Solubility Rules For Ionic Compounds In Water
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1Solubility Rules for Ionic Compounds in Water
Soluble Ionic Compounds:
+
+
+
1.
All common compounds of Group 1 ions (Li
, Na
, K
etc…) and the ammonium
+
ion (NH
) are soluble.
4
- ), acetates (C
- or CH
COO - ), chlorates (ClO
-
2.
All common nitrates (NO
H
O
),
3
2
3
2
3
3
- ) are soluble.
and perchlorates (ClO
4
All common chlorides (Cl - ), bromides (Br - ), and iodides (I - ) are soluble, except
3.
+
2+
2+
those of Ag
, Pb
and Hg
.
2
2-
2+
2+
2+
+
2+
4.
All common sulfates (SO
) are soluble, except those of Ca
, Ba
, Sr
, Ag
, Pb
,
4
2+
and Hg
.
2
Insoluble Ionic Compounds:
1.
All common metal hydroxides are insoluble, except those of Group 1 and the larger
2+
members of Group 2 (starting with Ca
).
2-
3-
2-
2.
All common carbonates (CO
), phosphates (PO
), and sulfides (S
) are insoluble,
3
4
+
except those of Group 1 and NH
(because of Soluble rule #1).
4
Practice: predict the solubility of the following compounds.
a) Na
CO
b) Ca(CH
CO
)
c) MgCO
d) BaCl
e) AgCl
2
3
3
2
2
3
2
Tips for memorizing the solubility rule:
As with anything you need to memorize, learn 1 or 2 a day and then 1 or 2 more
the next day while reviewing the previous day. This is easier than trying to
memorize all at once. It also helps to look at the exceptions on the Periodic
Table.
- are
+
+
1) Soluble rules #1 and #2 are important since salts of Na
, K
, and NO
3
very common and Soluble list #1 explains most of the exceptions for the
Insoluble rules.
2) Mnemonics - To remember the exceptions for chlorides, bromides, iodides
2+
+
2+
(Soluble rule #3)....HAP…H = Hg
, A = Ag
, P = Pb
2
3) To remember the exceptions for sulfates (Soluble rule #4)...C-PBS (as in
2+
2+
2+
2+
watch Public Television)… C = Ca
, P = Pb
, B = Ba
, S = Sr
(plus others)
The exceptions are the same as Soluble rule #3 plus the heavier Group 2 ions.
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