Acids and Bases Chapter 19. I. Describing Acids & Bases.

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Intro to Acids & Bases.

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Presentation transcript:

Acids and Bases Chapter 19

I. Describing Acids & Bases

A. Taste

I. Describing Acids & Bases A. Taste B. Touch

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator

Indicator Substance that is one color in an acidic solution and another color in a basic solution

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus 2. phenolphthalein

I. Describing Acids & Bases A. Taste B. Touch C. Reactions with Metals D. Electrical Conductivity E. Indicator 1. litmus 2. phenolphthalein 3. bromothymol blue

II. Defining Acids & Bases

A. Arrhenius Definition

II. Defining Acids & Bases A. Arrhenius Definition 1. Acid

Arrhenius Acid A substance that dissociates in water to produce H + ion

A. Arrhenius Definition 1. Acid 2. Base II. Defining Acids & Bases

Arrhenius Base A substance that dissociates in water to form OH - ions

B. Bronsted-Lowry Definition II. Defining Acids & Bases

B. Bronsted-Lowry Definition 1. Acid II. Defining Acids & Bases

Bronsted-Lowry Acid A substance that can donate a proton

B. Bronsted-Lowry Definition 1. Acid 2. Base II. Defining Acids & Bases

Bronsted-Lowry Base A substance that can accept a proton

B. Bronsted-Lowry Definition C. Polyprotic Acids II. Defining Acids & Bases

Polyprotic Acids Those acids that donate more than one proton

III. Reactions

A. What does an acid do in water?

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water?

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base 2. Bronsted-Lowry Base

III. Reactions A. What does an acid do in water? 1. Arrhenius Acid 2. Bronsted-Lowry Acid B. What does a base do in water? 1. Arrhenius Base 2. Bronsted-Lowry Base C. Conjugate Acid-Base Pairs

IV. Water

A.Water is amphoteric

IV. Water A.Water is amphoteric B.Water experiences self- ionization

IV. Water A.Water is amphoteric B.Water experiences self- ionization C.If there’s water, there’s H 3 O + and OH -

V. pH Scale

pH Scale A way to describe how much acid (H 3 O + ) is in a solution.

A.[H 3 O + ] can vary greatly V. pH Scale

A.[H 3 O + ] can vary greatly B.A neutral solution contains mol/L H 3 O + V. pH Scale K eq = 1.0 x

A.[H 3 O + ] can vary greatly B.A neutral solution contains mol/L H 3 O + C.The pH scale is a logarithmic scale V. pH Scale pH = - log [H 3 O + ]

A.[H 3 O + ] can vary greatly B.A neutral solution contains mol/L H 3 O + C.The pH scale is a logarithmic scale D.Finding [OH - ] V. pH Scale

A.[H 3 O + ] can vary greatly B.A neutral solution contains mol/L H 3 O + C.The pH scale is a logarithmic scale D.Finding [OH - ] E.Calculating pOH V. pH Scale

VI. Strong Acids & Weak Acids

A. Strong Acids

VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate

VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate 2. Are good electrolytes

VI. Strong Acids & Weak Acids A. Strong Acids 1. Completely dissociate 2. Are good electrolytes 3. Equation notation:

HClHBrHI The 7 Strong Acids HNO 3 H 2 SO 4 HClO 3 HClO 4

Self Check – Ex. 1 What is the concentration of H 3 O + ions in a 0.25 M solution of HBr. What is the pH of this solution?

VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

1. Partially dissociate before... VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

1. Partially dissociate before Poor electrolyte VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

1. Partially dissociate before Poor electrolyte 3. Described by: VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

1. Partially dissociate before Poor electrolyte 3. Described by: 4. Finding H 3 O + for weak acids VI. Strong Acids & Weak Acids A. Strong Acids B. Weak Acids

Self Check – Ex. 2 What is the concentration of H 3 O + ions in a 1.0 M solution of HC 2 H 3 O 2 (K a = 1.8 x )

Solving weak acid problems

1.Write equilibrium equation

Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression

Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium)

Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium) 4.Substitute equilibrium values into equilibrium expression.

Solving weak acid problems 1.Write equilibrium equation 2.Write equilibrium expression 3.Make a table of concentrations (before, change, & equilibrium) 4.Substitute equilibrium values into equilibrium expression. 5.Solve

Self Check – Ex. 2 What is the concentration of H 3 O + ions in a 1.0 M solution of HC 2 H 3 O 2 (K a = 1.8 x )

Self Check – Ex. 3 The pH of a M solution of formic acid is What is the K a for HCOOH?