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![Page 1: Acids & Bases. Naming Review Binary Acids 1.Start the acid name with “hydro-“ 2.Add the root of the second element with the suffix “ic” 3.Add the word.](https://reader035.fdocuments.in/reader035/viewer/2022062304/56649ec45503460f94bcf246/html5/thumbnails/1.jpg)
Acids & BasesAcids & Bases
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Naming ReviewNaming Review
Binary Acids1. Start the acid name with “hydro-“2. Add the root of the second element with the suffix “ic”3. Add the word “acid” EX. HCl- hydrochloric acid
Polyatomic Acids• Use the root name of the polyatomic• Add “ic” if the polyatomic ends in –ate What I ATE was ICky• Add “ous” if the polyatomic ends in –ite I took a bITE it was deliciOUS• Add the word “acid”
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DefinitionsDefinitions
AcidsAcids• Ionize to form hydronium ions (H3O+) in water
(Arrhenius)• Proton donor (Bronsted-Lowry)• Electron-pair acceptor (Lewis)
HCl + H2O H3O+ + Cl–
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DefinitionsDefinitions
BasesBases• Dissociate or ionize to form hydroxide ions (OH-) in water (Arrhenius)• Proton acceptor (Bronsted - Lowry)• Electron-pair donor (Lewis)
NH3 + H2O NH4+ + OH-
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Acid-Base ReactionsAcid-Base Reactions
Conjugate Base – the species that remains Conjugate Base – the species that remains after the acid has given up a protonafter the acid has given up a proton
Conjugate Acid – the species that is formed when the base gains a proton
HCl + H2O H3O+ + Cl-acid conjugate
baseconjugate acid
base
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HF + H2O F- + H3O+
Acid
Base
Conjugate Acid
Conjugate Base
HF
H2O
H3O+
F-
Acid-Base ReactionsAcid-Base Reactions
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PropertiesProperties
sour taste
corrosive
electrolytes
turn litmus red
react with metals to form H2 gas
bitter taste
corrosive
electrolytes
turn litmus blue
slippery feel
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UsesUses
H3PO4 - soft drinks, fertilizer, detergents
H2SO4 - fertilizer, car batteries
HCl - gastric juice
HC2H3O2 - vinegar
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UsesUses
NaOH - lye, drain and oven cleaner
Mg(OH)2 - laxative, antacid
NH3 - cleaners, fertilizer
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Strong vs. WeakStrong vs. Weak
Strong Acid/BaseStrong Acid/Base• 100% ions in water – completely dissociate• strong electrolyte
Weak Acid/BaseWeak Acid/Base• few ions in water –
incomplete dissociation• weak electrolyte
- +
- +
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Strong AcidsStrong Acids
H2SO4 Sulfuric Acid
HClO4 Perchloric Acid
HCl Hyrochloric AcidHNO3 Nitric Acid
HBr Hydrobromic AcidHI Hydroidic Acid
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Strong BasesStrong Bases
Ca(OH)2 Calcium hydroxide
Sr(OH)2 Strontium hydroxide
Ba(OH)2 Barium hydroxide
NaOH Sodium hydroxideKOH Potassium hydroxideRbOH Rubidium hydroxideCsOH Cesium hydroxide
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pH ScalepH Scale
0
7INCREASING
ACIDITY NEUTRALINCREASING
BASICITY
14
pHpH• a measure of the concentration of
H3O+ ions in solution• measured with a pH meter or an
indicator with a wide color range
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pH ScalepH Scale
pH of Common SubstancespH of Common SubstancespH of Common SubstancespH of Common Substances
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Which of the following "molecular" pictures best represents a concentrated solution of the weak acid HA?
ConcepTestConcepTest
A B
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ACID + BASE ACID + BASE SALT + WATER SALT + WATER
HCl + NaOH HCl + NaOH NaCl + H NaCl + H22OO
Neutralization does not always mean pH = 7.
=
Neutralization ReactionNeutralization Reaction
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KOH + HNO3 H2O + KNO3
Acid?
Base?
Salt?
HNO3
KOH
KNO3
Neutralization ReactionNeutralization Reaction
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IndicatorsIndicators
IndicatorIndicator• Substance that changes color in an acid or base• Acid-base indicators are very weak acids and bases that change
color when they:– accept a proton from acid – donate one to a base
Indicator Color of acid Color of base
Litmus paper Red Blue
Phenolphthalein Colorless Pink
Goldenrod Yellow Red
Bromothymol blue Yellow Blue
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TitrationTitration
The controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of solution of unknown concentration
Equivalence Point – the point at which two solutions used in a titration are present in chemically equivalent amounts• Occurs at a pH that is halfway between the two curves
End Point – the point at which an indicator changes color
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TitrationTitration
Beaker – vinegar + phenolphthaleinBuret – sodium hydroxide
As soon the liquid in the beaker
changes color, stop the dropping. Notice the amount
of titrating solution used
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Titration CurvesTitration Curves
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Titration CurvesTitration Curves
strong acid / strong base weak acid / strong base
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H2O: Acid or Base?H2O: Acid or Base?
Amphoteric – a species that can react as either an acid or a base
NH3 + H2O NH4+ + OH-
HCl + H2O H3O+ + Cl– acid base
base acid
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Self-Ionization of H2OSelf-Ionization of H2O
Two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
H2O + H2O <----> H3O + OH⁺ ⁻ At 25 C – the concentrations of H3O + OH in pure water are 1.0x10⁺ ⁻ -7M [ H3O ] = 1.0x10⁺ -7M [ OH ] = 1.0x10⁻ -7M Ionization constant of water is Kw
Kw = [ H3O ] [ OH ]⁺ ⁻
Kw = [ H3O ] [ OH ] = (1.0x10⁺ ⁻ -7M)(1.0x10-7M) = 1.0x10-14M2
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Ionization ProblemsIonization Problems
A 1x10-4M solution of HNO3 has been prepared for a lab experiment.
a. Calculate [ H3O ] ⁺
b. Calculate [ OH ]⁻
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pH & ConcentrationpH & Concentration
pH of a solution is the negative of the common logarithm of the hydronium ion concentration
pH = -log [ H3O ] ⁺
neutral solution at 25C [ H3O ] = 1.0x10⁺ -7MpH = -log (1.0x10-7) = -(-7) = 7
pOH = -log (1.0x10-7) = -(-7) = 7
pH + pOH = 14
Kw= [ H3O ] [ OH ] =1.0x10⁺ ⁻ -14M2
-log(1.0x10-14) = 14
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pH & Conc. CalculationspH & Conc. Calculations
1. What is the pH of a 1x10-3M NaOH solution?
2. What is the pH of a solution if the [ H3O ] ⁺is 3.4x10-5M?
3. Determine the hydronium ion of an aqueous solution that has a pH of 4.0
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pH & Conc. CalculationspH & Conc. Calculations
4. The pH of a solution is measured and determined to be 7.52
a. What is the hydronium ion concentration?
b. What is the hydroxide ion concentration?
c. Is the solution acidic or basic?