1. The document discusses acid-base theories including Arrhenius, Brønsted-Lowry, and Lewis concepts of acids and bases. 2. Key aspects covered are the definition of acids and bases as proton donors and acceptors, autoionization of water, and acid dissociation constants. 3. Common examples are given of acids and bases in different theories including ammonia acting as a Brønsted-Lowry base and boron trifluoride acting as a Lewis acid.

1. Acid Base in Everyday Life)
H2
Arrhenius Concept
H H+ H
3O +
OH OH -
NH 3
Bronsted-Lowry Concept

2. proton donor)
proton acceptor)
NH 3(aq) + H 2O (1) NH 4 + (aq) + OH - (aq)
base 2 ........ acid 1 ........ acid 2 ........ base 1
NH 3 H 2O
NH 3 H 2O NH 4 +
OH - NH 4 + OH -
Lewis Concept
electron pair
acceptor)
electron pair
donor)
concept Arrhenius
Bronsted-Lowry
OH - (aq) + CO 2 (aq) HCO 3 - (aq)

3. BF 3 + NH 3 BF 3-NH 3
–
– H+ 1
H+ 1
=
CH 3COOH (aq) + H 2O (aq) CH 3COO - (aq) + H 3O +
(aq)
<<<
>>>
1. CH 3COOH H 3O + /
H 2O CH 3COO -
2. H 3O + CH 3COOH /
CH 3COO - H 2O
K>1
K<1
K=1
2

4. 1. 1.
2. Hydro = HCl HBr HI 2. 1 = LiOH NaOH KOH
3. Oxy = HNO3 HClO3 RbOH CsOH
HClO4 H2SO4 3. 2 = Ca(OH)2 Sr(OH)2
4. 100% Ba(OH)2
5. 4. 100 % ( 2
200 %)
5.
strong acid) 100%
HCl H2SO4 HN03 HBr HClO4 HI
weak base) 100%
Hydroxide 1 2 ( NaOH LiOH CsOH Ba(OH) 2
Ca(OH) 2 )
weak
acid)
vinegar) acetylsalicylic
acid) saccharin
niacin (nicotinic acid)
CH 3COOH
CH 3COOH (aq) + H2O (1) H3O + (aq) + CH3COO - (aq)
Ka

5. weak
base) NH 3
urea aniline ammonia
NH3(aq) + H2O (aq) NH4 + (aq) + OH - (aq)
3
1. Monoprotic 1 HNO 3 , HClO 3 , HClO 4 ,
HCN
2. Diprotic 2 H 2SO 4 , H 2CO 3
3. Polyprotic 3 H 3PO 4
Polyprotic H+
Ka
Ka H+
H 2SO 4 H+ + HSO 4 - Ka 1 = 10 11
HSO 4 - H+ + SO 4 2- Ka 2 = 1.2 x 10 -2
Polyprotic K 1 >> K 2 >> K 3 H +
K1 K 2 =10 3 pH
Polyprotic K1 K2
K2

6. OH - 3
1. OH - LiOH NaOH KOH RbOH CsOH
2. OH - 2 Ca(OH) 2 Sr(OH) 2 Ba(OH) 2
3. OH - 3 Al(OH) 3 Fe(OH) 3
1. K Ka = [H +] Kb = [ OH -]
2 /N 2 /N
2. H +] [H +] = [ OH -] =
[Ka.N]^1/2 [Kb.N]^1/2
3. % %
H +] x OH -] x
100 / N 100 / N
% = Ka x % = Kb x
4. K 100 / N 100 / N
4
o

7. o -------
o
o
pH
nonelectrolyte)
self-ionization
autoprotolysis
H 2O (1) + H 2O (1) H 3O + (aq) + OH -(aq)
.... acid 1 .....base 2 .............acid 2 ........base 1
2H 2O (1) = H 3O + (aq) + OH - (aq)
Kw
K w = [H 3O +][ OH -] = 1.0 x 10 -14 25 C
(K w 0 C = 0.12 x 10 -14 60 C = 9.6 x 10 - 14 M2)
pK w = pH + pOH
pH log [H 30 +] = 7 pOH -log[ OH
-] = 7

8. pH
1-14 pH
14
pH 6.5 pH
pH HCl 1.0 x
10 - 8 M
HCl H + 1.0 x 10 - 8 M
H+ 1.0 x 10 - 7 M
H+ 1.0 x 10 -8 + 1.0 x 10 - 7 M
pH = -log (1.0 x 10 -8 + 1.0 x 10 -7 )
= 6.96
Buffer Solution)
pH
pH

9. pH 0.10 M NH 3
0.20 M NH 4Cl Kb NH 3 1.8x10 -5 25 oC
M) NH 3(aq) + H 2O (1) NH 4 + (aq) + OH -
(aq)
........................................................ ................ 0.10 .........
..............................0.20 ............0
........................................................ .......... -
x ..........................................+x ..............+x
........................................................ .................. 0.10-
x ..................................0.20+x .......x
Kb=
1.8 x 10 -5 =
0.20 + x ~ 0.20 0.10 - x ~ 0.10

10. = 1.8 x 10 -5
.............................................................. x = [ OH - ] = 1.8x10 -5
x = 9.0 x 10 -5
............................................................ pH = 14.00 - pOH =
14.00 + log[ OH - ]
.............................14.00 + log (9.0 x 10 -5) = 14.00 - 5.05 =
8.95
NH 3 + H + = NH 4 +
NH 4 ++ OH -= NH 3+H 2O
pH 4.30
1 HS0 4 - / SO 4 2- Ka = 1.2 x 10 -2
2 HOAc / OAc - Ka = 1.8 x 10 -5
3 HCN / CN - Ka = 4.0 x 10 -10
pH = 4.30 [H +] = 5.0 X 10 - 5 M
HOAc / OAc - Ka H +] = 5.0 X
10 - 5 M
.............. acid + H 2O = H 3O + + conjugate base

