acids and bases. define acids and bases in terms of the three definitions: arrhenius bronsted and...
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ACIDS AND BASES
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· Define acids and bases in terms of the three definitions:· Arrhenius· Bronsted and Lowry· Lewis
· Define Amphoteric
· Identify and label conjugate pairs.
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· Taste sour · Burn when touching skin. · Turn blue litmus red. · Neutralize basic solutions. · Corrosive to metals· strong or weak electrolytes
ACIDS
BASES· Taste bitter · Feel slippery· Turn red litmus blue · Neutralize acidic solutions· strong or weak electrolytes
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Arrhenius Definition
yes, this is really him...looks happy, eh?
Svante Arrhenius (1859 - 1927)
Acids – Compounds that yield hydrogen ions (H+) in aqueous solution.
Bases – Compounds that yield OH- ions in aqueous solution.
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HCl (aq) → H+ (aq) + Cl–
(aq)
NaOH (aq) → Na+ (aq) + OH–
(aq)
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The Bronsted-Lowry Theory
20 years later:
An acid is a proton (H+) donor.
A base is a proton (H+) acceptor.
Lowry
Bronsted
NH3base~ no OH– ?
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Ammonia accepts a proton from water:
NH3 (g) + H2O(l) NH4+
(aq) + OH-(aq)
H+
acceptor
Base is a proton (H+) acceptor:
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Result is the H3O+ ion called the hydronium ion.H+ and H3O+ are written interchangeably.
HCl (g) + H2O(l) H3O+(aq) + Cl-
(aq)
H+
acceptordonor
NH3 (g) + HCl(g) NH4+
(g) + Cl-(g)
H+
Acids is a proton (H+) donor:
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A substance which can act as either an acid or a base is described as being amphoteric.
Water is amphoteric.Bicarbonate ion is also amphoteric.
HCO3- + OH- CO3
2- + H2OH+
acceptordonor
HCO3-
+ H2O H2CO3 + OH-
H+
acceptor donor
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Acids and bases accept and donate electrons, NOT protons.
Lewis acids accept (keep) electrons. Lewis bases donate (lose) electrons.
Gilbert Lewis Definition
CH3COO-(aq) + H2O(l) OH-
(aq) + CH3COOH (aq)
H+
base acid
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Transition metal ions with charges of 2+ or 3+, create an acidic solution with water.
Step 1: Formation of a hydrate.
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Step 2: Loss of H+ making acidic solution.
Fe(H2O)63+ + H2O H3O
+ + Fe(H2O)5(OH)2+ H+
H
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Conjugate acid is what remains after a base has accepted a proton.
Conjugate base is what remains after the acid has donated its proton.
NH3 (g) + H2O(l)
base acid
NH4+
(aq) + OH-(aq)
Con. baseCon. acid
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B + H2Obase acid
BH+ + OH-
Con. baseCon. acid
Each is called a conjugate pair.
HA + H2Obaseacid
H3O+ + A-
Con. baseCon. acid
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· Arrhenius defined acids as substances which release H+ ions in water and bases as substances which release OH¯ ions in water.
· Bronsted and Lowry defined acids as proton donors and bases as proton acceptors.
· Substances that behave as BOTH acids and bases, these are called amphoteric.
· An acid and its conjugate base or a base and its conjugate acid are known as conjugate pairs.
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CAN YOU / HAVE YOU? · Define acids and bases in terms of the three
definitions:· Arrhenius· Bronsted and Lowry· Lewis
· Define Amphoteric
· Identify and label conjugate pairs.