chapter 19 open textbook to page 586. many substances contain acids. vinegar (acetic acid)...
TRANSCRIPT
![Page 1: CHAPTER 19 Open Textbook to page 586. MANY SUBSTANCES CONTAIN ACIDS. VINEGAR (ACETIC ACID) CARBONATED DRINKS (PHOSPHORIC ACID) GRAPE JUICE (TARTARIC ACID)](https://reader034.vdocuments.mx/reader034/viewer/2022051014/5514ef65550346b0478b5dbd/html5/thumbnails/1.jpg)
CHAPTER 19
Open Textbook to page 586
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MANY SUBSTANCES CONTAIN ACIDS.
•VINEGAR (ACETIC ACID)•CARBONATED DRINKS (PHOSPHORIC ACID)•GRAPE JUICE (TARTARIC ACID)•APPLES (MALIC ACID)•LEMONS (CITRIC ACID)
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MANY SUBSTANCES CONTAIN BASES.
•LYE (SODIUM HYDROXIDE) FOUND IN COMMERCIAL DRAIN CLEANERS
•MILK OF MAGNESIA (MAGNESIUM HYDROXIDE)
•BAKING SODA (SODIUM BICARBONATE)
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ACIDS:
5 GENERAL PROPERTIES:
1)HAVE A SOUR TASTE.
2) CHANGE THE COLOR OF ACID-BASE INDICATORS.
3)REACT WITH ACTIVE METALS TO RELEASE H2 (g).
Mg (s) + 2 HCl (aq) MgCl2 + H2 (g)
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4) REACT WITH BASES TO PRODUCE SALTS AND WATER.
5) SOME ACIDS CONDUCT ELECTRIC CURRENT.
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ACID NOMENCLATURE
BINARY ACID: ACID THAT CONTAINS ONLY
2 DIFFERENT ELEMENTS,
i.e.,
HYDROGEN AND ONE OF THE MORE ELECTRONEGATIVE ELEMENTS.
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NAMES OF BINARY ACIDS
• HF HYDROFLUORIC ACID
• HCl HYDROCHLORIC ACID
• HBr HYDROBROMIC ACID
• HI HYDROIODIC ACID
• H2S HYDROSULFURIC ACID
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OXYACIDSACID THAT IS A COMPOUND OF
HYDROGEN,
OXYGEN, AND
a 3rd ELEMENT USUALLY A NONMETAL
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COMMON OXYACIDS
• CH3COOH Acetic acid• H2CO3 Carbonic acid• HNO3 Nitric acid• H3PO4 phosphoric acid• H2SO4 sulfuric acid• H2SO3 sulfurous acid• HClO4 perchloric acid• HClO3 chloric acid• HClO2 chlorous acid• HClO hypochlorous acid
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Common Industrial Acids
• SULFURIC ACID:MOST COMMONLY PRODUCED INDUSTRIAL CHEMICAL
USED IN CAR BATTERIES
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2)NITRIC ACID:
• STAINS PROTEINS YELLOW
• USED IN MAKING EXPLOSIVES
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3)PHOSPHORIC ACID:
• USED DIRECTLY FOR MANUFACTURINGFERTILIZERS AND ANIMAL FEED.
• FLAVORING AGENT IN SOFT DRINKS
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4)HYDROCHLORIC ACID:
• PRODUCED BY STOMACH
• IN HARDWARE STORES, DILUTE SOL’N KNOWNAS MURIATIC ACID AND IS USED TO CORRECT
ACIDITY OF SWIMMING POOLS AND TO CLEAN MASONRY.
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BASES5 GENERAL PROPERTIES
• TASTE BITTER.
• CHANGE THE COLOR OF ACID-BASE INDICATORS.
• DILUTE AQUEOUS SOLUTIONS FEEL SLIPPERY.
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BASES5 GENERAL PROPERTIES
• REACT WITH ACIDS TO PRODUCE SALTS AND WATER.
• CONDUCT ELECTRIC CURRENT.
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Svante Arrhenius Theory limitedto aqueoussolutions
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ARRENHIUS ACIDS & BASES
• ARRENHIUS ACID:
INCREASES THE CONC.
OF HYDROGEN IONS, H+, IN AQUEOUS SOLUTIONS
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ARRENHIUS ACIDS & BASES
• ARRENHIUS BASE:
INCREASES THE CONCENTRATION
OF HYDROXIDE IONS, OH-, IN AQUEOUS SOLUTIONS
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AQUEOUS SOLUTIONS OF BASES
• ALKALINE• IONIC HYDROXIDES WHICH
DISSOCIATE IN SOLUTION TO RELEASE OH- (aq).
• SODIUM HYDROXIDE: NaOHNaOH (s) Na+ (aq) + OH- (aq)
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Group 1 HydroxidesNaOHKOHLiOHRbOHCsOH
Group 2 HydroxidesCa(OH)2
Ba(OH)2
Sr(OH)2
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AnotherACID-BASE THEORIES
• ARRENHIUS DEFINITION REQUIRES SUBSTANCES TO BE AQUEOUS.
• DEFINITIONS REVISED TO INCLUDE SUBSTANCES WHEN THEY ARE NOT IN A WATER SOLUTION.
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BRONSTED-LOWRY ACIDS & BASES
• BRONSTED-LOWRY ACID:
A MOLECULE or ION THAT IS A
PROTON DONOR.
