1.Consider the reaction when a
Answer:
– Most alkali metal (group I metals) are always soluble
– Cations/Anions such as NH4+, HCO3-; ClO3-, NO3- are alwayssoluble
– Most halides are soluble, F-,Cl-,Br-,I-, exceptions = Ag+,Hg2+2, Pb+2 compounds
– Most sulfates are soluble (SO4-2); exceptions = Ag+, Ca+2,Sr+2, Ba+2, Hg2+2, Pb+2 compounds
– In general (except all alkali metals) these ions will NOT besoluble: PO4-3, CrO4-2, S-2, CO3-2
1.Consider the reaction when aqueous solutions ofChromium(II) iodide and sodium acetate are combined. The net ionicequation for this reaction is
CrI2(aq) + NaCH3COO(aq) = no reaction
Note that acetates and sodium are soluble, will not formcompounds
2.Consider the reaction when aqueous solutions oflead(II) acetate and manganese(II) iodide are combined. The netionic equation for this is
3. Consider the reaction when aqueous solutions oflead(II) nitrate and manganese (II) bromide are combined. The netionic equation for this is
Similar as in 2, Bromide ions and Lead form precipitate
Pb2+(aQ) + 2Br-(aq) = PbBr2(s)
4. Write the balanced net ionic equation for this reaction.Pb(NO3)2(aq)+MnI2(aq)->PbI2(s)+Mn(NO3)2(aq)
Net ionic includes only solid formatino
Pb2+(aq) + 2I-(aq) = PbI2(s)
5. Write a net ionic equation for the reaction thatoccurs when aqueous solutions of ammonia and nitric acid arecombined
net ionic is:
NH3(aq) + H+(aq) = NH4+(aq)
6. Write a net ionic equation for the reaction thatoccurs when aqueous solutions of ammonia and hypochlrous acid arecombined
similarly:
NH3(aq) + HClO(a) = NH4+(aq) + ClO-(aq)
ClO- must be added, since it is molecular and will form ClO- +H2O <-> HClO
7. Write a net ionic equation for the reaction thatoccurs when aqueous solutions of ammonia and hydrochloric acid arecombined
NH3(aq) + H+(aq) = NH4+(aq)
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