11. H + = 5.0 X 10 –5 Ka = 1.8 x 10 -5 HOAc] / [OAc
- ] = 2.8
pH
HIn
HIn (aq) + H 2O (l) H 3O + (aq) + In - (aq)
Ka = [H 3O +][ In - ] / [ HIn]
pH
HIn (aq) + H 2O (l) H 3O + (aq) + In - (aq)
..............................................................................
H 3O +

12. OH - , OH - H 3O +
pH
pH pH = -log K Hin + 1
---
–
( : Acid-Base Theory)
definition)

13. Arrhenius) Brønsted-Lowry acid)
Lewis)
Hard-Soft Acids-Bases: HSAB)
Fahjan's Rules)
Svante Arrhenius)
2427 H+)
H3O+) OH−)
HCl (aq) → H+ (aq) + Cl− (aq)
NaOH (aq) → Na+ (aq) + OH− (aq)
(Auto-dissociation)

14. ------ H3O+)
OH−)
H+)
H3O+)
H2O(l) + H2O(l) ⇌ H3O+(aq) + OH−(aq)
AlCl3 NH3 N(CH3)3
(Neutralization)
H+)
OH−)
H+(aq) + OH−(aq) → H2O (l)
Svante Arrhenius)

15. (Johannes Nicolaus Brønsted)
(Thomas Martin Lowry)
2466 (Proton Transferring)
AH)
Proton Donor) B)
Proton Acceptor)
AH + B ⇌ A− + BH+
(CH3COOH)
CH3COOH (aq)) + H2O (l) ⇌ CH3COO− (aq)) + H3O+ (aq)
Thomas
Martin Lowry)
Johannes
Nicolaus
Brønsted Base) H+)
Brønsted)
---
Brønsted Acid)

16. CH3COO−)
H+)
H3O+)
--- conjugate
acid–base pair) CH3COOH)
conjugate acid) CH3COO−)
CH3COO−) conjugate base)
H2O )
H3O+)
H O+ + NH ⇌ H O + NH
Fe(H O) H O ⇌ [Fe(H O) OH] H O+
H SO H O ⇌ HSO H O+
CH COOH + NH → NH CH COO−
NH H O ⇌ H O+ + NH
H O+(aq) + Cl−(aq) + NH g) → Cl−(aq) + NH aq)

17. HCl(benzene) + NH benzene) → NH Cl(s)
HCl(g) + NH g) → NH Cl(s)
Amphoteric)
AH + B ⇌ A− + BH+
HNO3 + H2O ⇌ NO3− + H3O+
(
H2O + NH=C(NH2)2 ⇌ OH− + H2N=C(NH2)2+
(

18. H+ + OH− ⇌ H2O
NH4+ + NH2− ⇌ 2NH3
H3SO4++HSO4−⇌ H2SO4
Autoionization
Process) protic solvent)
H2O ⇌ H+ + OH−
2NH3 ⇌ NH4+ + NH2−
H2SO4 ⇌ H3SO4++HSO4−
Autoprotolysis
Constant: KAP) Ionic Product)
KAP KW
1.0 × 10−14 25℃: KAP = KW = [H+][OH−] = 1.0 ×
10−14 25℃

19. pKAP H2SO4 2.9 25℃
pKAP NH3 27.7 50℃
pKAP
pKw
0 5 10 15 20 25 30 35 40
℃)
pKw 14.943 14.734 14.535 14.346 14.167 13.997 13.830 13.680 13.53
[ pKAP = −logKAP pKW = −log (1.0 ×
10−14) = 14.0 25℃]
Acid Dissociation Constant: Ka)
HA ⇌ A− + H+

20. pKa 25℃
pKa HA) conjugate acid, HB) B)
− + MeCN) DMSO)
HA ⇌ A + H
-
8.5 0.9
2,4- 16.66 5.1 3.9
21.51 11.1 4.2
23.51 12.6 4.756
29.14 18.0 9.99
+ +
BH ⇌ B + H
19.56 10.8 11.4
18.82 9.0 10.72
12.53 3.4 5.2
10.62 3.6 4.6

21. ---
BF3 Me3N:
Gilbert Newton Lewis)
Electron Pair)
Electron Pair
Acceptor)" Electron Pair
Donor)"
Me N: + BF → Me N: + BF
Me N: Lewis Base)
BF BF Lewis
Acid) Me N:
Adduct)
Complex)
BF F− → BF
BF OMe → BF OMe Gilbert
I I− → I Newton Lewis)

22. SiF F− → SiF

23. " acid
indicator) H3O
2
1. 2
3
2. pH

24. pH 8.3-10.0
pH 4.2-6.2
pH 6.0-7.6

25. pH 6.8-8.4
pH
3.1-4.4
4.2-6.3
5.0-8.0
6.0-7.6
6.8-8.4
8.3-10.0
1)
pH 4.2-6.3

26. pH 4.2
pH 4.2-6.3
(
pH 6.3
----------------------
2)
pH 8.3- 10.0
pH 8.3-10.0
X
pH X
X pH 10

27. pH
1-3
3-4 -
6-7 -
6-7 -
8-9 -
9-10 -
10-11 -
pH
pH pH " pH meter
pH
pH

28. https://sites.google.com/site/acidsbase/krd-bes/smbati-khxng-
sarlalay-krd-bes
http://www.thaigoodview.com/library/contest2551/science03/07/
acidbase00.html
http://www.trueplookpanya.com/true/knowledge_detail.php?mul
_content_id=2225
http://th.wikipedia.org
http://nakhamwit.ac.th/pingpong_web/Acid&Base.htm