Textbook Question
Write the formula for the conjugate acid of each base. a. NH3 b. ClO4– c. HSO4– d. CO32–
Ch.16 - Acids and Bases
Chapter 16, Problem 41b
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCl
Verified step by step guidance1
Identify the acid: The given acid is hydrochloric acid (HCl).
Determine if the acid is strong or weak: HCl is a strong acid.
Strong acids completely dissociate in water, so they do not have an acid ionization constant (K_a) expression.
For strong acids like HCl, the concentration of hydrogen ions [H^+] is equal to the initial concentration of the acid.
Since HCl is a strong acid, there is no need to write a K_a expression.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Strong vs. Weak Acids
Strong acids completely dissociate in water, releasing all their protons (H+), while weak acids only partially dissociate. This distinction is crucial for understanding acid behavior in solution and predicting the extent of ionization.
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Weak Acid-Strong Base Titration Curve
Acid Ionization Constant (Ka)
The acid ionization constant (Ka) quantifies the strength of a weak acid by measuring the equilibrium concentration of its ions in solution. It is defined by the expression Ka = [H+][A-]/[HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the undissociated acid.
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Hydrochloric Acid (HCl)
Hydrochloric acid (HCl) is classified as a strong acid because it completely dissociates in aqueous solution. This means that when HCl is dissolved in water, it releases all of its hydrogen ions, resulting in a high concentration of H+ ions and a low pH.
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Related Practice
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Both H2O and H2PO4– are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.
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