Multiple Choice
Which of the following equations correctly shows NO₂⁻ acting as a Bronsted-Lowry base?
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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The following equation shows the equilibrium in an aqueous solution of ethylamine:C2H5NH2(aq) + H2O(l) ⇌ C2H5NH3+(aq) + OH−(aq)Which of the following represents a conjugate acid-base pair?
A
H2O and C2H5NH3+
B
C2H5NH2 and OH−
C
H2O and OH−
D
C2H5NH2 and C2H5NH3+
Verified step by step guidance1
Identify the concept of conjugate acid-base pairs. In a chemical reaction, a conjugate acid-base pair consists of two species that transform into each other by the gain or loss of a proton (H⁺).
Examine the given equilibrium reaction: \( \text{C}_2\text{H}_5\text{NH}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{C}_2\text{H}_5\text{NH}_3^+(\text{aq}) + \text{OH}^−(\text{aq}) \).
Identify the species that undergoes a change in protonation. \( \text{C}_2\text{H}_5\text{NH}_2 \) gains a proton to become \( \text{C}_2\text{H}_5\text{NH}_3^+ \), indicating that these two are a conjugate acid-base pair.
Understand that \( \text{C}_2\text{H}_5\text{NH}_2 \) is the base, and \( \text{C}_2\text{H}_5\text{NH}_3^+ \) is the conjugate acid formed after the base accepts a proton.
Review the other options: \( \text{H}_2\text{O} \) and \( \text{OH}^- \) are not a conjugate acid-base pair in this context because \( \text{OH}^- \) is formed by the loss of a proton from \( \text{H}_2\text{O} \), but \( \text{H}_2\text{O} \) is not directly related to \( \text{C}_2\text{H}_5\text{NH}_3^+ \) in terms of proton transfer.
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