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Lecture_36_120611

# Lecture_36_120611 - Lecture 36 pH Goals Use the ion-product...

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Lecture 36: pH Goals: Use the ion-product constant of water to calculate the [H 3 O + ] and [OH - ] in an aqueous solution. Calculate pH from [H3O+]; given the pH, calculate the [H 3 O + ] and [OH - ] of a solution. Outline (Timberlake 10.3-10.4): ± Ionization of Water (10.3) ± The pH Scale (10.4) Problems for Extra Practice: 10.33, 10.35, 10.37, 10.41, 10.43, 10.45

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Acid Dissociation Constant, K a • In a weak acid, the rate of the dissociation of the acid is equal to the rate of the association. HA + H 2 O H 3 O + + A • The equilibrium expression is: K eq = [H 3 O + ][A ] [HA][H 2 O] • Because the concentration of H 2 O is constant, the K a expression for a weak acid is: K a = [H 3 O + ][A ] [HA]
Direction of a Reaction • In any acid-base reaction, there are two acids and two bases – One acid is stronger than the other acid – One base is stronger than the other base • By comparing their relative strengths, we can determine the direction of the reaction HF(aq) + H 2 O(l) H 3 O+(aq) + F - (aq)

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Conjugate Acid-Base Pairs
Direction of a Reaction • In any acid-base reaction, there are two acids and two bases – One acid is stronger than the other acid – One base is stronger than the other base • By comparing their relative strengths, we can determine the direction of the reaction HF(aq) + H 2 O(l) H 3 O + (aq) + F - (aq) Weaker acid Weaker base Stronger acid Stronger base

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Acid Characteristics and K a K a = [H 3 O + ][A - ] [HA] Acid dissociation constant
Some Acid Dissociation Constants K a values for some weak acids are shown in Table 10.4.

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Lecture_36_120611 - Lecture 36 pH Goals Use the ion-product...

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