1. Write an equation for the precipitation reaction that occurs (if any) when solutions of sodium carbonate and copper(II) chloride are mixed.
2. Combine the cation from one reactant with the anion from the other. Make sure to write correct (charge-neutral) formulas for the new ionic compounds. Na 2 CO 3 (aq) + CuCl 2 (aq)
3. Use the solubility rules to determine whether any of the potential new products are indeed insoluble. Na 2 CO 3 (aq) + CuCl 2 (aq) NaCl + CuCO 3
4. If all of the potentially insoluble products are soluble, there will be no precipitate. Write NO REACTION next to the arrow.
5. One of the potentially insoluble products is insoluble, so write its formula as the product of the reaction, using (s) to indicate solid. Write the soluble product with (aq) to indicate aqueous. Na 2 CO 3 (aq) + CuCl 2 (aq) NaCl(aq) + CuCO 3 (s)
6. Balance the equation. Na 2 CO 3 (aq) + CuCl 2 (aq) NaCl(aq) + CuCO 3 (s) Na 2 CO 3 (aq) + CuCl 2 (aq) 2NaCl (aq) + CuCO 3 (s)
Use the solubility rules to predict what will happen when the following solutions are mixed. Write the balanced equation for any reaction that occurs. Na 2 SO 4 (aq) and Pb(NO 3 ) 2 (aq)
Write chemical, complete ionic, and net ionic equations for each of the following reactions that produce a precipitate. Aqueous solutions of potassium iodide and silver nitrate are mixed, forming the precipitate silver iodide.
Aqueous solutions of aluminum chloride and sodium hydroxide are mixed, forming the precipitate aluminum hydroxide.
Aqueous solutions of sodium carbonate and manganese (V) chloride are mixed.