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Hydrochloric Acid, HCl

The stomach produces HCl to aid in the digestion of food.

Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

BaseBitter tasteTurns red litmus blueSlippery to the touch

IONS

Acid + Base SaltSalt + Water

HCl + NaOH NaCl + HOH salt water

Neutralization Reaction

Properties

electrolytes

turn litmus red

sour taste

react with metals to form H2 gas

slippery feel

turn litmus blue

bitter taste

ChemASAP

vinegar, milk, soda, apples, citrus fruits

ammonia, lye, antacid, baking soda

electrolytes

Common Bases

Sodium hydroxide NaOH lye or caustic soda

Potassium hydroxide KOH lye or caustic potash

Magnesium hydroxide Mg(OH)2 milk of magnesia

Calcium hydroxide Ca(OH) 2 slaked lime

Ammonia water NH3 H2O household ammonia

Name Formula Common Name

.NH4OH

NH41+ + OH1-

ammonium hydroxide

hydroxideion

OH1-

AcidSour tasteTurns blue litmus redReacts with some metals to produce H2

Dissolves carbonate salts, releasing CO2

Common Acids and Bases

Strong Acids (strong electrolytes)

HCl hydrochloric acidHNO3 nitric acidHClO4 perchloric acidH2SO4 sulfuric acid

Weak Acids (weak electrolytes)

CH3COOH acetic acidH2CO3 carbonic

Strong Bases (strong electrolytes)

NaOH sodium hydroxideKOH potassium hydroxideCa(OH)2 calcium hydroxide

Weak Base (weak electrolyte)

NH3 ammonia

Kotz, Purcell, Chemistry & Chemical Reactivity 1991, page 145

NH3 + H2O NH4OH

Indicators

Compounds that show a color change in an acid or base.

• Most indicators are weak organic acids or bases that react with ions in solution. It is this chemical reaction that produces the color change.

Red Cabbage IndicatorCopyright © 2007 Pearson Benjamin Cummings. All rights reserved.

pH of Common Substance

14 1 x 10-14 1 x 10-0 0 13 1 x 10-13 1 x 10-1 1 12 1 x 10-12 1 x 10-2 2 11 1 x 10-11 1 x 10-3 3 10 1 x 10-10 1 x 10-4 4 9 1 x 10-9 1 x 10-5 5 8 1 x 10-8 1 x 10-6 6

6 1 x 10-6 1 x 10-8 8 5 1 x 10-5 1 x 10-9 9 4 1 x 10-4 1 x 10-10 10 3 1 x 10-3 1 x 10-11 11 2 1 x 10-2 1 x 10-12 12 1 1 x 10-1 1 x 10-13 13 0 1 x 100 1 x 10-14 14

NaOH, 0.1 MHousehold bleachHousehold ammonia

Lime waterMilk of magnesia

Borax

Baking sodaEgg white, seawaterHuman blood, tearsMilkSalivaRain

Black coffeeBananaTomatoesWineCola, vinegarLemon juice

Gastric juice

Mor

e ba

sic

Mor

e ac

idic

pH [H1+] [OH1-] pOH

7 1 x 10-7 1 x 10-7 7

ELECTROLYTES

• Conduct electricity

• Strong acids and bases

TUMMY ACHE

Ca(OH)2

or

Mg(OH)2

Another name for household Vinegar

HC2H3O2 Acetic Acid

pH of Common Substances

Timberlake, Chemistry 7th Edition, page 335

1.0 MHCl0

gastricjuice1.6

vinegar2.8

carbonated beverage3.0

orange3.5

apple juice3.8

tomato4.2

lemonjuice2.2 coffee

5.0

bread5.5

soil5.5

potato5.8

urine6.0

milk6.4

water (pure)7.0

drinking water7.2

blood7.4

detergents8.0 - 9.0

bile8.0

seawater8.5

milk of magnesia10.5

ammonia11.0

bleach12.0

1.0 MNaOH(lye)14.0

8 9 10 11 12 14133 4 5 621 70

acidic neutral basic[H+] = [OH-]

ACIDS

a) Remember that H+ reacts with H2O to produce H3O+

ex. HNO3 + H2O H3O+ + NO3-

b) strong acids – one that completely ionizes in aqueous solution

ex. HCl and HNO3

c) weak acids –are weak electrolytes (ionize only little)

ex. HC2H3O2

BASES

b) strong bases – strong electrolytes; completely dissociates

ex. NaOH, KOH c) weak bases – not very soluble in water so they don’t give off many OH- ions

ex. Mg(OH)2 and NH3 (ammonia)

NH3 + H2O NH4+ + OH-

pH Paper

pH 0 1 2 3 4 5 6

pH 7 8 9 10 11 12 13