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Acids and BasesAcids and BasesChapter 19Chapter 19Chapter 19Chapter 19
I. Describing Acids & BasesI. Describing Acids & Bases
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
D. Electrical ConductivityD. Electrical Conductivity
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
D. Electrical ConductivityD. Electrical Conductivity
E. IndicatorE. Indicator
IndicatorIndicator
Substance that is one color in an acidic solution and another color in a basic solution
Substance that is one color in an acidic solution and another color in a basic solution
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
D. Electrical ConductivityD. Electrical Conductivity
E. IndicatorE. Indicator1.1. litmuslitmus
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
D. Electrical ConductivityD. Electrical Conductivity
E. IndicatorE. Indicator1.1. litmuslitmus2.2. phenolphthaleinphenolphthalein
I. Describing Acids & BasesI. Describing Acids & BasesA. TasteA. Taste
B. TouchB. Touch
C. Reactions with MetalsC. Reactions with Metals
D. Electrical ConductivityD. Electrical Conductivity
E. IndicatorE. Indicator1.1. litmuslitmus2.2. phenolphthaleinphenolphthalein3.3. bromothymol bluebromothymol blue
II. Defining Acids & BasesII. Defining Acids & Bases
II. Defining Acids & BasesII. Defining Acids & Bases
A. Arrhenius DefinitionA. Arrhenius Definition
II. Defining Acids & BasesII. Defining Acids & Bases
A. Arrhenius DefinitionA. Arrhenius Definition1. Acid1. Acid
Arrhenius AcidArrhenius Acid
A substance that dissociates in water to produce H+ ion
A substance that dissociates in water to produce H+ ion
A. Arrhenius DefinitionA. Arrhenius Definition1. Acid1. Acid
2. Base2. Base
II. Defining Acids & BasesII. Defining Acids & Bases
Arrhenius BaseArrhenius Base
A substance that dissociates in water to form OH- ions
A substance that dissociates in water to form OH- ions
B. Bronsted-Lowry DefinitionB. Bronsted-Lowry Definition
II. Defining Acids & BasesII. Defining Acids & Bases
B. Bronsted-Lowry DefinitionB. Bronsted-Lowry Definition1. Acid1. Acid
II. Defining Acids & BasesII. Defining Acids & Bases
Bronsted-Lowry AcidBronsted-Lowry Acid
A substance that can donate a protonA substance that can donate a proton
B. Bronsted-Lowry DefinitionB. Bronsted-Lowry Definition1. Acid1. Acid
2. Base2. Base
II. Defining Acids & BasesII. Defining Acids & Bases
Bronsted-Lowry BaseBronsted-Lowry Base
A substance that can accept a protonA substance that can accept a proton
B.B. Bronsted-Lowry DefinitionBronsted-Lowry Definition
C.C. Polyprotic AcidsPolyprotic Acids
II. Defining Acids & BasesII. Defining Acids & Bases
Polyprotic AcidsPolyprotic Acids
Those acids that donate more than one protonThose acids that donate more than one proton
III. ReactionsIII. Reactions
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
2. Bronsted-Lowry Acid2. Bronsted-Lowry Acid
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
2. Bronsted-Lowry Acid2. Bronsted-Lowry Acid
B. What does a base do in water?B. What does a base do in water?
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
2. Bronsted-Lowry Acid2. Bronsted-Lowry Acid
B. What does a base do in water?B. What does a base do in water?
1. Arrhenius Base1. Arrhenius Base
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
2. Bronsted-Lowry Acid2. Bronsted-Lowry Acid
B. What does a base do in water?B. What does a base do in water?
1. Arrhenius Base1. Arrhenius Base
2. Bronsted-Lowry Base2. Bronsted-Lowry Base
III. ReactionsIII. ReactionsA. What does an acid do in water?A. What does an acid do in water?
1. Arrhenius Acid1. Arrhenius Acid
2. Bronsted-Lowry Acid2. Bronsted-Lowry Acid
B. What does a base do in water?B. What does a base do in water?
1. Arrhenius Base1. Arrhenius Base
2. Bronsted-Lowry Base2. Bronsted-Lowry Base
C. Conjugate Acid-Base PairsC. Conjugate Acid-Base Pairs
IV. WaterIV. Water
IV. WaterIV. WaterA.A. Water is amphotericWater is amphoteric
IV. WaterIV. WaterA.A. Water is amphotericWater is amphoteric
B.B. Water experiences self-Water experiences self-ionizationionization
IV. WaterIV. WaterA.A. Water is amphotericWater is amphoteric
B.B. Water experiences self-Water experiences self-ionizationionization
C.C. If there’s water, there’s If there’s water, there’s HH33OO++ and OH and OH--
V. pH ScaleV. pH Scale
pH ScalepH Scale
A way to describe how much acid (H3O+) is in a solution.
A way to describe how much acid (H3O+) is in a solution.
