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Identifying Spectator Ions

• Chemical Equations
  • Reactions to Consider:
  • KOH(aq) + Fe(NO3)3(aq) →
  • NaC2H3O2(aq) + CaS(aq) →
  • K₂SO4(aq) + Pb(NO3)2(aq) →
  • CaCl2(aq) + Na3PO4(aq) →
  • KNO3(aq) + MgI2(aq) →
  • Mixed Solutions:
  • Solutions of iron (II) sulfate and barium hydroxide are mixed.
  • Solutions of calcium nitrate and sodium chloride are mixed.
  • Solutions of potassium chloride and silver nitrate are mixed.
  • Solutions of ammonium sulfate and barium chloride are mixed.
  • Balanced Equations & Ionic Equations:
  • Formulate balanced equations, ionic equations, and net ionic equations for reactions listed.

Oxidation Numbers & Redox Reactions

• Redox Reactions:
  • Identifying oxidation, reduction, oxidizing agent, and reducing agent, using oxidation numbers.
  • Examples of Redox Reactions:
  • $Mg + 2HCl → MgCl2 + H2$
  • $2Fe + 3V2O3 → Fe2O3 + 6Vo$
  • $2KMnO4 + 5KNO2 + 3H2SO4 → 2MnSO4 + 3H2O + 5KNO3 + K2SO4$
  • $K2Cr2O7 + 3SnCl2 + 14HCl → 2CrCl3 + 3SnCl4 + 2KCl + 7H2O$
  • $2KMnO4 + 10NaCl + 8H2O → 5Cl2 + K2SO4 + 2MnSO4 + 8H2O + 5Na2SO4$
  • $2K2Cr2O7 + 2H2O + 3S → 3SO2 + 4KOH + 2Cr2O3$
  • $8KClO3 + C12H22O11 → 8KCl + 11H2O + 12CO2$
  • $3H2C2O4 + 2KMnO4 → 6CO2 + 2K2O + Mn2O3 + 3H2O$
  • $2Mn(NO3)2 + 5NaBiO3 + 16HNO3 → 2HMnO4 + 5Bi(NO3)3 + 5NaNO3 + 7H2O$
  • $4H2C2O4 + 2KMnO4 → 8CO2 + K2O + Mn2O3 + 4H2O$

Balancing Chemical Equations

• Exercise:
  • Balance the following equations:
  • $NaNO3 + PbO → Pb(NO3)2 + Na2O$
  • $AgI + Fe2(CO3)3 → FeI3 + Ag2CO3$
  • $C2H4O2 + O2 → CO2 + H2O$
  • $ZnSO4 + Li2CO3 → ZnCO3 + Li2SO4$
  • $V2O5 + CaS → CaO + V2S3$
  • $Mn(NO2)2 + BeCl2 → Be(NO2)2 + MnCl2$
  • $AgBr + GaPO4 → Ag3PO4 + GaBr3$
  • $H2SO4 + B(OH)3 → B2(SO4)3 + H2O$
  • $S + O2 → SO2$
  • $Fe + AgNO3 → Fe(NO3)2 + Ag$

Stoichiometry of Reactions

• Example Stoichiometry Problem:
  • $2 MgO + F2 → 2 MgF2 + O2$
  • How many moles of O2 gas will be produced from the reaction of 3.4 moles of MgO?
  • How many moles of F2 are required to create 8.5 moles of MgF2?
  • Reaction: $4 Fe + 3O2 → 2 Fe2O3$
  • How many moles of Fe are needed to make 2 moles of Fe2O3?
  • How many moles of O2 are needed to make 2 moles of Fe2O3?
  • How many moles of O2 are needed to make 8.4 moles of Fe2O3?
  • How many moles of Fe2O3 will be made from 3.5 moles of O2?

Anaerobic Respiration and Related Calculations

• Anaerobic Reaction Example:
  • Glucose Conversion: $C6H12O6 → 2 C2H5OH + 2 CO2$
  • Molecular weight of glucose = 180 g/mol and ethanol = 46 g/mol.
  • Calculation: How many grams of carbon dioxide produced from 1.00 g of glucose?
• Antacid Reaction:
  • Calcium Hydroxide Reaction with Hydrochloric Acid: $Ca(OH)2 + 2 HCl → CaCl2 + 2 H2O$
  • Molar mass of $Ca(OH)2 = 75 ext{ g/mol}$
  • Calculation: How many moles of HCl needed for 150 g of Ca(OH)2?
• Ba(NO3)2 Precipitation:
  • Reaction: $3 Ba(NO3)2(aq) + Al2(SO4)3(aq) → 3 BaSO4(s) + 2 Al(NO3)3(aq)$
  • How many mL of 0.280 M Ba(NO3)2 are needed to precipitate all sulfate ions from 25.0 mL of 0.350 M aluminum sulfate?

Limiting Reactants

1. Reaction: $N2 + 3H2 → 2 NH3$

   • Calculate:
   • Grams of NH3 from 28 g of N2.
   • Grams of NH3 from 25 g of H2.
   • Identify limiting reactant when 28 g of N2 and 25 g of H2 are reacted.

2. Reaction: $C3H8 + 5 O2 → 4 H2O + 3 CO2$

   • Calculate:
   • Moles of water from 28 g of C3H8.
   • Moles of water from 45 g of O2.
   • Identify limiting reactant when 28 g of C3H8 and 45 g of O2 are reacted.

3. Precipitation Reaction:

   • $2 AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2 KNO3(aq)$
   • Calculate: How many grams of silver chromate will precipitate when 150 mL of 0.500 M silver nitrate are added to 100 mL of 0.400 M potassium chromate?

Percent Yield Calculation

• Example: If only 7.25 g of silver chromate precipitates, calculate the percent yield from the previous problem.

Identifying Types of Reactions

• Types of reactions to review include:
  • Combination: $P4 + O2 → P2O3$
  • Decomposition: $CaCO3 → CaO + CO2$
  • Single Replacement: $Pb + FeSO4 → PbSO4 + Fe$
  • Double Replacement: $MgCl2 + Li2CO3 → MgCO3 + LiCl$
  • Acid/Base: $Na3PO4 + KOH → NaOH + K3PO4$
  • Combustion: $C6H12 + O2 → CO2 + H2O$

Predicting a Precipitate

• Understand the solubility rules for ions:
  • The common ions studied include:
  • $NO3^-$, $ClO2^-$, $S2-$, $OH^−$, $Br^−$, $SO4^{2-}$, $Cl^{-}$, $PO4^{3-}$, $C2H3O2^{-}$
  • Relevant alkali metals and transition metals:
  • $Li^+$, $Na^+$, $K^+$, $NH_4^+$
  • $Ca^{2+}$, $Sr^{2+}$, $Ba^{2+}$, $Ni^{2+}$, $Fe^{3+}$, $Zn^{2+}$, $Cu^{2+}$, $Ag^+$, $Hg_2^{2+}$, $Pb^{2+}$
  • Predict the formation of precipitates based on the solubility of the involved ions.