Net Ionic Equations

1. Net Ionic Equations There are 8 questions and you must answer 5 on the AP Exam!

2. Net Ionic Equations I • iron(III) ions are reduced by iodide ions. • hydrogen sulfide is bubbled through a solution of silver nitrate. • potassium permanganate solution is added to concentrated hydrochloric acid. • concentrated (15M) ammonia solution is added in excess to a solution of copper(II) nitrate. • magnesium metal is added to dilute nitric acid, giving as one of the products a compound in which the oxidation number for nitrogen is -3.

3. Net Ionic Equations I • Fe3+(aq) + I-(aq) Fe2+(aq) + I2 [or I3-(aq)] • H2S(aq) + Ag+(aq) Ag2S(s) + H+(aq) • MnO4-(aq) + H+(aq) + Cl-(aq) Mn2+(aq) + Cl2(g) + H2O • NH3(aq) + Cu2+(aq) [Cu(NH3)4]2+(aq) • Mg(s) + NO3-(aq) + H+(aq) Mg2+(aq) + NH4+(aq)

4. Net Ionic Equations II • excess water is added to solid calcium hydride. • excess silver acetate is added to a solution of trisodium phosphate. • solid sodium cyanide is added to water. • solid potassium hydride is added to anhydrous ethyl alcohol. • lithium metal is burned in air.

5. Net Ionic Equations II • CaH2(s) + H2O  H2(g) + Ca2+(aq) + OH-(aq) • AgCH3COO(s) + PO43-(aq) CH3COO-(aq) +Ag3PO4(s) [or Ag2HPO4 \ AgH2PO4] • NaCN(s) + H2O  HCN(aq) + Na+(aq) + OH-(aq) • KH(s) + C2H5OH  K+ + C2H5O- + H2(g) • Li(s) + O2(g) Li2O(s) \ Li(s) + N2(g) Li3N(s)

6. Net Ionic Equations III • aluminum metal is added to a solution of copper(II) chloride. • liquid phosphorus trichloride is poured into a large excess of water. • manganese(II) nitrate solution is mixed with sodium hydroxide solution. • equal volumes of dilute equimolar solutions of sodium carbonate and hydrochloric acid are mixed.

7. Net Ionic Equations III • Al(s) + Cu2+(aq) Al3+(aq) + Cu(s) • PCl3(l) + H2O  H3PO3(aq) + H+(aq) + Cl-(aq) • Mn2+(aq) + OH-(aq) Mn(OH)2(s) • CO32-(aq) + H+(aq) HCO3-(aq)

8. Net Ionic Equations IV • solid sodium carbide is added to an excess of water • an excess of sodium hydroxide solution is added to a solution of aluminum chloride • a mixture of solid calcium oxide and solid tetraphosphorus decaoxide is heated • solid barium peroxide is added to cold dilute sulfuric acid

9. Net Ionic Equations IV • Na2C2(s) + H2O  C2H2(g) + Na+(aq) + OH-(aq) • Al(H2O)63+(aq) + OH-(aq) AlO2-(aq) + H2O [or Al(OH)3(aq) \ Al(OH)4-(aq)] • CaO(s) + P4O10(s) Ca3(PO4)2(s) • BaO2(s) + H+(aq) + SO42-(aq) BaSO4(s) + H2O2(aq)

10. Net Ionic Equations V • dilute acetic acid solution is added to solid magnesium carbonate • the hydrocarbon hexane is burned in excess oxygen. • solid magnesium nitride is added to excess deuterium oxide. • gaseous hydrofluoric acid reacts with solid silicon dioxide

11. Net Ionic Equations V • CH3COOH(aq) + MgCO3(s) H2O + CO2(g) + Mg2+(aq) + CH3COO-(aq) • C6H14(l) + O2(g) CO2(g) + H2O(g) • Mg3N2(s) + D2O  ND3 + Mg(OD)2(s) [or MgO(s) \ Mg2+(aq) + OD-(aq)] • HF(g) + SiO2(s) SiF4 + H2O

12. Net Ionic Equations VI • potassium dichromate solution is added to an acidified solution of sodium sulfite. • dilute hydrochloric acid is added to a solution of diamminesilver(I) nitrate • equimolar amounts of trisodium phosphate and hydrogen chloride, both in solution, are mixed. • propene gas is mixed with bromine vapor.

