AGENDA
• WE ARE GOING TO LEARN
• PROPERTIES OF ACIDS AND BASES
• ACID AND BASE NOMENCLATURE
• WHAT IS AN ACID AND WHAT IS A BASE?
• WHAT IS ANOTHER WAY OF CLASSIFYING AN ACID AND A BASE?
• WHAT IS YET ANOTHER WAY OF CLASSIFYING AS AN ACID AND A BASE?
• WHAT IS pH, pOH AND HOW DO WE CALCULATE THEM?
• WHAT IS [H+] AND [OH-] ALL ABOUT AND HOW DO WE CALCULATE THEM?
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PROPERTIES OF ACIDS
• AQUEOUS SOLUTIONS OF ACIDS HAVE A SOUR TASTE.
• DON’T TRY THIS YOURSELF
•
OBVIOUSLY
• ACIDS CHANGE THE COLOR OF ACID-BASE INDICATORS
• SOME ACIDS REACT WITH ACTIVE METALS TO FORM H2 GAS
• ACIDS REACT WITH BASES TO FORM WATER AND A SALT.
• A SALT – NOT ONLY TABLE SALT NaCl.
Could be KI or Na2SO4
• ACIDS CONDUCT ELECTRIC CURRENT
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PROPERTIES OF BASES
• AQUEOUS SOLUTIONS OF BASES TASTE BITTER.
• NO – DON’T TASTE THEM
• BASES CHANGE THE COLOR OF ACID BASE INDICATORS
• DILUTE AQUEOUS SOLUTIONS OF BASES ARE SLIPPERY
• BASES REACT WITH ACIDS TO PRODUCE WATER AND A SALT
• BASES CONDUCT ELECTRIC CURRENT
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NOMENCLATURE FOR BINARY
ACIDS
• A BINARY ACID CONTAINS HYDROGEN AND 1 OTHER ELEMENT
(THAT IS ELECTRONEGATIVE) I.E. HCl, HI, HBr, H2S
• BINARY ACIDS ARE NAMED BY HYDRO- PREFIX AND –IC SUFFIX
• HYDROCHLORIC ACID, HYDROBROMIC ACID, HYDROSULFURIC ACID
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NOMENCLATURE FOR OXYACIDS
• AN OXYACID IS AN ACID THAT CONTAINS HYDROGEN, OXYGEN,
AND ONE OTHER ELEMENT
• THE FORMULA FOR THESE IS WRITTEN AS HYDROGEN PLUS A
POLYATOMIC ION.
• NOTE – THE HYDROGEN IS BONDED TO THE OXYGEN
• SEE NEXT PAGE
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H2SO4
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NOMENCLATURE FOR OXYACIDS
• SEE NOTES HANDOUT FOR CHART OF NAMES
• OXYACIDS = H+ PLUS OXYANION. (THE NEGATIVE SIDE)
• NOMENCLATURE RULES FOR OXYANIONS.
• 1.
• 2.
SINCE ALL HAVE H+ YOU DON’T NEED TO MENTION IT.
THE ACID NAME STEMS FROM THE OXYANION OR THE CENTRAL
ELEMENT.
• 3. IF THE POLYATOMIC ION ENDED IN –ate, THEN CHANGE TO –ic
• 4. IF THE POLYATOMIC ION ENDED IN –ite, THEN CHANGE IT TO -ous
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OXYACIDS NOMENCLATURE
EXAMPLES
• H2SO4
• SULFATE ION
• ATE  IC
• SULFURIC ACID
• HNO2
• NITRITE ION
• -ITE  -OUS
• NITROUS ACID
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MOST COMMON ACIDS
•
•
•
•
•
SULFURIC ACID H2SO4
•
PETROLEUM REFINERY, METALLURGY, FERTILIZERS
NITRIC ACID HNO3
•
EXPLOSIVES, FERTILIZER
PHOSPHORIC ACID H3PO4
•
FERTILIZERS AND ANIMAL FEED
HYDROCHLORIC ACID (AKA MURIATIC ACID) HCL
•
IRON AND STEEL PRODUCTION, CLEANING, POOLS
ACETIC ACID CH3COOH
•
•
PLASTICS, FOOD SUPPLEMENTS, FUNGICIDE
VINEGAR IS 4% OR 8% ACETIC ACID
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CLASSIFYING AS ACIDS
• THERE ARE 3 DIFFERENT METHODS OF CLASSIFYING
COMPOUNDS AS ACIDS
• WE WILL LEARN 2 OF THEM.
