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Use your book (pg 459-468) Use your book (pg 459-468)
Make three flaps on page 144•Arrhenius Arrhenius •Brønsted-LowryBrønsted-Lowry• Lewis
How do they define acids and bases?Give an example of eachUse diagrams for representation
I. Introduction toAcids & Bases
Ch. 15 & 16 - Acids & BasesCh. 15 & 16 - Acids & Bases
A. PropertiesA. Properties
electrolytes 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
B. DefinitionsB. Definitions
ArrheniusArrhenius - In aqueous solution… - In aqueous solution…
HCl + H2O H3O+ + Cl– •AcidsAcids form hydronium ions (H3O+)
H
HH H H
H
ClClO O
–+
acid
B. DefinitionsB. Definitions
ArrheniusArrhenius - In aqueous solution… - In aqueous solution…
•BasesBases form hydroxide ions (OH-)
NH3 + H2O NH4+ + OH-
H
H
HH H
H
N NO O–+
H
H
H H
base
B. DefinitionsB. Definitions
Brønsted-LowryBrønsted-Lowry
HCl + H2O Cl– + H3O+
•AcidsAcids are proton (H+) donors.
•BasesBases are proton (H+) acceptors.
conjugate acidconjugate base
baseacid
B. DefinitionsB. Definitions
H2O + HNO3 H3O+ + NO3–
CBCAAB
B. DefinitionsB. Definitions
Amphoteric - can be an acid or a base. - can be an acid or a base.
NH3 + H2O NH4+ + OH-
CA CBB A
B. DefinitionsB. Definitions
F -
H2PO4-
H2O
HF
H3PO4
H3O+
Give the conjugate base for each of the following:
Polyprotic - an acid with more than one H - an acid with more than one H++
B. DefinitionsB. Definitions
Br -
HSO4-
CO32-
HBr
H2SO4
HCO3-
Give the conjugate acid for each of the following:
B. DefinitionsB. Definitions
LewisLewis•AcidsAcids are electron pair acceptors.
•BasesBases are electron pair donors.
Lewis base
Lewis acid
C. StrengthC. Strength
Strong Acid/BaseStrong Acid/Base• 100% ionized in water• strong electrolyte
- +
HCl
HNO3
H2SO4
HBr
HI
HClO4
NaOH
KOH
Ca(OH)2
Ba(OH)2
C. StrengthC. Strength
Weak Acid/BaseWeak Acid/Base• does not ionize completely• weak electrolyte
- +
HF
CH3COOH
H3PO4
H2CO3
HCN
NH3