Use the following table to determine whether or not a precipitate forms when the solutions listed below are mixed. In the space at the left, write the formula for the precipitate if one is
formed. Write NP if no precipitate is formed. Use examples 1 and 2 as guides.
Solubility Rules for Some Common Compounds
1.Compounds that contain these ions will not form precipitates.
All ions from group 1 metals
Ammonium, nitrate, and acetate polyatomic ions
Chloride, bromide, and iodide ions, unless combined with silver, mercury(I), or lead
2.Compounds that contain these ions usually will form precipitates.
Oxide and sulfide ions
Carbonate, hydroxide, and phosphate polyatomic ions
3.If a compound contains an ion mentioned in Rule 1, it will not form a precipitate, even if it contains an ion mentioned in Rule 2.
For example, ammonium sulfide will dissolve in water. Although sulfides usually don’t dissolve in water, all ammonium compounds will dissolve.
Example 1: sodium hydroxide and lead(II) nitrate
If a reaction were to occur, lead(II) hydroxide and sodium nitrate would form. According to
the table, lead(II) hydroxide forms a precipitate. The formula for the precipitate is Pb(OH)2.
Example 2: ammonium acetate and potassium phosphate
If a reaction were to occur, ammonium phosphate and potassium acetate would form.
According to the table, neither forms a precipitate. No reaction occurs.

1.potassium chloride and mercury(I) nitrate
2.ammonium carbonate and potassium nitrate