Acids and Bases
• Arrhenius Definitions:
– When reacting with water,
• Acids release hydrogen ions (ex: HNO3)
• Bases release hydroxide ions (ex: NaOH)
• Salts are ionic compounds that release neither
hydrogen ions nor hydroxide ions
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Expanded Definitions
• Bronsted-Lowery Definition:
– Acids donate hydrogen ions
– Bases receive hydrogen ions
– Ampherteric: serves as both an acid and a
base
• Lewis Definition:
– Acids receive electron pairs
– Bases donate electron pairs
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Operational Definitions
• Acids:
– Sour taste
– React with metals to produce hydrogen gas
– Electrolytes
– Turn acid – base indicators different
colors
– React with bases to produce salt and water
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Operational Definition
• Bases:
– Bitter taste
– Slippery
– Electrolytes
– Turn acid – base indicators different
colors
– React with acids to produce salt and water
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Naming Bases and Salts
• To name bases and salts follow the
standard rules for naming ionic
compounds.
• NaOH
– Sodium hydroxide
• CaCl2
– Calcium chloride
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Naming Acids
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Binary Acid
Only two elements
First element is hydrogen
Named - - hydro _____ic acid
HCl
– Hydrochloric acid
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Naming Acids
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Ternary Acids
Three elements
First element is hydrogen
Other elements are part of a polyatomic ion
Naming does not require a prefix
ATE  IC
ITE  OUS
H2SO4
– Sulfuric acid
• H2SO3
– Sulfurous acid
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Examples
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H3PO4
Phosphoric acid
HF
Hydrofluoric acid
HClO2
Chlorous acid
• Name the
following acids:
• HBr
• HNO3
• HNO2
• HI
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