Acids and Bases

Acids Bases&

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Definitions

• Acids – produce H+

• Bases - produce OH-

• Acids – donate H+

• Bases – accept H+

• Acids – accept e- pair• Bases – donate e- pair

Arrhenius

Bronsted-Lowry

Lewis

only in water

any solvent

used in organic chemistry,wider range of substances

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Examples

Arrhenius

Bronsted-Lowry

Lewis

HCl NaOH

HCl NH3

:NH3BF3

HCN

The hydrogen ion in aqueous solution

H+ + H2O H3O+ (hydronium ion)

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The Bronsted-Lowry Concept

Conjugate pairs

HCl Cl- CH3COOH CH3COO-

NH4+ NH3 HNO3 NO3-

How does a conjugate pair differ?H+ transfer

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H2O H+ + OH-

Does pure water conduct electrical current?

(H+)(OH-) = 10-14

For pure water: (H+) = (OH-) = 10-7M

This is neutrality and at 25oC is a pH = 7.

Water is a very, very, very weak electrolyte.

How are (H+) and (OH-) related?

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Strong and Weak Acids/Bases

Strong acids/bases – 100% dissociation into ions

HCl NaOHHNO3 KOHH2SO4

Weak acids/bases – partial dissociation, both ions and molecules

CH3COOH NH3

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What is acid rain?

CO2 (g) + H2O H2CO3 H+ + HCO3-

Dissolved carbon dioxide lowers the pH

Atmospheric pollutants from combustion

NO, NO2 + H2O … HNO3

SO2, SO3 + H2O … H2SO4

bothstrong acids

pH < 5.3© iTutor. 2000-2013. All Rights Reserved

General properties

ACIDS

• Taste sour• Turn litmus• React with active

metals – Fe, Zn• React with bases

BASES

• Taste bitter• Turn litmus• Feel soapy or

slippery (react with fats to make soap)

• React with acids

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pH Table

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