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Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

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Lewis acids Brnsted-Lowry Arrhenius acids Ralph A. Burns, Fundamentals of Chemistry 1999, page 483

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- ArrheniusH + H 3 O + OH Brnsted- Lowry (H + ) (H + ) Lewis

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Formula FormulaName of AcidName of Negative Ion of Salt HFhydrofluoricfluoride HBrhydrobromicbromide HIhydroiodiciodide HCl hydrochloricchloride HClOhypochloroushypochlorite HClO 2 chlorouschlorite HClO 3 chloricchlorate HClO 4 perchloricperchlorate H 2 S hydrosulfuricsulfide H 2 SO 3 sulfurous sulfite H 2 SO 4 sulfuricsulfate HNO 2 nitrousnitrite HNO 3 nitricnitrate H 2 CO 3 carboniccarbonate H 3 PO 3 phosphorousphosphite H 3 PO 4 phosphoricphosphate

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Sodium hydroxideNaOHlye or caustic soda Potassium hydroxideKOHlye or caustic potash Magnesium hydroxideMg(OH) 2 milk of magnesia Calcium hydroxideCa(OH) 2 slaked lime Ammonia waterNH 3 H 2 O household ammonia . hydroxide ion OH 1-

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1+ ++ hydronium ion H3O+H3O+ 1- chloride ion Cl - water H2OH2O hydrogen chloride HCl (an Arrhenius acid)

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HCl + H 2 O H 3 O + + Cl H HHHH H Cl OO + acid Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem NH 3 + H 2 O NH 4 + + OH - H H H H H H N NO O + H H H H

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Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 508

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ACID + BASE SALT + WATER HCl + NaOH NaCl + H 2 O HC 2 H 3 O 2 + NaOH NaC 2 H 3 O 2 + H 2 O . pH . ( ) Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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ACID + BASE SALT + WATER HCl + NaOH NaCl + H 2 O HC 2 H 3 O 2 + NaOH NaC 2 H 3 O 2 + H 2 O . pH= 7 . Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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Brnsted-Lowry 1+ + hydronium ion H3O+H3O+ 1- chloride ion Cl - (base) H2OH2O (acid) HCl ++ --

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Brnsted-Lowry (acid) H2OH2O (base) NH 3 ++ -- 1+ + ammonium ion NH 4 + 1- hydroxide ion OH -

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HClhydrochloric acid HNO 3 nitric acid HClO 4 perchloric acid H 2 SO 4 sulfuric acid CH 3 COOHacetic acid H 2 CO 3 carbonic NaOH sodium hydroxide KOH potassium hydroxide Ca(OH) 2 calcium hydroxide NH 3 ammonia Kotz, Purcell, Chemistry & Chemical Reactivity 1991, page 145 NH 4 OH ammonia NH 3 + H 2 O NH 4 OH

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( ) one more oxygen atom most common one less oxygen two less oxygen HClO 4 perchloric acid HClO 3 chloric acid HClO 2 chlorous acid HClO hypochlorous acid H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid H 3 PO 4 phosphoric acid H 3 PO 3 phosphorous acid H 3 PO 2 hypophosphorous acid HNO 3 nitric acid HNO 2 nitrous acid (HNO) 2 hyponitrous acid

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pH Scale Sren Sorensen (1868 - 1939)

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pH Scale Acid Base 0 7 14 Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 515 [H + ] pH 10 -14 14 10 -13 13 10 -12 12 10 -11 11 10 -10 10 10 -9 9 10 -8 8 10 -7 7 10 -6 6 10 -5 5 10 -4 4 10 -3 3 10 -2 2 10 -1 1 10 0 0 1 M NaOH Ammonia (household cleaner) Blood Pure water Milk Vinegar Lemon juice Stomach acid 1 M HCl Acidic Neutral Basic

