'Acid dissociation constant' diaporamas de présentation

Chapter 7

Chapter 7. Acids and Bases. Chapter 7 Acids and Bases. 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The pH Scale 7.4 Calculating the pH of Strong Acid Solutions 7.5 Calculating the pH of weak Acid Solutions 7.6 Bases 7.7 Polyprotic Acids

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Chapter 17 : Additional Aspects of Aqueous Equilibria

Section 2: Buffered Solutions. Chapter 17 : Additional Aspects of Aqueous Equilibria. Introduction. Solutions prepared with common ions have a tendency to resist drastic pH changes even when subjected to the addition of strong acids or bases. Such solutions are called buffered solutions .

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Models of Acids and Bases

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Acids & Bases

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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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Acids, Bases and Buffers

Acids, Bases and Buffers. History and Definitions. Your task is to research the history of acids and bases. Doing this you will need to find out about Arrhenius, Bronsted & Lowry and Lewis.

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Chapter 14 Acids and Bases

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A.P. Chemistry

A.P. Chemistry. Chapter 14 Acid- Base Chemistry. 14.1 Arrhenius Acid- an acid is any substance that dissolves in water to produce H + (H 3 O + ) ions Base- a base is a substance that dissolves in water to produce OH - ions Bronsted - Lowry Acid- an acid is a proton (H + ) donor

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Acids, Bases and Buffers

Acids, Bases and Buffers. History and Definitions. Your task is to research the history of acids and bases. Doing this you will need to find out about Arrhenius, Bronsted & Lowry and Lewis.

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Weak Acids and Bases

Weak Acids and Bases. Mg (s) + 2HCl (aq) --> MgCl 2 (aq) + H 2 (aq) Mg (s) + 2CH 3 COOH (aq) --> Mg(CH 3 COO 2 ) 2 (aq) + H 2 (aq). Working with Weak Acids and Bases. In a solution of a weak acid, what do we have? Acid molecules Small amount of H 3 O +

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Acid Base Equilibrium

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-Ionization Constants of Acids and Bases -Strengths of Acids and Bases

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-Ionization Constants of Acids and Bases -Strengths of Acids and Bases

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Review

Review. 1. What is the Bronsted -Lowry definition of an acid? Of a base? 2. Identify five properties of an acid and five properties of a base.

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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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Chemistry 122

Chemistry 122. Strengths of Acids and Bases. Strong Acids and Bases. The strength of an acid depends on how much it ionizes in water Strong acids completely ionize, releasing all their H + Ex. HCl and H 2 SO 4 HCl (g) + H 2 O (l) ? H 3 O + ( aq ) + Cl - ( aq ) (100% ionized)

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Equilibria of Weak Acids and Bases

Equilibria of Weak Acids and Bases. Strong/Weak Acids. Strong HBr, HI, HCl, HNO 3 , H 2 SO 4 , HClO 4 Readily transfer H + ion to water Completely dissociated Strong electrolyte Weak HC 2 H 3 O 2 , HCN, HNO 2 , HClO, HCO 3 - Does not readily transfer H+ ion Most remains un-ionized.

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Acid/Base Strength

Acid/Base Strength. Strong and Weak Acids. Strong acids : completely ionize in aqueous solutions HCl (g) + H 2 O (l) ? H 3 O + (aq) + Cl - (aq) Weak acids : ionize slightly ion aqueous solutions CH 3 COOH (aq) + H 2 O (l) H 3 O + (aq) + CH 3 COO - (aq)

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