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Ch.16 - Acids and Bases
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.16 - Acids and BasesProblema 42a
Capitolo 16, Problema 42a

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HF

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Identify the acid: HF is hydrofluoric acid.
Determine if the acid is strong or weak: HF is a weak acid.
Explain why HF is a weak acid: HF does not completely dissociate in water, meaning it only partially ionizes.
Write the chemical equation for the ionization of HF: \( \text{HF} \rightleftharpoons \text{H}^+ + \text{F}^- \).
Write the expression for the acid ionization constant \( K_a \): \( K_a = \frac{[\text{H}^+][\text{F}^-]}{[\text{HF}]} \).

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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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03:50
Characteristics of Ka and Kb

Hydrofluoric Acid (HF)

HF is classified as a weak acid because it does not fully dissociate in water. Its ionization can be represented by the equilibrium reaction HF ⇌ H+ + F-, and the corresponding Ka expression can be used to calculate its ionization in solution.
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01:12
Binary Acid Identification Example
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