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Reactions in Aqueous Solutions

Chemical Reactions. Reactions in Aqueous Solutions. Learning Goals. Write complete ionic and net ionic equations for chemical reactions in aqueous solutions. Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas .

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Reactions in Aqueous Solutions

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  1. Chemical Reactions Reactions in Aqueous Solutions

  2. Learning Goals • Write complete ionic and net ionic equations for chemical reactions in aqueous solutions. • Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas. • Identify acid-base reactions and oxidation-reduction reactions.

  3. Aqueous Solutions • An aqueous solutioncontains one or more dissolved substances (called solutes) in water (the solvent).

  4. Aqueous Solutions • Water is always the solvent in an aqueous solution. • Solutes can be anything that is dissolved in water: • Ex: Sugar, alcohol, acids, bases, ionic compounds

  5. Aqueous Solutions • When ionic compounds dissolve in water, their ions separate in a process called dissociation.

  6. Aqueous Solutions • When two solutions that contain ions as solutes are combined, the ions might react. • If they react, it is always a double replacement reaction. • 3 types of products can form, a precipitate, water, or gas.

  7. Precipitation Reactions • Precipitation Reactions

  8. Solubility Rules • Use the solubility rules to predict which of the following substances are likely to be soluble in water: • Aluminum nitrate • Magnesium chloride • Rubidium sulfate • Nickel (II) hydroxide • Lead (II) sulfide • Magnesium hydroxide • Iron (III) phosphate

  9. Practice • Use the solubility rules to predict what will happen when the following solutions are mixed. Write the balanced equation for any reaction that occurs. • KNO3 (aq) and BaCl2(aq)

  10. Practice • Na2SO4(aq) and Pb(NO3)2(aq) • KOH(aq) and Fe(NO3) 3(aq)

  11. Practice • Ba(NO3)2 (aq) and NaCl(aq) • Na2S (aq) and Cu(NO3)2(aq)

  12. Practice • NH4Cl(aq) and Pb(NO3)2(aq)

  13. Ionic Equations • 2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s) • 2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s)

  14. Ionic Equations • Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations.

  15. Ionic Equations • Ions that do not participate in a reaction are called spectator ionsand are not usually written in ionic equations.

  16. Ionic Equations • Formulas that include only the particles that participate in reactions are called net ionic equations.

  17. Ionic Equations • 2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s) • 2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s) • 2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)

  18. Practice • Write chemical, complete ionic, and net ionic equations for each of the following reactions that produce a precipitate. • Aqueous solutions of potassium iodide and silver nitrate are mixed, forming the precipitate silver iodide.

  19. Practice • Aqueous solutions of aluminum chloride and sodium hydroxide are mixed, forming the precipitate aluminum hydroxide.

  20. Practice • When aqueous solutions of sodium carbonate and manganese (V) chloride are mixed, a precipitate containing manganese is formed.

  21. Reactions that Produce Water • Some reactions produce more water molecules. • No evidence of a chemical reaction is observable. • Water is a very stable compound. • When substances that can form water are mixed, there is a strong tendency for the reaction to occur.

  22. Reactions that Produce Water • Acids and Bases: • Arrhenius acids: substances that produces H+ ions when dissolved in water. • Acids that completely ionize into H+ are called strong acids.

  23. Reactions that Produce Water • Acids and Bases: • Arrhenius bases: substances that produces OH- ions when dissolved in water. • Bases that completely ionize into OH- are called strong bases.

  24. Reactions that Produce Water • HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq) • Without spectator ions H+(aq) + OH–(aq) → H2O(l).

  25. Practice • Write chemical, complete ionic, and net ionic equations for each of the following reactions that produce water. • Mixing sulfuric acid and aqueous potassium hydroxide produces water and aqueous potassium sulfate.

  26. Practice • When benzoic acid (HC7H5O2) and magnesium hydroxide are mixed, water and magnesium benzoate are produced.

  27. Practice • Aqueous nitric acid reacts with aqueous potassium hydroxide.

  28. Reactions that Produce Gas • Gases that are commonly produced are carbon dioxide, hydrogen cyanide, and hydrogen sulfide. • 2HI(aq) + Li2S(aq) → H2S(g) + 2LiI(aq)

  29. Reactions that Produce Gas • Two reactions can be combined and represented by a single chemical reaction.

  30. Reactions that Produce Gas • Combined equation • HCl(aq) + NaHCO3(aq) + H2CO3(aq) → H2CO3(aq) + NaCl(aq) + H2O(l) + CO2(g) • Overall equation • HCl(aq) + NaHCO3(aq) → H2O(l) + CO2(g) + NaCl(aq)

  31. Practice • Write chemical, complete ionic, and net ionic equations for each of the following reactions. • Perchloric acid reacts with aqueous potassium carbonate, forming carbon dioxide gas and water.

  32. Practice • Nitric acid reacts with aqueous potassium rubidium sulfide (KBrS), forming hydrogen sulfide gas.

  33. Oxidation-Reduction Reactions • Oxidation-Reduction Reactions involve a transfer of electrons. • Often reactions between metals and nonmetals.

  34. Oxidation-Reduction Reactions • 2Na(s) + Cl2(g)  2NaCl(s) • Na + Cl  Na+ + Cl- e-

  35. Oxidation-Reduction Reactions • 2Mg(s) + O2(g)  2MgO(s) • Mg + O  Mg2+ + O2- e- e- Also a combustion reaction!!

  36. Oxidation-Reduction Reactions • All combustion reactions are oxidation-reduction reactions!

  37. Oxidation-Reduction Reactions • 2Al(s) + Fe2O3(s)  2Fe(s) + Al2O3(s) • Al + Fe3+  Fe + Al3+ e- e- e- Also a single replacement reaction!!

  38. Oxidation-Reduction Reactions • Oxidation-Reduction Reactions

  39. Practice • For each reaction, show how electrons are gained and lost: • 2Na(s) + Br2(l)  2NaBr (s)

  40. Practice • For each reaction, show how electrons are gained and lost: • 2Ca(s) + O2(g)  2CaO(s)

  41. Classifying Reactions • Synthesis (combination) • Combustion • Decomposition • Single Replacement

  42. Classifying Reactions • Double Replacement • Precipitation Reactions • Acid-Base Reactions • Oxidation-Reduction Reactions

  43. Classifying Reactions • Classify each of the following reactions in as many ways possible. • 2K(s) + Cl2(g)  2KCl(s) • 2Mg(s) + O2(g)  2MgO(s)

  44. Classifying Reactions • Classify each of the following reactions in as many ways possible. • Fe2O3(s) + 2Al(s)  Al2O3(s) + 2Fe(s) • HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3 (aq)

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