• SOME COMPOUNDS ARE ACIDS ACCORDING TO ONE
DEFINITION BUT NOT ACCORDING TO OTHER(S)
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ARRHENIUS ACIDS AND BASES
• SINCE ACIDS AND BASES CONDUCT ELECTRIC CURRENT, MR.
ARRHENIUS THEORIZED THAT ACIDS PRODUCT IONS IN WATER.
• DEFINITION:
AN ARRHENIUS ACID IS A CHEMICAL COMPOUND THAT
INCREASES THE CONCENTRATION OF HYDROGEN IONS (H+) IN
AQUEOUS SOLUTION
• DEFINITION:
AN ARRHENIUS BASE IS A CHEMICAL COMPOUND THAT
INCREASES THE CONCENTRATION OF HYDROXIDE IONS (OH-) IN
AQUEOUS SOLUTION.
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BUT FIRST – THE HYDRONIUM ION
• H+ IS TOO REACTIVE TO STAY ALONE FOR TOO LONG
• AND THERE’S ALL THIS WATER AROUND, SO…
• H+ + H2O  H3O+
• YOU MAY SEE ACID/BASE REACTIONS WRITTEN BOTH WAYS
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ARRHENIUS ACIDS AND BASES
• HNO3 (l)+ H2O (l)  H3O+ (aq) + NO3- (aq)
• HCl (g) + H2O (l)  H3O+ (aq) + Cl- (aq)
• NaOH (s) ----------------- > Na+ (aq) + OH- (aq)
HO
• KOH (s) ----------------- > K+ (aq) + OH- (aq)
H2O
2
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STRENGTH OF ACIDS AND BASES
• A STRONG ACID IONIZES COMPLETELY IN AQUEOUS SOLUTION
• HCl, H2SO4
• A WEAK ACID RELEASES FEW HYDROGEN IONS IN AQUEOUS
SOLUTION
• CH3COOH, H3PO4
• A WEAK BASE RELEASES FEW HYDROXIDE (OH-) IONS…
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BRØNSTEAD-LOWRY ACIDS AND
BASES
• A BRØNSTEAD-LOWRY ACID IS A MOLECULE OR ION THAT IS A
PROTON DONOR.
• A BRØNSTEAD-LOWRY BASE IS A MOLECULE OR ION THAT IS A
PROTON ACCEPTOR.
• ALL ARRHENIUS ACIDS ARE ALSO BRØNSTEAD-LOWRY ACIDS,
BUT NOT VICE VERSA.
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BRØNSTEAD-LOWRY EXAMPLE
• HCl + NH3  NH4+ + Cl-
• SEE HOW HCl TRANSFERS A PROTON TO NH+?
• HCl IS B-L ACID, NH3 IS B-L BASE.
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STUPID DETAIL FOR PEDANTS
• JUST IN CASE ITS ON THE FINAL OR YOU’RE EVER ON
JEOPARDY
• TECHNICALLY SPEAKING, NaOH IS NOT A BRØNSTEAD-LOWRY
BASE, HOWEVER, IT DISSOLVES IN WATER TO CREATE OHIONS, WHICH ARE BRØNSTEAD-LOWRY BASES.
• SO YEAH, NaOH IS PRETTY MUCH A B-L BASE UNLESS YOU
WANT TO GET REALLY SPECIFIC.
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MORE (OBVIOUS) DEFINITIONS
• MONOPROTIC ACID – AN ACID THAT CAN ONLY DONATE 1
PROTON.
• HCl
• POLYPROTIC ACID – AN ACID THAT CAN DONATE MORE THAN 1
PROTON.
• H2SO4,
• H3PO4
AKA A DIPROTIC ACID
AKA A TRIPROTIC ACID
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NOTICE
• ARRHENIUS AND BRØNSTEAD-LOWRY ACIDS RELY ON
HYDROGEN BEING TRANSFERRED.
• IT IS THE PROTON BEING TRANSFERRED IN BRØNSTEAD-LOWRY, AND IT
CREATES THE HYDRONIUM ION WHICH DEFINES ARRHENIUS ACIDS.
