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Lecture 7

CHEM 1A03 Lecture Notes - Lecture 7: Hydronium, Chief Operating Officer, Quadratic Equation


Department
Chemistry
Course Code
CHEM 1A03
Professor
David Brock
Lecture
7

This preview shows pages 1-3. to view the full 10 pages of the document.

Introduction
-autoionization
-equilibrium 
 
-amphoteric = !
-"#

 
 
o$%& $&$'()
Importance of Acid-Base Chemistry
-*
-+,-.
-*
Qualitative Acid-Base Tests
- Acidic = /!0
- Alkaline = /0
Arrhenius Theory
- Late 19th 
-11
!
o23$4&5
- Acids = 367
- Bases = 3 +6#
- Acid-base reaction = 38 

-9, 
-.!,excludes species /:52650
Bronsted-Lowry Theory
- Acid = 6#
- Base = 6#
-;!!acid and base as reactants
conjugate acid and conjugate base products
Relative Strength of Acid-Base Conjugates

Only pages 1-3 are available for preview. Some parts have been intentionally blurred.

-towards weaker conjugate
acid and base
-<,!

-;!=>stronger acid, weaker
conjugate base
Lewis Theory
-?electrons (Bronsted-Lowryprotons)
- Acids = 
- Bases = 
-*88!
Strong Acids and Bases
- Strong acids =  
o> very 1/
0
o;8Ka >> 1
o;
o+@

Only pages 1-3 are available for preview. Some parts have been intentionally blurred.

5
HCl, HBr, HI
+AH2SO4, HNO3, HClO4
- Strong bases
oGroup I and group II hydroxides
-+ #> 
ooxides, O2
oHydrides, with H-6#1
oB 
o>very 1#
Weak Acid and Bases
- Does not 3
- reverse reaction,  equilibrium
constant
-* 3"
"
o-<< 1
- pKa pKb!
- “p” – “negative log”
- Smaller pKa, stronger the acid
- Smaller pKb, stronger the base
- Anything NOT a strong acid or base = a weak acid or base
Other Ways to Identify
--= weakly acidic carboxylic acid
oEx. Ibuprofen, !!/pKa 4.4)
Carbonic acid =  /pKa1 6.4, pKa2
10.2)
Pyruvic acid /0#/pKa 2.5)
-C1#centered around nitrogen
oEx. Ammonia (pKb = 4.74)
oMethylamine (pKb = 3.36)
oDiethylamine (pKb = 3.16)
- Nitrogen = =
Module II
Weak Acids and Ka
- Acid base equilibria with a weak acid and water
-17D65+77>1
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