|Exercise: Net Ionic Equations and Redox Balancing||
FYI - Solubility Rules
It is useful to remember some simple "rules" (really more like guidelines) to help in predicting reactions. For common compounds such as we see in general chemistry we can use the following rules:
Copper metal (Cu(s)) is immersed in an aqueous solution of silver nitrate (AgNO3). The solution turns light blue and a silver coating appears on the copper.
Dilute solutions of antimony(III) chloride and sodium sulfide are mixed to give a precipitate.
Dilute solutions of silver nitrate and potassium iodide are combined and give a yellow precipitate.
Dilute solutions of aluminum chloride and sodium hydroxide are mixed, giving a gelatinous precipitate.
Dilute solutions of calcium chloride and sodium phosphate are combined to give a precipitate.
Dilute solutions of nitric acid and sodium hydroxide are mixed, generating heat.
Dilute solutions of sulfuric acid and sodium hydroxide are mixed, generating heat.
A dilute solution of hydrochloric acid is poured over limestone (calcium carbonate) and a non-flammable, odorless gas is released as the rock dissolves.
Dilute solutions of lead(II) nitrate and sodium chloride are combined and give a white precipitate.
Dilute solutions of barium chloride and sodium sulfate are combined to give a white insoluble precipitate.
In addition to these exercises you should familiarize yourself with the text materials.
© R A Paselk
Last modified 23 October 2008