13. Net Ionic Equations VI • Cr2Oa(2-,7 )(aq) + HSOa(-,3)(aq) SOa(2-,4 )(aq) + Cr3+(aq) + H2O • H+(aq) + Cl-(aq) + [Ag(NH3)2]+(aq) AgCl(s) + NH4+(aq) • PO43-(aq) + H+(aq) HPO42-(aq) • C3H6(g) + Br2(g) C3H6Br2

14. Net Ionic Equations VII • solid aluminum nitrate is dissolved in water. • solutions of potassium iodide, potassium iodate, and dilute sulfuric acid are mixed. • a solution of tin(II) sulfate is added to a solution of iron(III) sulfate • a suspension of copper(II) hydroxide is treated with an excess of ammonia water.

15. Net Ionic Equations VII • Al(NO3)3(s) + H2O  Al(H2O)63+(aq) + NO3-(aq) • I-(aq) + IO3-(aq) + H+(aq) H2O + I2(aq) [or I3-(aq)] • Sn2+(aq) + Fe3+(aq) Sn4+(aq) + Fe2+(aq) • Cu(OH)2(s) + NH3(aq) [Cu(NH3)4]2+(aq) + OH-(aq)

16. Net Ionic Equations VIII • a saturated solution of calcium hydroxide is added to a solution of magnesium chloride. • solid silver sulfide is warmed with dilute nitric acid. • hydrogen gas is passed over hot copper(II) oxide • solid zinc sulfide is heated in an excess of oxygen.

17. Net Ionic Equations VIII • OH-(aq) + Mg2+(aq) Mg(OH)2(s) • Ag2S(s) + H+(aq) + NO3-(aq) Ag+(aq) + S(s) + NO2(g) + H2O • H2(g) + CuO(s) H2O(g) + Cu(s) • ZnS(s) + O2(g) ZnO(s) + SO2(g)

18. Net Ionic Equations IX • a limited amount of liquid bromine is added to an excess of benzene. • a solution of diamminesilver(I) chloride is treated with dilute nitric acid. • metallic copper is heated with concentrated sulfuric acid. • sulfur dioxide gas is bubbled into an excess of a saturated solution of calcium hydroxide.

19. Net Ionic Equations IX • Br2(l) + C6H6(l) C6H5Br + HBr • [Ag(NH3)2]+(aq) + Cl-(aq) + H+ AgCl(s) + NH4+(aq) • Cu(s) + H2SO4 Cu2+ + SO2 + H2O • SO2(g) + Ca(OH)2(aq) CaSO3(s) + H2O

20. Net Ionic Equations X • manganese(IV) oxide is added to warm, concentrated hydrobromic acid. • hydrogen sulfide gas is added to a solution of cadmium nitrate. • chlorine gas is bubbled into cold dilute sodium hydroxide. • Solid iron(III) oxide is heated in excess carbon monoxide.

21. Net Ionic Equations X • MnO2(s) + H+(aq) + Br-(aq) Mn2+ + Br2 + H2O • H2S + Cd2+ CdS(s) + H+ • Cl2(g) + OH-(aq) ClO-(aq) + Cl-(aq) + H2O • Fe2O3(s) + CO(g) Fe(s) + CO2(g)

22. Net Ionic Equations XI • solid magnesium carbonate is heated. • trisodium phosphate crystals are added to water • gaseous diborane, B2H6, is burned in excess oxygen. • small chunks of solid sodium are added to water.

23. Net Ionic Equations XI • MgCO3(s) MgO(s) + CO2(g) • Na3PO4(s) + H2O  Na+(aq) + OH-(aq) + HPO42-(aq) [or H2PO4-(aq)] • B2H6(g) + O2(g) H2O + B2O3 [or H3BO3] • Na(s) + H2O  Na+(aq) + OH-(aq) + H2(g)

24. Net Ionic Equations XII • hydrogen peroxide solution is added to acidified potassium iodide solution. • pure methyl alcohol and pure acetic acid are mixed. • an excess of concentrated ammonia solution is added to freshly precipitated copper(II) hydroxide. • a sample of pure 2-butene is treated with hydrogen bromide gas.

25. Net Ionic Equations XII • H2O2(aq) + H+(aq) + I-(aq) H2O + I2(aq) or I3-(aq)] • CH3OH + CH3COOH  CH3COOCH3 + H2O • NH3(aq) + Cu(OH)2(s) [Cu(NH3)4]2+(aq) + OH-(aq) • C4H8(g) + HBr(g) C4H9Br

26. Net Ionic Equations XIII • water is added to a sample of pure phosphorus tribromide. • hydrogen peroxide is added to an acidified solution of potassium dichromate. • calcium metal is added to a dilute solution of hydrochloric acid. • a solution of sulfuric acid is added to a solution of barium hydroxide until the same number of moles of each compound has been added.

