KNOW
Acetate
Bicarbonate
Carbonate
Hydroxide
Hyperchlorite
Nitrate
Nitrite
Phosphate
Sulfate
Sulfite
Ammonium
C
2
H
3
O
2
-
HCO
3
-
Soluble
CO
3
2-
OH - The strongest base of all
OCl -
NO
3
-
NO
2
-
Soluble
PO
4
3-
SO
4
2-
SO
3
2-
NH
3
+
( H
3
0 +
is the strongest acid of all) (hydronium ion)
SOLUBLE:
All sodium (Na), potassium (K) and ammonium (NH
4
+
) compounds are soluble.
All nitrates are soluble (ex: NH
4
NO
3
– ammonium nitrate, used in fertilizer).
Most chlorides are soluble (except silver (Ag), mercury (Hg) and lead (Pb) chlorides)
Most sulfates are soluble (except strontium (Sr), barium (Ba) and lead (Pb) sulfate)
(ex: of soluble sulfate: Na
2
SO
4
- Sodium sulfate)
---------
INSOLUBLE:
Most carbonates are IN soluble (except those with Group 1A or NH
4
+
cations)
(Group 1A: Li, Na, K, Rb, Cs, Fr)
Most hydroxides and oxides are IN soluble (except those with Group 1A or NH
4
+
cations)
Most sulfides are IN soluble (except those with Group 1A or NH
4
+
cations)
(ex of insoluble sulfide: HgS – mercury sulfide)
1

STRONG ACIDS
HClO
4
H
2
SO
4
HI
HBr
HCl
HNO
3
From Group 7
ALWAYS
: A polyatomic ion with an “ H + ” will create an acid –
The H
+
will replace the “ - “ (negative sign for “ion”).
ALWAYS :
Group 1 A with a hydroxide ( OH ) will create a strong base
ALWAYS :
Strong base in the equation will always make the equation DOUBLE REPLACEMENT
ALWAYS :
Strong base with any acid will always create a WATER and SALT
Ex:
* HC
2
H
3
O
2
+ NaOH -----

H
2
O + NaC
2
H
3
O
2
(HC
2
H
3
O
2
is acetate with an “H”, creating Acetic acid)
2

Hydrochloric acid
Phosphorous acid
Phosphoric Acid
Hydrofluoric acid
Hydroselenic acid
Acetic acid
HCl
H
3
PO
3
H
3
PO
4
HF
H
2
Se
CH
3
COOH
H
2
CO
3
H
2
S
STRONG ACID
Carbonic acid
Hydrosulfuric acid
Hypochlorite ion
Cyanide ion
Ammonia
Carbonate ion
Aluminum hydroxide
Phosphate ion
Silicate ion
Hydroxide ion
ClO -
CN
-
NH
3
CO
3
2-
Al(OH)
3
PO
43-
SiO
3
2-
OH -
Weak acid
Neutral solution
Weak base
STRONG BASE
STRONG BASES:
All the hydroxides of Group 1A: LiOH, NaOH, KOH, RbOH and CsOH are strong bases
The alkaline earth (Group 2A) hydroxides: Ca(OH)
2
, Ba(OH)
2
and Sr(OH)
2
are also strong bases.
From notes:
STRONG BASES (contain OH):
LiOH
NaOH
From Group 1A
KOH
Sr(OH)
2
Ca(OH)
2
Ba(OH)
2
From Group 2A
3

KNOW:
Deuterium
2 2
H aka:
1 1 d and
Tritium
3 3
H aka: t
1 1
NUCLEAR BELT OF STABILITY
Above the belt : TOO MANY NEUTRONS - beta emission
Below the belt : NOT ENOUGH NEUTRONS – positron emission
(either by spontaneous positron emission or by electron capture followed by positron emission, but either way, a positron comes flyin out)
THE RULES:
1.
Not enough neutrons : POSITRON emission through electron capture and then positron ( B
+
) emission or through spontaneous positron emission)
2.
Too many neutrons : Neutron is converted into a proton and the leftover Beta
(B ) particle is kicked out
3.
Atomic weight over 83
: Use the helium nuclei “equation” to kick out an alpha particle (positively charged)
FISSION: LESS MASS IN PRODUCT (“Mass Defect”)
What nuclear power plants there are in U.S. are fission.
Europe’s are breeder reactors.
4

[H
+
] of .1 M? pH is 1 pOH is 13
[OH-] is 10 -3
.001 M of NaOH
[OH-] is .001
.001 M Ba(OH)
2
[OH-] is .002 (because there’s 2x of OH)
[OH-] = .001 or 1 x 10
-3 pOH = 5 pH = 11
[H
+
] = 10
-11
[OH
-
] = .002 pOH = 2.7 pH = 11.3
[H + ] = 10 -11.3
and, the inverse log of (-11.3) is 5.01 X 10
-12
5

Strong electrolytes: Strong acids, strong bases and soluble ionic compounds
Weak electrolytes: Weak acids, weak bases
Non electrolytes: Covalent compounds or insoluble ionic compounds
Neutralization reaction example:
Question:
Al(OH)
3
+ HNO
2
----

H
2
0 + Al(NO
2
)
Answer:
Al(OH)
3
+ 3 HNO
2
--

3H
2
0 + Al(NO
2
)
3
Hydroxide with metals: ALWAYS FORMS BASES
ALL COVALENT Compounds with NITROGEN or PHOSPHOROUS are WEAK BASES
When strong acids & bases are all on the reactant side, use TWO arrows
KNOW:
Causes of acid rain (sulfur oxides & nitrogen oxides)
Where these come from (sulfur oxides are from coal-burning power plants and coalburning industries) – (nitrogen oxides are from transportation)
Normal pH of rain: 5.6
Limestone (statue) / acid rain equation:
CaCO
3
+ H
2
SO
4
---

CaSO
4
+ H
2
CO
3
H
2
CO
3
is further broken down (it’s carbonic acid)
Into: H
2
O + CO
2
6