Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate
Write balanced complete ionic and net ionic equations for each reaction. a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)
Verified Solution
Key Concepts
Complete Ionic Equation
Net Ionic Equation
Precipitation Reaction
Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)
Write balanced complete ionic and net ionic equations for each reaction. b. MgS(aq) + CuCl2(aq) → CuS(s) + MgCl2(aq)
Write balanced complete ionic and net ionic equations for each reaction. d. HC2H3O2(aq) + K2CO3(aq) → H2O(l ) + CO2(g) + KC2H3O2(aq)
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl- Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations for the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.