| ACID
IONIZATION EQUILIBRIA |
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Acid
ionization constant – Ka |
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Definition
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Derivation
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Determining
the degree of ionization |
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Electrical conductivity or
colligative properties |
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Measurement
of pH |
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Calculations involving Ka |
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Approximation
method |
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Procedure
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Example
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Quadratic
formula |
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Procedure
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Example
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Calculating
Ka using pH |
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Procedure
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Example
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Calculating
percent ionization for a weak acid |
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Definition
of percent ionization |
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Procedure |
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Examples
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Given initial
concentration and pH |
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Given initial
concentration and Ka |
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Calculations
involving polyprotic acids |
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Sequential
ionization of polyprotic acids |
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Some
polyprotic acids and their Ka’s |
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Patterns
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Procedure
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Example
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| BASE
IONIZATION EQUILIBRIA |
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Base ionization constant – Kb |
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Definition
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Derivation
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Calculations
involving Kb |
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Approximation
method |
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Using the
quadratic formula |
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Example |
| RELATIONSHIP
BETWEEN THE IONIZATION CONSTANTS OF ACIDS AND THEIR CONJUGATE BASES |
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Relative
strengths of acids and bases |
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The
stronger the acid, the weaker the conjugate base |
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The
stronger the base, the weaker the conjugate acid |
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Acid-base
reactions proceed in the direction of the weaker acid and weaker base |
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Examples
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The
mathematical relationship between Ka and Kb |
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Relationship derived |
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Calculating
Kb for the conjugate base of an acid |
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Procedure
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Example
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| MOLECULAR
STRUCTURE AND ACID STRENGTH |
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Two
factors affect the extent to which an acid ionizes |
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Bond
strength |
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Bond
polarity |
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Binary acids |
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Effect of bond strength |
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Effect
of bond polarity |
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Oxyacids |
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Effect
of increasing electronegativity of the central atom |
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Effect
of increasing number of O atoms |
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Polyprotic
acids and their corresponding acid anions |
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Effect
of increasing charge on the acid particle |
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Example
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| ACID
- BASE PROPERTIES OF SALT SOLUTIONS |
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Salt
hydrolysis |
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Definition
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Description
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Examples
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Ions
and hydrolysis |
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Ions
that do not undergo
hydrolysis |
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Ions
that do undergo hydrolysis |
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Predicting
whether a salt solution will be acidic, basic, or neutral |
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Rules of
thumb |
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Examples
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Calculating
the pH of salt solutions |
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Procedure
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Examples
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| THE
COMMON ION EFFECT |
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Definitions
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Descriptions
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Qualitative
models of the common ion effect |
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A
solution of a weak acid HA |
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A
solution of a weak base B |
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Calculations
involving the common ion effect |
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Procedure
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Example
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| BUFFERS |
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Definition |
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Important role of buffers |
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Description |
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Making buffer solutions |
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By
direct addition |
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Forming
the salt in solution |
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How a
buffer works |
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Identifying
solutions that are buffers and those that are not |
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Two
important characteristics of buffers |
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The pH
of the initial buffer solution |
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Buffering
capacity |
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The
derivation of the Henderson-Hasselbalch equation |
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Calculations
involving buffers |
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Calculating
the pH of the initial buffer solution |
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Calculating
the pH of a buffer solution after the addition
of acid or base to that
solution |
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Making a
buffer solution of a specified pH |
| ACID-BASE
TITRATION CURVES |
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Acid-base
titration |
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Definition
of acid-base titration |
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Equivalence
point |
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End
point |
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Indicators
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Three types of titration curves |
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Titration
of a strong acid by a strong base |
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Titration
of a weak acid by a strong base |
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Titration of a weak base by a strong acid |
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pH
calculations and titrations |
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Procedure |
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Examples
involving the titration of a strong acid by a strong base |
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Examples
involving the titration of a weak acid by a strong base |