Step 4. Determine the relative strengths of the acids and bases.
The stronger acid is the one that donates protons more readily. The stronger base is the one that accepts protons more readily.
In this reaction, H₂CO₃ is a stronger acid than NH₄⁺, and NH₃ is a stronger base than HCO₃⁻.
Step 5. Predict the direction of the reaction.
The reaction will proceed in the direction that favors the formation of the weaker acid and the weaker base.
In this reaction, the weaker acid is NH₄⁺ and the weaker base is HCO₃⁻. Therefore, the reaction will proceed in the direction of the formation of NH₄HCO₃ and NaCl.
Conclusion:
The predominant Bronsted-Lowry acid-base reaction when solutions of ammonium chloride and sodium hydrogen carbonate are combined is the formation of ammonium hydrogen carbonate and sodium chloride.
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