acids, bases & salts n acid properties : n sour taste, react with metals to produce hydrogen...
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Acids, Bases & Salts Acids, Bases & Salts Acid Properties:
Sour taste, react with metals to produce hydrogen gas,
electrolytes, affect indicators (turns blue litmus paper to
red)
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Acids, Bases & Salts Acids, Bases & Salts Base Properties: Bitter taste, produce
electrolytes, affect indicators (turns red litmus
paper to blue)
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Acids Acids Electrolytes: substances
that conduct electric current when dissolved in
water.
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Acids Acids Indicators: chemical substances that change
color based on acid concentration.
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Acids Acids Arrhenius Theory: acids
produce H+ ions when dissolved (ionized) in
water.
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Acids Acids Arrhenius Theory: bases
produce OH- ions when dissolved (ionized) in
water.
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Acids Acids Dissociation vs. ionization: dissociation is the separation
of ions in solution. In ionization, neutral molecules react with water to form ions.
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Acids Acids Bronsted-Lowry Theory:
acids donate protons (H+) in a chemical reaction.
Ex. HCl(g) + H2O(l) --> H3O+(aq) + Cl-(aq)
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Acids Acids The HCl gas donates a
proton to the water molecule, producing the hydronium ion. HCl is considered an
acid, water is considered a base.
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Acids Acids Bronsted-Lowry Theory: bases accept protons (H+) in
a chemical reaction.HCl and Cl- are considered
a conjugate acid/base pair.
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Acids Acids Conjugate acid/base pairs:
Conjugate base - the particle leftover after the
acid donates a proton.
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Acids Acids Conjugate acid/base pairs:
Conjugate acid - the particle produced after the
base accepts the proton.
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Acids Acids Identify the acid, base,
conjugate base and conjugate acid in the following:
HNO3(aq) + NaOH(aq) --> H2O(l) + NaNO3(aq).
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Acids Acids Practice problems #1-2, p.
576.What do you want to
know?
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Acids Acids Lewis Theory: an acid is any
substance that accepts an electron pair. A base is any substance that donates an
electron pair. NH3 + BF3 --> NH3BF3
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Acids Acids Use electron dot diagrams to determine if a substance
is a Lewis acid or base.Ex. Classify Cl- as a Lewis
acid or base.
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Acids Acids Coordination complexes:
molecular ligands (attachments) approach a
metal cation and bond using secondary (d-orbital)
valance.
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Acids Acids Complex ion formation: ex.
Ag+ + NH3 --> ? (coordination number of 2).
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Acids Acids What is the name of
[CoCl2(NH3)5]Br
Practice Problems #3-8, p. 578. Any questions?
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Acid Nomenclature Acid Nomenclature Binary acids: acids
consisting of 2 elements.Ex. HCl
HIHBr
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Acid Nomenclature Acid Nomenclature Ternary Acids and Bases:
acids or bases containing three elements.
Common ternary acid - formed by using H+ and a common polyatomic ion.
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Acid Nomenclature Acid Nomenclature Use the polyatomic name and
the suffix -ic. Ex. H2SO4
HNO3
HClO3
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Acid Nomenclature Acid Nomenclature A ternary acid that is the same as the common acid but with one less oxygen uses the suffix -ous.
Ex. H2SO3
HClO2
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Acid Nomenclature Acid Nomenclature A ternary acid that is the same as the common acid but with two less oxygens uses the prefix -hypo and the suffix -
ous. Ex. HClO
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Acid Nomenclature Acid Nomenclature A ternary acid that is the same as the common acid but with one more oxygen uses the prefix -per and the suffix -ic.
Ex. HClO4
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Acid Nomenclature Acid Nomenclature Common ternary base - formed by using metal and the hydroxide polyatomic
ion.Ex. NaOH, Mg(OH)2
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Acid Nomenclature Acid Nomenclature Organic acids: carboxylic
acids, -COOHName the chain and add -
oic acid.
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Acid Nomenclature Acid Nomenclature Practice Problems #9-13, p.