A.A. [H[H33OO++] can vary greatly] can vary greatly
V. pH ScaleV. pH Scale
A.A. [H[H33OO++] can vary greatly] can vary greatly
B.B. A neutral solution contains A neutral solution contains 0.0000001 mol/L H0.0000001 mol/L H33OO++
V. pH ScaleV. pH Scale
Keq = 1.0 x 10-14Keq = 1.0 x 10-14
A.A. [H[H33OO++] can vary greatly] can vary greatly
B.B. A neutral solution contains A neutral solution contains 0.0000001 mol/L H0.0000001 mol/L H33OO++
C.C. The pH scale is a The pH scale is a logarithmic scalelogarithmic scale
V. pH ScaleV. pH Scale
pH = - log [H3O+]pH = - log [H3O+]
A.A. [H[H33OO++] can vary greatly] can vary greatly
B.B. A neutral solution contains A neutral solution contains 0.0000001 mol/L H0.0000001 mol/L H33OO++
C.C. The pH scale is a The pH scale is a logarithmic scalelogarithmic scale
D.D. Finding [OHFinding [OH--]]
V. pH ScaleV. pH Scale
A.A. [H[H33OO++] can vary greatly] can vary greatly
B.B. A neutral solution contains A neutral solution contains 0.0000001 mol/L H0.0000001 mol/L H33OO++
C.C. The pH scale is a The pH scale is a logarithmic scalelogarithmic scale
D.D. Finding [OHFinding [OH--]]
E.E. Calculating pOHCalculating pOH
V. pH ScaleV. pH Scale
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak Acids
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA. Strong AcidsA. Strong Acids
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA. Strong AcidsA. Strong Acids
1.1. Completely dissociateCompletely dissociate
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA. Strong AcidsA. Strong Acids
1.1. Completely dissociateCompletely dissociate
2.2. Are good electrolytesAre good electrolytes
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA. Strong AcidsA. Strong Acids
1.1. Completely dissociateCompletely dissociate
2.2. Are good electrolytesAre good electrolytes
3.3. Equation notation: Equation notation:
HClHCl
HBrHBr
HIHI
The 7 Strong AcidsThe 7 Strong Acids
HNOHNO33
HH22SOSO44
HClOHClO33
HClOHClO44
Self Check – Ex. 1Self Check – Ex. 1
What is the concentration What is the concentration of Hof H33OO++ ions in a 0.25 ions in a 0.25 MM
solution of HBr.solution of HBr.
What is the pH of this What is the pH of this solution?solution?
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA.A. Strong AcidsStrong Acids
B.B. Weak AcidsWeak Acids
1.1. Partially dissociate before. . .Partially dissociate before. . .
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA.A. Strong AcidsStrong Acids
B.B. Weak AcidsWeak Acids
1.1. Partially dissociate before. . .Partially dissociate before. . .
2.2. Poor electrolytePoor electrolyte
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA.A. Strong AcidsStrong Acids
B.B. Weak AcidsWeak Acids
1.1. Partially dissociate before. . .Partially dissociate before. . .
2.2. Poor electrolytePoor electrolyte
3.3. Described by:Described by:
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA.A. Strong AcidsStrong Acids
B.B. Weak AcidsWeak Acids
1.1. Partially dissociate before. . .Partially dissociate before. . .
2.2. Poor electrolytePoor electrolyte
3.3. Described by:Described by:
4.4. Finding HFinding H33OO++ for weak acids for weak acids
VI. Strong Acids & Weak AcidsVI. Strong Acids & Weak AcidsA.A. Strong AcidsStrong Acids
B.B. Weak AcidsWeak Acids
Self Check – Ex. 2Self Check – Ex. 2
What is the concentration of What is the concentration of HH33OO++ ions in a 1.0 ions in a 1.0 MM solution solution
of HCof HC22HH33OO22 ( (KKaa = 1.8 x 10 = 1.8 x 10-5-5))
Solving Solving weak acidweak acid problems problems
Solving Solving weak acidweak acid problems problems
1.1. Write equilibrium equationWrite equilibrium equation
Solving Solving weak acidweak acid problems problems
1.1. Write equilibrium equationWrite equilibrium equation
2.2. Write equilibrium expressionWrite equilibrium expression
Solving Solving weak acidweak acid problems problems
1.1. Write equilibrium equationWrite equilibrium equation
2.2. Write equilibrium expressionWrite equilibrium expression
3.3. Make a table of concentrations Make a table of concentrations (before, change, & equilibrium)(before, change, & equilibrium)
Solving Solving weak acidweak acid problems problems
1.1. Write equilibrium equationWrite equilibrium equation
2.2. Write equilibrium expressionWrite equilibrium expression
3.3. Make a table of concentrations Make a table of concentrations (before, change, & equilibrium)(before, change, & equilibrium)
4.4. Substitute equilibrium values Substitute equilibrium values into equilibrium expression.into equilibrium expression.
Solving Solving weak acidweak acid problems problems
1.1. Write equilibrium equationWrite equilibrium equation
2.2. Write equilibrium expressionWrite equilibrium expression
3.3. Make a table of concentrations Make a table of concentrations (before, change, & equilibrium)(before, change, & equilibrium)
4.4. Substitute equilibrium values Substitute equilibrium values into equilibrium expression.into equilibrium expression.
5.5. SolveSolve
Self Check – Ex. 2Self Check – Ex. 2
What is the concentration of What is the concentration of HH33OO++ ions in a 1.0 ions in a 1.0 MM solution solution
of HCof HC22HH33OO22 ( (KKaa = 1.8 x 10 = 1.8 x 10-5-5))
Self Check – Ex. 3Self Check – Ex. 3
The pH of a 0.100 M The pH of a 0.100 M solution of formic acid is solution of formic acid is 2.38. What is the 2.38. What is the KKaa for for
HCOOH?HCOOH?
