2NaBr(aq) + Pb(OH)2(aq)  PbBr2(s) + 2NaOH(aq)

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2NaBr(aq) + Pb(OH)2(aq)  PbBr2(s) + 2NaOH(aq) Warmup 1. Write (predict products too) and balance this equation: sodium bromide and lead(II)hydroxide solutions are mixed to create a precipitate in a basic solution. 2NaBr(aq) + Pb(OH)2(aq)  PbBr2(s) + 2NaOH(aq) You’ll need your solubility rules, ion sheets, and Oops I Did it Again Lab today.

Net Ionic Equations

Part I: Net Ion Equations Actually….in double replacement reactions, we only show the species that changed phase, or that were integrated or disintegrated into something new. We eliminate “spectator ions” and just show the net ionic equation. Also, we have to use solubility rules to predict the precipitate. 2Na++ 2Br-+ Pb2+ + 2OH-  Pb2+ + 2Br- + 2Na+ + 2OH- 2Br-(aq) + Pb2+(aq)  PbBr2(s)

For each pair of ionic compounds shown: a For each pair of ionic compounds shown: a. Split the reactants into ions and write the complete ionic equation. b. Write the net ionic equation. Indicate solid precipitates (insoluble compounds) in the products. Na2S(aq) + AlCl3(aq)  ??????????? Na+ + S2- + Al3+ + Cl-  Na+ + S2- + Al3+ + Cl- 3S2-(aq) + 2Al3+(aq)  Al2S3(s) Ba(NO3)2(aq) + Ag2SO4(aq)  ??????????? Ba2+ + NO3- +Ag+ + SO42-  Ba2+ + NO3- + Ag+ + SO42- Ba2+(aq) + SO42- (aq)  BaSO4(s)

Hint: chlorates tend to be soluble For each pair of ionic compounds shown: a. Split the reactants into ions and write the complete ionic equation. b. Write the net ionic equation. Indicate solid precipitates (insoluble compounds) in the products. Pb3(PO4)2(aq) + NaClO3(aq)  Pb2+ +PO43- + Na+ + ClO3-  Pb2++ PO43- +Na+ + ClO3- NO REACTION KI(aq) + Pb(NO3)2(aq)  K+ + I- + Pb2+ + NO3-  K+ + I- + Pb2+ + NO3- 2I-(aq) + Pb2+(aq)  PbI2(s)

K2CrO4(aq) + Ba(NO3)2 (aq)  product A potassium chromate solution and barium nitrate solution are combined, producing a yellow precipitate. Write the net ionic equation for this reaction and identify the precipitate. K2CrO4(aq) + Ba(NO3)2 (aq)  product molecular equation 2K+ +CrO42- +Ba2+ + 2NO3- 2K+ +CrO42- +Ba2+ +2NO3- complete ionic equation  2KNO3(?) and BaCrO4(?) CrO42-(aq) + Ba2+(aq)  BaCrO4(s)

(do these with a neighbor, 5 minutes) Write the net ionic equation for the reaction, if any, that occurs when aqueous solutions of the following are mixed. You will have to predict and write the products! Chromium(III) chloride and sodium hydroxide Silver nitrate and ammonium carbonate Copper(II)sulfate and mercury(I) nitrate Strontium nitrate and potassium iodide

Chromium(III) chloride and sodium hydroxide Cr3+(aq) + 3OH-(aq)  Cr(OH)3(s) b. Silver nitrate and ammonium carbonate Ag+(aq) + CO32-(aq)  Ag2CO3(s) c. Copper(II)sulfate and mercury(I) nitrate SO42-(aq) + Hg22+(aq)  Hg2SO4(s) d. Strontium nitrate and potassium iodide Sr2+ + NO3- + K+ + I-  Sr2+ + NO3- + K+ + I- NO REACTION

Oooops I Did it Again! Lab! Spend 10 minutes on prelab Please label all 8 of your disposable pipets and do NOT throw them away!