'Percent dissociation' diaporamas de présentation

CHAPTER 17

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Acid-Base Equilibria

Acid-Base Equilibria. The reaction of weak acids with water, OR the reaction of weak bases with water, always results in an equilibrium!! The equilibrium constant for the reaction of a weak acid with water is K a. [H 3 O+] [F - ]. K a =. [HF]. Acid-Base Equilibria.

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Acids and Bases

Acids and Bases. Acid/Base Definitions. Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases are proton acceptors. Acid Dissociation. HA ? H + + A -

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Acids and Bases

Acids and Bases. Acid/Base Definitions. Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases are proton acceptors. Acid Dissociation. HA ? H + + A -

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The Equilibrium of Weak Acids and Bases

The Equilibrium of Weak Acids and Bases. The Equilibrium of Weak Acids and Bases. The dissociation of an acidic or basic compound in aqueous solution produces ions that interact with water (REVIEW!) Pure water contains a few ions, produced by the dissociation of water molecules:.

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Acid-Base Strength: Ka, Kb, Kw

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Ka, Kb

Ka, Kb. Acid and Base Dissociation Constants. How do we calculate [H + ] for a weak acid?. We know that strong acids dissociate 100% and that, therefore, the [H + ] equals that [acid] that we start with What about weak acids?

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Ka, Kb

Ka, Kb. Acid and Base Dissociation Constants. How do we calculate [H + ] for a weak acid?. We know that strong acids dissociate 100% and that, therefore, the [H + ] equals that [acid] that we start with What about weak acids?

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The Acid Dissociation Constant, K a

The Acid Dissociation Constant, K a. The Acid Dissociation Constant. When a weak acid dissolves in water, it does not completely dissociate.

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The Acid Dissociation Constant, K a

The Acid Dissociation Constant, K a. The Acid Dissociation Constant. When a weak acid dissolves in water, it does not completely dissociate.

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Mixing weak acids

Mixing weak acids. Calculate the pH of a solution that contains 1.00 M HCN ( K a = 6.2 x10 -10 ) and 5.00 M HNO 2 ( K a = 4.0 x 10 -4 ). Also calculate the concentration of cyanide ion (CN - ) in this solution at equilibrium. Percent Dissociation.

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