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pH Timberlake, Chemistry 7 th Edition, page 335 1.0 M HCl 0 gastric juice 1.6 vinegar 2.8 carbonated beverage 3.0 orange 3.5 apple juice 3.8 tomato 4.2 lemon juice 2.2 coffee 5.0 bread 5.5 soil 5.5 potato 5.8 urine 6.0 milk 6.4 water (pure) 7.0 drinking water 7.2 blood 7.4 detergents 8.0 - 9.0 bile 8.0 seawater 8.5 milk of magnesia 10.5 ammonia 11.0 bleach 12.0 1.0 M NaOH (lye) 14.0 8 910 111214 13 34 5 6 2 1 70 acidic neutral basic [H + ] = [OH - ]

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pH = 3 pH = 7 pH = 11 OH - H3O+H3O+ H3O+H3O+ H3O+H3O+ [H 3 O + ] = [OH - ] [H 3 O + ] > [OH - ] [H 3 O + ] < [OH - ] concentration (moles/L) 10 -14 10 -7 10 -1 Timberlake, Chemistry 7 th Edition, page 332

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pH pH = -log [H 1+ ] Kelter, Carr, Scott, Chemistry A World of Choices 1999, page 285

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Acid Base pH = -log [H 1+ ] pH = 7 Acidic Basic Neutral [H + ] [OH - ] [H + ] = [OH - ]

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pH pH pOH [H 3 O + ] [OH - ] pH + pOH = 14 pH = -log[H 3 O + ] [H 3 O + ] = 10 -pH pOH = -log[OH - ] [OH - ] = 10 -pOH [H 3 O + ] [OH - ] = 1 x10 -14

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pH = - log [H + ] pH = 4.6 pH = - log [H + ] 4.6 = - log [H + ] - 4.6 = log [H + ] Given: 2 nd log 10 x antilog multiply both sides by -1 substitute pH value in equation take antilog of both sides determine the [hydronium ion] choose proper equation [H + ] = 2.51x10 -5 M You can check your answer by working backwards. pH = - log [H + ] pH = - log [2.51x10 -5 M] pH = 4.6 Recall, [H + ] = [H 3 O + ]

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HCl + H 2 O H 3 O + + Cl - acidbase acid conjugates HCl + H 2 O H 3 O + + Cl - acid base CA CB

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NH 3 + H 2 O NH 4 1+ + OH - baseacid base conjugates base acid CA CB NH 3 + H 2 O NH 4 1+ + OH -

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! base acid CA CB NH 3 + H 2 O NH 4 1+ + OH - HCl + H 2 O H 3 O + + Cl - acid base CA CB : ..

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1- ++ sulfuric acid H 2 SO 4 water H2OH2O hydrogen sulfate ion HSO 4 - hydronium ion H3O+H3O+ 1+ 1- ++ sulfate ion SO 4 2- water H2OH2O hydrogen sulfate ion HSO 4 - hydroxide ion OH - 1- 2-

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( ) HC 2 H 3 O 2 + H 2 O H 3 O 1+ + C 2 H 3 O 2 - acid 1 base 1 base 2 acid 2 conjugates acid base CA CB HC 2 H 3 O 2 + H 2 O H 3 O 1+ + C 2 H 3 O 2 -

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Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

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pH pH 0 1 2 3 4 5 6 pH 7 8 9 10 11 12 13

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1 2345 6 789101112 Pink - pH phenolphthalein methyl red methyl orange

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Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 520

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COLOR CHANGES AS A FUNCTION OF pH INDICATOR pH 2 3 4 5 6 7 8 9 10 11 12 RED APPLE SKIN BEETS BLUEBERRIES RED CABBAGE CHERRIES GRAPE JUICE RED ONION YELLOW ONION PEACH SKIN PEAR SKIN PLUM SKIN RADISH SKIN RHUBARB SKIN TOMATO TURNIP SKIN * * YELLOW at pH 12 and above

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Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

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Phenolphthalein Colorless = Acidic pH Pink = Basic pH H+H+

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-O-O O C C O O-O- (Colorless acid form, HIn)(Pink base form, In - ) OH HO C C O O-O-