Teresa Nguyen and Rachel Tung
P.4
Solubility
Solubility:

The ability for a substance to dissolve in water.
Memorize Solubility Rules:
Compounds with the following are ALWAYS soluble
Alkali metals (H, Li, Na, K, Rb, Cs, Fr)
Nitrate (NO3-), Nitrite (NO2-)
Ammonium (NH4+), Ammonia (NH3)
Chlorate (ClO3-), Chlorite (ClO2-), Perchlorate (ClO4-)
Acetate (C2H3O2 )
Acidic Hydrogen (H_)
Compounds with the following are always
soluble…
Chloride (Cl-), Bromide (Br-), Iodide (I-)
Chromate (CrO42-)
Sulfate (SO42-)
Compounds with the following are always
insoluble…
Hydroxide (OH )
Oxide (O2-)
(S2-)
Sulfide
Phosphate (PO43-)
UNLESS with…
Silver (Ag+), Dimercury (Hg22+), Lead (Pb2+)
Silver (Ag+), Dimercury (Hg22+), Strontium (Sr2+),
Barium (Ba2+)
Mercury (Hg22+), Lead (Pb2+), Calcium (Ca2+),
Strontium (Sr2+), Barium (Ba2+)
UNLESS with…
Calcium (Ca2+), Strontium (Sr2+), Barium (Ba2+)
Strontium (Sr2+), Barium (Ba2+)
Compounds with the following are ALWAYS insoluble
Sulfite (SO32-)
Carbonate (CO32-)
Solubility Problems: Name whether these compounds are soluble or insoluble
RaOH
CaO
Ag2CrO4
SrSO4
K3PO4
(NH4)2O
HCl
PbI2
Al2(CO3)3
Zn(C2H3O2)2
Teresa Nguyen and Rachel Tung
P.4
Reactions
Chemical Reactions:

Chemical reaction – process by which one or more substances are changed into one or
more different substances
Reactants  Products
yields

Reactants – original substances

Products – resulting substances
Classifying Types of Reactions:

Synthesis
o 2 or more substances yields 1 product


A + X  AX
Decomposition
o 1 reactant yields 2 products

AX  A + X
o Specific Decomposition Reactions


Metallic carbonates yield metallic oxides and carbon dioxide

Metallic hydroxides yield metallic oxides and water

Metallic chlorates yield metallic chlorides and oxygen

Carbonic acid yields carbon dioxide and water
Single Displacement
o An element exchanges places with an ion of a compound to form a different
compound and a element

Single element on both sides of reaction

A + BX  B + AX

Check activity series to see if a single displacement reaction will occur

A reaction will only occur if the single element (A) is higher in the
series than the element in the compound (B).
Teresa Nguyen and Rachel Tung
P.4

Double-Displacement
o The ions from two compounds exchange places to form two different
compounds


AX + BY  AY + BX
Combustion
o A compound (usually hydrocarbon) reacts with oxygen and yields carbon dioxide
and water
Predicting Reaction Types – Steps:
1. Identify the type of reaction
2. Predict products in the word equation
3. Write formula equation using symbols
4. Balance equation
o Use coefficients to make sure both sides of the reaction have an equal number
of atoms for each element
5. Indicate phase of matter
o Use solubility rules

(s) = solid, (g) = gas, (l) = liquid, (aq) = aqueous
o If all of them are aqueous in a double displacement reaction,
there is no reaction.
*Remember:
o Ammonia – NH3
o Sulfur – S8
o Phosphorus – P4
Teresa Nguyen and Rachel Tung
P.4
Predicting Reaction Types WS:
Indicate the type of reaction (NR for no reaction), complete the word equation, and write a
balanced chemical equation for each of the following. Make sure to include phase symbols.
____ 1. Barium and Chlorine gas 
Activity Series:
____2. Magnesium and Potassium Iodide 
____ 3. Hydrochloric Acid and Ammonium Sulfide 
____ 4. Lithium Hydroxide 
____ 5. ___C6H12O6 + ___O2 
Element
Li
Rb
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Ni
Sn
Pb
____ 6. Rubidium and Sodium Nitrate 
____ 7. Silver + Fluorine 
____8. Phosphoric Acid and Calcium Hydroxide 
____ 9. Strontium Phosphide 
____ 10. Aluminum and Silver Bromide 
H2
Cu
Hg
Ag
Pt
Au
F2
Cl2
Br2
I2
Reactivity
React with cold
water and acids
replacing H
React with acids
or steam, but
usually not liquid
water, to replace
hydrogen
All react with
acids, but not
water, to replace
hydrogen
All react with
oxygen to from
oxides
Mostly
unreactive
Listed from most
to least reactive
Teresa Nguyen and Rachel Tung
P.4
Answer Key
Solubility Problems:
RaOH – insoluble
Ag2CrO4 – insoluble
K3PO4 - soluble
HCl - soluble
Al2(CO3)3 – insoluble
CaO – insoluble
SrSO4 – insoluble
(NH4)2O - soluble
PbI2 – insoluble
Zn(C2H3O2)2 – soluble
Predicting Reaction Types WS:
S
1. Barium and Chlorine gas  Barium Chloride
Ba(s) + Cl2(g)  BaCl2(aq)
NR
2. Magnesium and Potassium Iodide  No Reaction
Mg(s) + KI(aq)  NR
NR
3. Hydrochloric Acid and Ammonium Sulfide  No Reaction
HCl(aq) + (NH4)2S(aq)  NR (all aqueous)
D
4. Lithium Hydroxide  Lithium Oxide and Water
2LiOH(s)  Li2O(s) + H2O(l)
C
5. ___C6H12O6(g) + _6_O2(g)  6 CO2(g) + 6 H2O(g)
SD
6. Rubidium and Sodium Nitrate  Sodium and Rubidium Nitrate
Rb(s) + NaNO3(aq)  Na(s) + RbNO3(aq)
S
7. Silver + Fluorine  Silver Fluoride
2Ag(s) + F2(g)  2AgF(s)
DD
8. Phosphoric Acid and Calcium Hydroxide  Calcium Phosphate and Water
2H3PO4(aq) + 3Ca(OH)2(aq)  Ca3(PO4)2(s) + 6H2O(l)
D
9. Strontium Phosphide  Strontium and Phosphorous
2Sr3P2(s)  6Sr(s) + P4(s)
SD
10. Aluminum and Zinc Bromide  Zinc and Aluminum Bromide
2Al(s) + 3ZnBr2(aq)  3Zn(s) + 2AlBr3(aq)