27. Net Ionic Equations XIII • H2O + PBr3(s) H3PO3(aq) + H+(aq) + Br-(aq) • H2O2 + H+(aq) + Cr2O72-(aq) Cr3+(aq) + H2O + O2(g) • Ca(s) + H+(aq) Ca2+(aq) + H2(g) • H+(aq) + SO42-(aq) + Ba2+(aq) + OH-(aq) BaSO4(s) + H2O

28. Net Ionic Equations XIV • excess dilute nitric acid is added containing the tetraaminecadmium(II) ion. • sulfur dioxide gas is bubble through an acidified solution of potassium permanganate. • pellets of aluminum metal are added to a solution containing an excess of sodium hydroxide. • a solution of sodium hydroxide is added to a solution of sodium dihydrogen phosphate until the same number of moles of each compound had been added.

29. Net Ionic Equations XIV • H+(aq) + [Cd(NH3)4]2+(aq) Cd2+(aq) + NH4+(aq) • SO2(g) + H+(aq) + MnO4-(aq) Mn2+(aq) + H2O + SO42-(aq) • Al(s) + OH-(aq) AlO2-(aq) + H2O + H2(g) [or Al(OH)4-(aq) \ Al(OH)63-(aq)] • OH-(aq) + H2PO4-(aq) H2O + HPO42-(aq)

30. Net Ionic Equations XV • a solution containing tin(II) ions is added to an acidified solution of potassium dichromate. • liquid bromine is added to a solution of potassium iodide. • an excess of ammonia gas is bubbled through a solution saturated with silver chloride. • water is added to a sample of pure sodium hydride.

31. Net Ionic Equations XV • Sn2+(aq) + H+(aq) + Cr2O72-(aq) Sn4+(aq) + Cr3+(aq) + H2O • Br2(l) + I-(aq) Br-(aq) + I2(aq) [or I3-(aq)] • NH3(g) + Ag+(aq) [Ag(NH3)2]+(aq) • NaH + H2O  Na+(aq) + H2(g) + OH-(aq)

32. Net Ionic Equations XVI • an excess of chlorine gas is added to pure acetylene. • a dilute solution of sulfuric acid is electrolyzed between platinum electrodes. • excess oxygen gas is mixed with ammonia gas in the presence of platinum. • dilute nitric acid is added to crystals of pure calcium oxide

33. Net Ionic Equations XVI • Cl2(g) + C2H2(g) C2H2Cl4 • H2O  H2(g) + O2(g) • O2(g) + NH3(g) NO2 + H2O • H+(aq) + CaO(s) Ca2+(aq) + H2O

34. Net Ionic Equations XVII • a solution of sodium hydroxide is added to a solution of calcium hydrogen carbonate until the number of moles of sodium hydroxide added is twice the number of moles of the calcium salt. • solid calcium oxide is exposed to a stream of carbon dioxide gas. • dinitrogen trioxide gas is bubbled into water. • Sodium hydrogen carbonate is dissolved in water. • pellets of lead are dropped into hot sulfuric acid.

35. Net Ionic Equations XVII • OH-(aq) + HCO32-(aq) H2O + CO32-(aq) • CaO(s) + CO2(g) CaCO3(s) • N2O3(g) +H2O  HNO2(aq) • NaHCO3(s) + H2O  Na+(aq) + HCO3-(aq) [or H2CO3(aq) + OH-(aq)] • Pb(s) + H+(aq) + SO42-(aq) H2O + SO2(g) + Pb2+(aq) [or PbSO4]

36. Net Ionic Equations XVIII • potassium permanganate solution is added to a solution of oxalic acid, H2C2O4, acidified with a few drops of sulfuric acid. • magnesium turnings are added to a solution of iron(III) chloride. • ethyl acetate is treated with a solution of sodium hydroxide. • a suspension of zinc hydroxide is treated with concentrated sodium hydroxide solution.

37. Net Ionic Equations XVIII • MnO4-(aq) + H2C2O4 + H+(aq) Mn2+(aq) + H2O + CO2(g) • Mg(s) + Fe3+(aq) Mg2+(aq) + Fe2+(aq) • CH3COOC2H5 + OH-(aq) C2H5OH(aq) + CH3COO-(aq) • Zn(OH)2 + OH-(aq) ZnO22-(aq) + H2O [or Zn(OH)3-(aq)]

38. Net Ionic Equations XIX • dilute sulfuric acid is added to a solution of barium acetate. • ammonium chloride crystals are added to a solution of sodium hydroxide. • solid phosphorus pentachloride is added to excess water. • a solution of hydrogen peroxide is catalytically decomposed. • powdered iron is added to a solution of iron(III) sulfate.

