What are the solubility rules for ionic compounds

Salts of the alkali metals are soluble. (Note: The alkali metals are in group 1.)

e.g. If M = Li, Na or K, then MX, M2X, M3X, etc. are soluble regardless of what X is.

2. Ammonium ( + NH4

) salts are soluble.

e.g. NH4 X, ( NH4

)2X, ( NH4

)3X, etc. are soluble regardless of what X is.

3. Nitrates NO3

-

are soluble.

e.g. MNO3, M(NO3)2, M(NO3)3, etc. are soluble regardless of what M is.

4. Halides i.e. chlorides (Cl-

), bromides (Br-

) and iodides (I-

) are soluble except for the

halides of lead (Pb2+), mercury (Hg+

and 2+ H 2

g ) and silver (Ag+

).

e.g. If X = Cl, Br or I, then MX, MX2, MX3, etc. are soluble unless M = Pb, Hg or Ag.

5. Sulfates ( 2-

SO4

) are soluble except for the sulfates of calcium, strontium, barium, silver

mercury and lead.

e.g. M2SO4, MSO4, M2(SO4)3, etc. are soluble unless M is from group 2 (the alkaline

earths) or M = Pb, Hg or Ag.

6. Carbonates ( 2- CO3

), phosphates ( 3- PO4

) and sulfides (S2-

) are insoluble except for

(i) the carbonates/phosphates/sulfides of the alkalis (because of Rule 1), and

(ii) ammonium carbonate/phosphate/sulfide (because of Rule 2).

7. Hydroxides (OH-

) are insoluble or slightly soluble except for the hydroxides of the

alkalis (because of Rule 1).

Note: The hydroxides of group 2 (the alkaline earth metals) are slightly soluble. Virtually

all other hydroxides are insoluble.

Explanation:

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