• HCl + NH3 NH4+ + Cl-
• HCl transfers a proton to the ammonia molecule
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Figure 14.3The Reaction of NH3 with HCl to Form
NH4+ and Cl-
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BRONSTED-LOWRY BASE
• MOLECULE OR ION THAT IS A PROTON ACCEPTOR.
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The Reaction of NH3 with HCl to Form NH4
+ and Cl-
AMMONIA ACCEPTS A PROTON FROM HCl thus AMMONIA IS A BRONSTED-LOWRY BASE
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BONSTED-LOWRY ACID-BASE REACTION
• PROTONS ARE TRANSFERRED FROM ONE REACTANT (THE ACID)
TO ANOTHER (THE BASE).
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ACID-BASE REACTIONS• BRONSTED-LOWRY ACID DONATES A
H+
• SPECIES REMAINING COULD RE-ACCEPT THAT H+ AND THUS ACT AS A BASE
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CONJUGATE BASE
• SPECIES THAT REMAINS AFTER A BRONSTED-LOWRY ACID HAS GIVEN UP A H+ ION.
• HF (aq) + H2O (l) F- (aq) + H3O+ (aq)
acid conjugate
base
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• BRONSTED-LOWRY BASE ACCEPTS A H+
• SPECIES REMAINING COULD RE-DONATE THAT H+ AND THUS ACT AS AN ACID
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CONJUGATE ACID
• SPECIES THAT FORMS AFTER A BRONSTED-LOWRY BASE HAS ACCEPTED A H+ ION.
• HF (aq) + H2O (l) F- (aq) + H3O+ (aq)
base conjugate
acid
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BRONSTED-LOWRY ACID-BASE REACTIONSAre equilibrium systems meaning that both theForward and the reverse reactions occur.
Each contain two conjugate acid-base pairs.
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Let’s identify the Conjugate Acid-Base Pairs
HNO3 (l) + H2O (l) H3O+ (aq) + NO3- (aq)
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Conjugate Acid/Base Pairs
•HA(aq) + H2O(l) H3O+(aq) + A(aq) conj conj conj conj
acid 1 base 2 acid 2 base 1
DO PROBLEM 48 on page 625
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AMPHOTERIC COMPOUNDS
• SPECIES THAT CAN ACT AS EITHER AN ACID OR A BASE
H2SO4(aq) + H2O H3O+(aq) + HSO4- (aq)
base
NH3 (g) + H2O (l) NH4+(aq) + OH- (aq)
acid
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Water as an Acid and a Base
•Water is amphoteric (it can behave either as an acid or a base).
• H2O (l) + H2O(l) H3O+ + OH
• conj conj– acid 1 base 2 acid 2 base 1
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MONOPROTIC ACIDS
• ACIDS THAT CAN DONATE ONLY ONE HYDROGEN ION PER MOLECULE.
• EXAMPLES
HCl
HNO3
HClO4
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Polyprotic Acids
• . . . can furnish more than one Hydrogen ion (H+) to the solution.
• Examples:
• H2SO4
• H3PO4
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All polyprotic acids ionize in a stepwiseManner i.e., one HYDROGEN ION at a time.
H2SO4 (l) + H2O (l) H3O+ (aq) + HSO4- (aq)
HSO4- (aq) + H2O (l) H3O+ (aq) + SO4
2- (aq)
Each step is weaker than the one before; therefore, concentration of ions formed in the first step is the greatest.
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POLYPROTIC ACIDS
• DIPROTIC ACID:
CAN DONATE TWO HYDROGEN IONS PER MOLECULES.
• TRIPROTIC ACID:
CAN DONATE THREE
HYDROGEN IONS
PER MOLECULE
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Lewis Acids and BasesEmphasizes role of electron pairs to form a
covalent bond
• Lewis Acid: electron pair acceptor
• Lewis Base: electron pair donor
Al3+ + 6H
OH
Al OH
H6
3+
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The Al(H2O)63+ ion
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Aluminum ion (Lewis Acid) accepts electron pairs From Water (Lewis Base) donates electron pairsto form covalent bonds.
Lewis Acid-Base Reaction:
formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor.
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LEWIS DEFINITION BROADEST OF THETHREE ACID-BASE DEFINITIONS
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STRONG ACIDS
• ACID THAT IONIZES COMPLETELY IN AQUEOUS SOLUTION.
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STRONG ACID Solutions
HClO4 (aq)
H2SO4 (aq)
HNO3 (aq)HCl (aq)HBr (aq)HI (aq)
MEMORIZE!!!
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WEAK ACIDS
• ACID THAT IONIZES LESS THAN COMPLETELY IN AQUEOUS SOLUTION.
• . Ka is the acid dissociation constant.• Smaller the Ka the weaker the acid.
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Figure 14.4Graphic Representation of the Behavior of Acids of Different Strengths in Aqueous Solution
a) Strong Acid
b) Weak Acid
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Figure 14.6
A Strong Acid (a) and a Weak Acid (b) in Water
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Bases•“Strong” and “weak” are used in the same sense for bases as for acids.
•strong = complete dissociation (hydroxide ion supplied to solution)
•NaOH(s) Na+(aq) + OH(aq)
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Strong Bases (Strong electrolytes)
Group 1A HydroxidesNaOHKOHLiOHRbOHCsOH
Group 2A HydroxidesCa(OH)2
Ba(OH)2
Sr(OH)2
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WEAK BASES (Weak electrolytes): Weak = incomplete dissociation
Kb is the base dissociation constant.Smaller the Kb the weaker the base.
NH3 ammoniaCH3NH2 methylamine
Other organic compounds that containnitrogen atoms.