39. Net Ionic Equations XIX • H+(aq) + SO42-(aq) + Ba2+(aq) + CH3COO-(aq) BaSO4(s) + CH3COOH(aq) • NH4Cl(s) + OH-(aq) NH3(aq) + H2O + Cl-(aq) • PCl5(s) + H2O  H3PO4(aq) + H2O + H+(aq) + Cl-(aq) • H2O2 H2O + O2 • Fe(s) + Fe3+(aq) Fe2+(aq)

40. Net Ionic Equations XX • chlorine gas is bubbled into a solution of sodium bromide. • a precipitate is formed when solutions of trisodium phosphate and calcium chloride are mixed. • benzene is treated with bromine in the presence of a catalyst. • gaseous silane, SiH4, is burned in oxygen.

41. Net Ionic Equations XX • Cl2(g) + Br-(aq) Cl-(aq) + Br2 • PO43-(aq) + Ca2+(aq) Ca3(PO4)2(s) • Br2 + C6H6 C6H5Br + HBr • SiH4(g) + O2(g) SiO2(s) + H2O

42. Net Ionic Equations XXI • equal volumes of 0.1M hydrochloric acid and 0.1M sodium monohydrogen phosphate are mixed. • hydrogen sulfide gas is bubbled through a solution of lead(II) nitrate. • solid zinc strips are added to a solution of copper(II) sulfate. • solid lithium oxide is added to excess water.

43. Net Ionic Equations XXI • H+(aq) + HPO42-(aq) H2PO4-(aq) • H2S(s) + Pb2+(aq) PbS(s) + H+(aq) • Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s) • Li2O(s) + H2O  Li+(aq) + OH-(aq)

44. Net Ionic Equations XXII • copper(II) sulfide is oxidized by dilute nitric acid • silver chloride is dissolved in excess ammonia solution. • propene reacts with water in the presence of a catalyst. • a solution of copper(II) sulfate is electrolyzed using inert electrodes.

45. Net Ionic Equations XXII • CuS(s) + H+(aq) + NO3-(aq) Cu2+(aq) + SO2 + NO + H2O • AgCl(s) + NH3(aq) [Ag(NH3)2]+(aq) + Cl-(aq) • C3H6 + H2O  C3H7OH • Cu2+(aq) + H2O  Cu(s) + O2(g) + H+(aq)

46. Net Ionic Equations XXIII • hydrogen sulfide gas is bubbled through excess potassium hydroxide solution. • solutions of silver nitrate and sodium chromate are mixed. • sodium hydroxide solution is added to a precipitate of aluminum hydroxide in water. • solid sodium sulfite is added to water.

47. Net Ionic Equations XXIII • H2S(g) + OH-(aq) S2-(aq) + H2O • Ag+(aq) + CrO42-(aq) Ag2CrO4(s) • Al(OH)3(s) + OH-(aq) H2O + AlO2-(aq) [or Al(OH)4-] • Na2SO3(s) + H2O  Na+(aq) + HSO3-(aq) + OH-(aq)

48. Net Ionic Equations XXIV • a solution of formic acid, HCOOH, is oxidized by an acidified solution of potassium dichromate. • ammonia gas and carbon dioxide gas are bubbled into water. • concentrated hydrochloric acid solution is added to solid manganese(IV) oxide and the reactants are heated. • solutions of sodium fluoride and dilute hydrochloric acid are mixed. • a saturated solution of barium hydroxide is mixed with a solution of iron(III) sulfate.

49. Net Ionic Equations XXIV • HCOOH(aq) + H+(aq) + Cr2O72-(aq) CO2(g) + H2O + Cr3+(aq) • NH3(g) + CO2(g) + H2O  {NH4OH + H2CO3}  NH4+(aq) + CO32-(aq) • HCl + MnO2 Cl2(g) + Mn2+(aq) + H2O • F-(aq) + H+(aq) HF(aq) • Ba2+(aq) + OH-(aq) + Fe3+(aq) + SO42-(aq) BaSO4(s) + Fe(OH)3(s)

50. Net Ionic Equations XXV • a solution of ammonium sulfate is added to a potassium hydroxide solution. • carbon dioxide gas is bubbled through a concentrated solution of sodium hydroxide. • solid copper is added to a dilute nitric acid solution. • chlorine gas is bubbled into a cold solution of dilute sodium hydroxide.