Writing Net-Ionic Equations

Writing Net-Ionic Equations Net-ionic equations show the actual reaction taking place and leave out the spectator ions Example 2: A solution of sodium chloride is mixed with a solution of lead (II) nitrate to produce aqueous sodium nitrate and solid lead (II) chloride. Molecular equation: write out the formula of every compound with state and balance the equation 2NaCl (aq) + Pb(NO3)2 (aq) → 2NaNO3 (aq) + PbCl2 (s) Total ionic Equation: any ionic compound or strong acid that is dissolved in water (aqueous) splits into ions. 2Na+ (aq) + 2Cl- (aq) + Pb2+ (aq) + 2NO3- (aq) → 2Na+ (aq) + 2NO3- (aq) + PbCl2 (s) Net-ionic Equation: remove any ions that are present in both the reactants and products. They are spectators. This equation is actually what happens in the reaction. 2Cl- (aq) + Pb2+ (aq) → PbCl2 (s) For each of the following reactions, write the total ionic and net-ionic equations. 1. Na2CO3(aq) + Fe(NO3)2 (aq) → 2 NaNO3(aq) + FeCO3(s) Total Ionic: 2 Na+(aq) + CO32-(aq) + Fe2+(aq) + 2 NO3-(aq) → 2 Na+ (aq) + 2 NO3-(aq) + FeCO3(s) Net-ionic Fe2+(aq) + CO32-(aq) → FeCO3(s) 2. HF(aq) + NaOH(aq) → NaF(aq) + H2O(l) Total Ionic: HF(aq) + Na+(aq) + OH-(aq) → Na+(aq) + F-(aq) + H2O(l) Net-ionic HF(aq) + OH-(aq) → F-(aq) + H2O(l) 3. Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq) Total Ionic: Zn(s) + Cu2+(aq) + 2 NO3-(aq) → Cu(s) + Zn2+(aq) + 2 NO3-(aq) Net-ionic Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq) 4. 2 KOH(aq) + H2SO4(aq) → K2SO4(aq) + 2 H2O(l) Total Ionic: 2 K+(aq) + 2 OH- (aq) + H+(aq) + HSO4-(aq) → 2 K+(aq) + SO42- (aq) + 2 H2O(l) Net-ionic 2 OH- (aq) + H+(aq) + HSO4-(aq) → SO42- (aq) + 2 H2O(l) Exercises: For each of the following write the molecular, total ionic, and net-ionic equations 5. Aqueous solutions of Calcium chloride and sodium sulfate are mixed to produce an aqueous solution of sodium chloride and a solid of calcium sulfate Molecular Equation: CaCl2 (aq) + Na2SO4 (aq) → 2NaCl (aq)+ CaSO4 (s) Total ionic equation: Ca2+ (aq) + 2Cl- (aq) + 2Na+ (aq) + SO4- (aq) → 2Na+ (aq) + 2Cl- (aq)+ CaSO4(s) Net-ionic equation: 6. Ca2+ (aq) + SO4- (aq) → CaSO4(s) A piece of magnesium is dropped into an aqueous solution of lead (IV) acetate to produce a solution of magnesium acetate and solid lead. Molecular Equation: Total ionic equation: 2Mg (s) + Pb(CH3COO)4 (aq) → 2Mg(CH3COO)2 (aq) + Pb (s) 2Mg (s) + Pb4+ (aq) + 4CH3COO- (aq) → 2Mg2+ (aq) +2CH3COO- (aq) + Pb (s) Net-ionic equation: 2Mg (s) + Pb4+ (aq) → 2Mg2+ (aq) + Pb (s) 7. Solid sodium carbonate is added to a solution of iron (III) nitrate producing a precipitate of iron (III) carbonate and aqueous sodium nitrate. Molecular Equation: 3Na2CO3 (s) + 2Fe(NO3)3 (aq) → Fe2(CO3)3 (s) + 6NaNO3 (aq) Total ionic equation: 3Na2CO3 (s) + 2Fe3+ (aq) + 6NO3- (aq) → Fe2(CO3)3 (s) + 6Na+ (aq) + 6NO3- (aq) Net-ionic equation: 3Na2CO3 (s) + 2Fe3+ (aq) → Fe2(CO3)3 (s) + 6Na+ (aq) 8. A piece of calcium is dropped into an aqueous solution of hydrochloric acid resulting in hydrogen gas being evolved and a solution of calcium chloride remaining. Molecular Equation: Ca (s) + 2 HCl (aq) → H2 (g) + CaCl2 (aq) Total ionic equation: Ca (s) + 2 H+(aq) + 2 Cl- (aq) → H2 (g) + Ca2+(aq) + 2 Cl- (aq) Net-ionic equation: Ca (s) + 2 H+(aq) → H2 (g) + Ca2+(aq) 9. A solution of Ammonium phosphate is added to a solution of lithium hydroxide to produce aqueous lithium phosphate, aqueous ammonia (NH3) and water. Molecular Equation: (NH4)3PO4 (aq) + 3LiOH (aq) → Li3PO4 (aq) + 3NH3 (aq) + 3H2O (l) Total ionic equation: 3NH4+ (aq)+ PO43- (aq) + 3Li+ (aq) + 3OH- (aq) → 3Li+ (aq) + PO43- (aq) + 3NH3 (aq) + 3H2O (l) Net-ionic equation: NH4+ (aq) + OH- (aq) → NH3 (aq) + H2O (l)