Solubility of Ionic Compounds (to be filed in MISC. Section)

 

 

SOLUBLE COMPOUNDS (no ppt*)

Exceptions (change soluble to insoluble)

1

C2H3O21- , NO3 - , ClO3-, ClO4- salts

no exceptions

2

Group 1A (Na+), NH4+ salts

no exceptions

3

Cl -, Br -, I - salts

Except if combined with Ag+, Hg22+, Pb2+, Pb4+

4

SO42- , SO32- salts

Except if combined with Ag+, Ba2+, Pb2+, Pb4+,

Ca2+, Sr2+, Hg22+

 

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INSOLUBLE COMPOUNDS (ppt* forms)

Exceptions (change insoluble to soluble)

5

S2-, CO32-, PO43-, CrO42- salts

Except if combined with Na+, K+, NH4+

6

OH - salts (bases)

Except if combined with Na+, K+, Ca2+, Cs+, Li+, NH4+, Rb+, Ba2+, Sr2+

 ppt* = precipitate (an insoluble solid will form)

 

 Ions in the Exceptions column of the INSOLUBLE COMPOUNDS SECTION of the chart mixed with any of the ions to their left, will cause those ions to move up to the soluble compound section on the top - making them soluble.

 

Ions in the Exceptions column of the SOLUBLE COMPOUNDS SECTION of the chart mixed with any of the ions to their left, will cause those ions to move down to the insoluble compound section on the bottom making them insoluble.

 

 

NOTE: This table is adapted after Figure 7.3 on page 185 of your textbook. With it you can determine if the product of a reaction is soluble (will dissolve in water) or insoluble (will form a precipitate).

 

IONS THAT I ADDED TO THE CHART (helps for Solubility Lab)

 

LINE 1 C2H3O21-, ClO3-, ClO4- additional soluble ions

LINE 3 Pb4+ as an exception

LINE 4 SO32- additional soluble ion

Ag+, Pb4+, Sr2+, Hg22+ as exceptions

LINE 5 CrO42- as an insoluble salt

Na+, K+, NH4+ as an exceptions

LINE 4 Sr2+, Cs+, Li+, NH4+, Rb+, Ba2+ as an exceptions