Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH–(aq)
Ch.16 - Acids and Bases
Chapter 16, Problem 37b
Write the formula for the conjugate base of each acid. b. H2SO3
Verified step by step guidance1
Identify the acid given in the problem: \( \text{H}_2\text{SO}_3 \).
Recall that a conjugate base is formed by removing one proton (\( \text{H}^+ \)) from the acid.
Remove one \( \text{H}^+ \) from \( \text{H}_2\text{SO}_3 \) to form the conjugate base.
After removing \( \text{H}^+ \), the remaining species is \( \text{HSO}_3^- \).
Thus, the formula for the conjugate base of \( \text{H}_2\text{SO}_3 \) is \( \text{HSO}_3^- \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Pairs
In acid-base chemistry, a conjugate base is formed when an acid donates a proton (H+). The relationship between an acid and its conjugate base is fundamental to understanding acid-base reactions, as it illustrates how substances can interchange between donating and accepting protons.
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Conjugate Acid-Base Pairs
Sulfurous Acid (H2SO3)
Sulfurous acid (H2SO3) is a weak diprotic acid that can donate two protons. When it loses one proton, it forms its conjugate base, bisulfite (HSO3-), and if it loses both protons, it forms sulfite (SO3^2-). Understanding the structure and behavior of sulfurous acid is essential for identifying its conjugate base.
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Acid-Base Equilibrium
Acid-base equilibrium refers to the balance between acids and their conjugate bases in solution. This concept is crucial for predicting the direction of acid-base reactions and understanding the strength of acids and bases, which is determined by their ability to donate or accept protons in a chemical reaction.
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Related Practice
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO32–(aq) + H2O(l) ⇌ HCO3–(aq) + OH–(aq)
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