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ACID-BASE REACTIONS
• MOVING FORWARD FROM BRØNSTEAD-LOWRY, SINCE THE
ACID GIVES UP THE PROTON, WHAT REMAINS IS ABLE TO
ACCEPT A PROTON, SO IT IS A BASE.
• THE SPECIES THAT IS LEFT AFTER A B-L ACID DONATES A PROTON IS
KNOWN AS THE CONJUGATE BASE OF THAT ACID.
• HF(aq)
+ H2O(l)
acid
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
F- (aq) + H3O+(aq)
conjugate base
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ACID-BASE REACTIONS
• THIS APPLIES TO BASES AS WELL.
A BASE THAT ACCEPTS A
PROTON IS NOW ABLE TO DONATE THAT PROTON PER ACIDS.
• THE SPECIES THAT IS LEFT AFTER A B-L BASE ACCEPTS A PROTON IS
KNOWN AS THE CONJUGATE ACID OF THAT BASE.
• HF(aq)
+ H2O(l)
base
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
F- (aq) + H3O+(aq)
conjugate acid
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ACID/BASE AND CONJUGATES
• THE STRONGER THE ACID, THE WEAKER ITS CONJUGATE BASE
WILL BE. (AND VICE VERSA)
• THE STRONGER THE BASE, THE WEAKER ITS CONJUGATE ACID.
(AND VICE VERSA)
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ACID BASE REACTIONS
• PROTON-TRANSFER REACTIONS FAVOR THE CREATION OF WEAKER ACIDS
AND WEAKER BASES.
• HClO4 (aq) + H2O(l)
Stronger acid
Stronger base
• CH3COOH(aq) + H2O(l)
Weaker acid
Weaker base
ClO4- (aq) + H3O+(aq)
Weaker base
Weaker acid
CH3COO- (aq) + H3O+(aq)
Stronger base
Stronger acid
• THE STRONGER ACID WILL “WIN THE BATTLE” IN DONATING PROTONS.
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WHAT MAKES AN ACID STRONG?
• THE STRENGTH OF AN ACID IS DUE TO HOW MUCH IT IONIZES.
• HOW MANY H+ DOES IT PRODUCE TO CREATE H3O+?
• STRONG ACIDS IONIZE 100%.
• WEAKER ACIDS, LESS THAN 100%
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AMPHOTERIC COMPOUNDS
• AMPHOTERIC COMPOUNDS CAN ACT AS EITHER AN ACID OR A
BASE
• WATER IS AMPHOTERIC
H2SO4 (aq) +
NH3 (g) +
H2O(l)
base
H2O(l)
HSO4 - (aq) + H3O+(aq)
NH4+ (aq) + OH-(aq)
acid
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POLYPROTIC ACIDS FORM
AMPHOTERIC COMPOUNDS
• START WITH PHOSPHORIC ACID, H3PO4.
• CREATES H2PO4-
WHICH CAN FORM EITHER
• HPO42- OR REVERT BACK TO H3PO4
• HPO42- CAN FORM PO43- OR REVERT BACK TO H2PO4-
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NEUTRALIZATION REACTIONS
• A STRONG ACID AND STRONG BASE NEUTRALIZE EACH OTHER
TO FORM WATER AND A SALT.
• A SALT, NOT THE SALT, NaCl
• ACID + BASE  WATER + SALT
• A SALT IS AN IONIC COMPOUND MADE FROM CATION FROM THE BASE
AND ANION FROM THE ACID.
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NEUTRALIZATION REACTIONS
NEUTRALIZATION IS THE REACTION OF HYDRONIUM IONS AND
HYDROXIDE IONS TO FORM WATER.
HCl (aq) +
H2O(l)
NaOH


Cl- (aq) + H3O+(aq)
Na+ (aq) + OH- (aq)
THEREFORE
Cl- (aq) + H3O+(aq) + Na+ (aq) + OH- (aq)  H2O(l) + NaCl (aq)
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YOU MAY HAVE HEARD OF ACID
RAIN…
• SO2 IS PRODUCED FROM BURNING OIL OR COAL
• SO2 REACTS WITH AIR TO FORM SO3
• ADD RAINCLOUD…
• SO3 (g) + H20 (l)  H2SO4 (aq)
• Due to regulations in 1990, acid rain has been reduced, but not
eliminated.
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