1. ACIDS & BASES

2. 1.What is a NEUTRAL solution? 2. PROPERTIES OF ACIDIC SOLUTIONS
1. Sour taste
a. Give several examples:
Vinegar, orange juice, lemons
2. Change color of indicators.
a. Acids turn litmus __________.
b. Acids turn phenolphthalein ______________.
3. React with active metals to release _________________.
4. Neutralize bases.
5. Are ELECTROLYTES.
Neither acidic nor basic properties
red
colorless
Hydrogen
Zn + 2 HCl  H2 + ZnCl2
HCl(g)  H+(aq) + Cl-(aq)

3. PROPERTIES OF BASIC SOLUTIONS
These properties are due to the ________________ ion
(or ________ ).
a. This ion is sometimes written as hydrated, with the formula
____________ and is called the ____________________ ion.
PROPERTIES OF BASIC SOLUTIONS
1. Slippery
a. This is noticeable in ___________________________________.
2. Change color of indicators.
a. Bases turn litmus _____________ .
b. Bases turn phenolphthalein ___________________.
3. Neutralize acids. React with solutions containing Mg2+ to form ppt
(Antacids – Rolaids)
4. Are ELECTROLYTES.
NaOH(s)  Na+(aq) + OH-(aq)
Hydrogen H+
H3O+
Hydronium
Detergents, Lye (NaOH)
Blue
pink

4. 5. Have a BITTER taste.
These properties are due to the _____________ ion.
Ex. NaOH, KOH, Ba(OH)2
WRITE THE EQUATION THAT SHOWS THAT WATER IS SLIGHTLY IONIZED.
H2O(l)  H+(aq) + OH-(aq)
The equilibrium constant for that reaction is
Kw = [H+] x [OH-] [ ] = mol/L
This product is equal to ___________________.
In PURE water, there are _____________
numbers of H+ and OH- ions.
Therefore, [H+] = [OH-] or [H+]2 = 1 x 10-14
AND [H+] = 1 X 10 -7
HYDROXIDE
1 x
EQUAL

5. In ACIDIC water, there are ____________ numbers of H+ than OH- ions.
If [H+] = 1 x 10-5 M, then [OH-] = _____________M
(Remember: [H+] x [OH-] = 1 x 10-14)
How does the [H+] compare to [OH-]?
In a BASIC solution, there are ____________ OH- ions than H+ ions.
GREATER
1 x 10-9
1 x 10-5____ =
1 x 10-9
104 of 10,000 x greater
more

6. pH 1. pH is defined mathematically: pH = - log [H+]
2. If [H+] = M, then pH = ____________.
3. In pure water, which is NEUTRAL, [H+] = 1 x 10-7 M
and pH = _________
4. If pH of a solution is 8, then [H+] = _____________.
AND, since [H+] x [OH-] = 1 x 10-14, [OH-] = __________.
5. Acidic solutions have a pH __________________.
6. Neutral solutions have a pH __________________.
7. Basic solutions have a pH ___________________. 1 7
1 x M
1 x M
Less than 7
Equal to 7
Greater than 7

7. pH scale
acidic
neutral
basic
STRONGLY
ACIDIC
STRONGLY
BASIC

8. 1.If [H+] = 2.30 x 10-6 M, the pH = ____________.
pH = - log 2.30 x 10-6
pH = 5.638
2. If [H+] = M, then pH = _________.
pH = - log .0370
pH = 1.432
3. If pH = 10.30, then [H+] = _________.
[H+] = 10-pH
[H+] =
[H+] = 5.0 x M
4. If [OH-] = x 10-3, find [H+] and pH.
[OH-] x [H+] = 1 x 10-14
[H+] = 1 x =
3.70 x 10-3
[H+] = x M

9. pH = - log x 10-12
pH =

10. STRONG ACID vs WEAK ACID

12. ACID (Arrhenius): Substance which releases H+ (H3O+) ions in water
STRONG ACIDS WEAK ACIDS
1.Completely ionize in dilute
solution
HCl(g)  H+(aq) + Cl-(aq)
EX. HCl, HNO3, H2SO4,
HI, HClO4 (Top, Table)
2. Many ions in solution –
Strong electrolytes
3. Ka: Very large
M HCl
[H+] = .01 M = 1 x10-2 M
pH = 2.0
Exception: H2SO4 .
1. Incomplete ionization in water
HF(g)  H+(aq) + F-(aq)
EX. HF, H2CO3, CH3COOH
2. Few ions in solution -
Weak electrolytes
3. Ka: Small number
The smaller the Ka, the weaker
the acid

13. IONIZATION CONSTANT OF WEAK ACIDS : Ka
5. Given: M HNO2, 10.%
ionized. Find [H+] and pH.
[H+] = .10(.30) = .030 M
pH = -log .030 =
1.52
IONIZATION CONSTANT OF WEAK ACIDS : Ka
For the acid HF, HF  H+(aq) + F-(aq)
Ka = [H+] x [F-]
[HF]
[ ] = mol/L

14. 1a. Show the ionizations of: HNO2, CH3COOH (or HCH3OO) in water b
1a. Show the ionizations of: HNO2, CH3COOH (or HCH3OO) in water b. Then, write the Ka expressions for each of those in 1a.