580Wha?
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Acid/Base Behavior Acid/Base Behavior Consider a compound in the
form HOX. If X is very electronegative then the H is given up as a proton and it acts as an acid. If not it acts
as a base.
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Acid/Base Behavior Acid/Base Behavior So, nonmetals tend to form
acids, metals tend to form bases when dissolved in water.
Ex. MgO CO
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Acid/Base Behavior Acid/Base Behavior Acidic and Basic Anhydrides:
acids and bases that have had water removed.
Ex. Acid anhydride + water --> acid
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Acid/Base Behavior Acid/Base Behavior Ex. Acid anhydride + water
--> acidSO2 + H2O --> H2SO3
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Acid/Base Behavior Acid/Base Behavior Ex. basic anhydride +
water --> baseNa2O + H2O --> 2 NaOH
Practice problems #14-15 p. 583
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Acid/Base Behavior Acid/Base Behavior Acid base strength: not all acids complete ionize in water.
That is a lot of the acid or base molecules remain
unreacted. Ex. Ammonia (weak base)
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Acid/Base Behavior Acid/Base Behavior Concept review #16-19 p.
584
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Salts and Solutions Salts and Solutions Salt : an ionic compound that
does not consist of H+ or OH-
Ex. KCl, MgO (any ionic compound that is not an Arrehnius acid or base)
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Neutralization Neutralization Neutralization reaction: a
acid reacts with a base to produce a salt and water.
Really just a double displacement reaction
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Neutralization Neutralization Ex. Produce the products
and balance the equation for the reaction of the acid HCl and the base AgOH.
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Neutralization Neutralization Naming salts - who cares?
Ex. Sodium hydrogen carbonate
Ex. Sodium dihydrogen phosphate
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Net Ionic EquationsNet Ionic EquationsSome ions in a
neutralization reaction are considered spectator ions.
That is, they are unchanged after the reaction.
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Net Ionic EquationsNet Ionic EquationsChemists often write net
ionic equations to show only those ions that actually take place in the reaction.
Ex. HCl + NaOH
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Net Ionic EquationsNet Ionic EquationsPolyprotic acids - go
through two steps of ionization
Ex. Sulfuric acid
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Net Ionic EquationsNet Ionic Equations The binary acids HCl, HBr,
and HI are strong acids, the rest are weak.
Ternary acids with 2 or more oxygens versus hydrogens are
strong.
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Net Ionic EquationsNet Ionic Equations Organic acids are weak.
Polyprotic acids: second step always results in a weak acid Group 1 and 2 bases are
strong.
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Net Ionic EquationsNet Ionic Equations Molecules and weak acids and
bases are not written in ionic form.
Salts are written in ionic form, oxides and gases are written
as molecules.
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Net Ionic EquationsNet Ionic EquationsPractice problems #23-27
p. 590. (in groups - 15 minutes)
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Ionization ConstantIonization ConstantThe Keq for the ionization
of a weak acid or base determines the extent that
[H3O+] or [OH-] ions will be produced at equilibrium.
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Ionization ConstantIonization ConstantKa is the ionization
constant of a weak acid. HX + H2O <--> H3O+ + X-.
What is Ka for this reaction?
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Ionization ConstantIonization Constant Kb is the ionization constant of
a weak base. NH3 + H2O <--> NH4
+ + OH-.
What is Kb for this reaction?
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Ionization ConstantIonization ConstantPercent ionization =
[amount ionized] / [original acid] x 100%
Problems 28-31, p. 592-593
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Ionization ConstantIonization ConstantCommon Ion Effect - adding
ions that are the same as one of those produced by the
ionization of a weak electrolyte …. (more)
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Ionization ConstantIonization Constant to a solution of the
electrolyte suppresses its ionization. Why???
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Ionization ConstantIonization ConstantLe Chatelier’s Principle -
you are increasing the concentration of products.
The system responds to reestablish equilibrium.
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Ionization ConstantIonization ConstantProblems 42-65 p. 597-598.