Multiple Choice
In the chemical equation HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO₂⁻(aq), which species act as Bronsted-Lowry acids?
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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Which of the following explains why HCO3^- is a stronger conjugate base than CO3^2^-?
A
HCO3^- is less stable than CO3^2^- due to its higher charge.
B
HCO3^- is a stronger conjugate base because it is the conjugate base of a weak acid, H2CO3.
C
HCO3^- has a higher electronegativity than CO3^2^-.
D
HCO3^- can donate a proton more easily than CO3^2^-.
Verified step by step guidance1
Identify the concept of conjugate bases: A conjugate base is formed when an acid donates a proton (H+). The strength of a conjugate base is inversely related to the strength of its corresponding acid.
Understand the relationship between acid strength and conjugate base strength: A weak acid has a strong conjugate base, while a strong acid has a weak conjugate base.
Analyze the given acids: H2CO3 (carbonic acid) is a weak acid, which means its conjugate base, HCO3^-, is relatively strong.
Compare the stability of the conjugate bases: CO3^2^- is the conjugate base of HCO3^-, which is a weaker acid than H2CO3. Therefore, CO3^2^- is a weaker conjugate base compared to HCO3^-.
Conclude that HCO3^- is a stronger conjugate base because it is derived from the weaker acid H2CO3, making it more capable of accepting a proton compared to CO3^2^-.
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