15. 2. The value of the Ka is a measure of the extent to which a weak acid ionizes in water.
Smaller Ka – Fewer H+ ions, weaker acid
Larger Ka – More H+ ions, stronger acid
Ka PROBLEMS
1. When mole of a weak acid is added to 1.00L of water,
moles of H+ is formed. Calculate the Ka of the acid.

16. 2. The Ka of benzoic acid is 6.3 x 10-5. Find [H+] when
[C6H5COOH] = M and [C6H5COO-] is M. What is the
pH of the solution?

17. 3. 100 mole of methanoic acid, HCOOH, ionizes in 2
mole of methanoic acid, HCOOH, ionizes in 2.00 L of water, forming 4.2 x 10-3 mol/L of H+ ions. Calculate the Ka of methanoic acid and the pH of the solution.

18. BASE(Arrhenius): Releases OH- ions in solution
STRONG BASES WEAK BASES_______________
Completely dissociate in water
KOH(s)  K+(aq) + OH-(aq)
Hydoxides of Group IA, soluble hydroxides of Group IIA
NaOH, KOH, LiOH, Ba(OH)2, Ca(OH)2
Strong electrolytes –
Many ions in solution
What is the [OH-] in M NaOH? Its pH?
[OH-] = = 1 x 10-3 M
[H+] = 1 x 10-11, pH =
Incomplete ionization in water
Common: NH3 + H2O  NH4+ + OH-
& slightly soluble hydroxides: Mg(OH)2, Al(OH)3
2. Few ions in solution –
Weak electrolytes
11.00

19. STRONG ACID + STRONG BASE
H Cl (aq) + Na OH (aq) 
Actual reaction: H+ + OH-  H2O
Spectator ions:
Na+ and Cl-
EX. Ba (OH)2 (aq) + H NO3(aq) 
Ba(OH)2 (aq) + HNO3(aq)  Ba(NO3)2 + H2O
Spectator ions: Ba+2, NO3-1
Net ionic equation: H+ + OH-  H2O
H2O(l) + Na Cl (aq)
Ba +2(NO3) H2O

20. TITRATION Adding measured volumes of a base of known
molarity to an acid of unknown molarity until the
end point is reached.
1. Equivalence point: Endpoint
moles acid = moles base
a. INDICATOR detects it
2. A student titrates vinegar with M NaOH cm3 of NaOH is required to titrate cm3 of vinegar. What is the concentration of the vinegar?
Mol H+ = Mol OH-
V x M H+ = V x M OH-

21. 3. What volume of a 0. 200 M H2SO4 solution is needed to titrate 22
3. What volume of a M H2SO4 solution is needed to titrate 22.5 ml of M KOH?

22. Bronsted-Lowry Acids & Bases
Acid: Proton (H+) donor
Base: Proton (H+) acceptor
NH H2O  NH OH -
Base1
H2O HCl  H3O Cl-
Acid1
H2O Cl  OH HCl
Conjugate Acid-Base Pair
Separated by the loss or gain of a proton (H+)
NH3 <------> NH and H2O <-----> H3O+
Acid2
Acid1
Base2
Base2
Acid2
Base1
Base2
Base1
Acid2
Conjugate acid/base pairs

23. Since H2O acts as EITHER and acid or a base, is it _______________
Other examples: _____________________ See Table.
Strong acid:
Donates a proton readily
Strong base:
Accepts a proton readily
*The stronger an acid, the _______________ its conjugate base.*
HI H2O  I H3O+
SALT: Product of a neutralization reaction
Ex. NaCl, Ca(NO3)2, BaSO4 a.
amphoteric
weaker
S. Acid
W. Base
+ ion from base, - ion from acid

24. Hydrolysis
Some salts react with water to form solutions which are either acidic or basic. These undergo HYDROLYSIS. 1. Salts formed from the reaction of a strong acid and a weak base form SLIGHTLY ACIDIC solutions. NH4Cl + HOH  NH4OH + HCl Weak base Strong acid HYDROLYZES (Acidic solution) 2. Salts formed from the reaction of a weak acid and a strong base form SLIGHTLY BASIC solutions. NaCH3COO + HOH  NaOH + CH3COOH HYDROLYZES Strong base Weak acid (Basic solution)

25.                                                              
3. Salts formed from the reaction of a strong acid and a strong base form NEUTRAL solutions.   NaCl + HOH  NaOH HCl DOES NOT HYDROLZE