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Aqueous Reactions

Aqueous Reactions. Dr. Ron Rusay. Aqueous Reactions. There are several general types: 1) Precipitation: An insoluble salt forms from the addition of solutions. (Refer to Solubility Rules) 2) Acid-Base Reactions (Neutralization) generally produces a salt plus water

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Aqueous Reactions

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  1. Aqueous Reactions Dr. Ron Rusay

  2. Aqueous Reactions • There are several general types: 1) Precipitation: An insoluble salt forms from the addition of solutions. (Refer to Solubility Rules) 2) Acid-Base Reactions (Neutralization) generally produces a salt plus water 3) Oxidation-Reduction (Redox) there is a change in oxidation numbers between reactants and products

  3. Solution Test Apparatusfor Electrolytes

  4. Conductivity

  5. Electrolytes • Aqueous solutions can be categorized into 3 types: non-electrolytes, strong electrolytes or weak electrolytes based on their ability to conduct electricity. • A solution must have ions to conduct. • Pure Water does not conduct. • Aqueous solutions can be tested for conductivity which will determine the degree of ionization of the solutes. • It is possible to have full or partial ionization.

  6. Electrolytes Molarity (M) = Moles solute / Liter solution • Almost all ionic compounds and a few molecular compounds are strong electrolytes. • Several molecular compounds are weak conductors, most are non-conductors. • Conductivity is directly related to the amount of ionization, i.e. ions in solution. Table salt, sodium chloride, is completely ionized: NaCl(s) + H2O(l)NaCl(aq)0.10M Na+(aq) + Cl-(aq)0.00M0.10M 0.10M

  7. Electrolytes Molarity (M) = Moles solute / Liter solution • Concentrations: • CaCl2 (s) + H2O(l)CaCl2(aq)0.10M Ca2+(aq) + 2Cl-(aq)0.00M0.10M 0.20M

  8. Electrolytes Molarity (M) = Moles solute / Liter solution • Sugars like sucrose are non-ionic, molecular compounds that dissolve but produce no ions. C12H22O11 (S) + H2O(l)C12H22O11 (aq) • Some molecular compounds like acetic acid ionize partially (dissociate) in water HC2H3O2 (l) + H2O(l) H3O+(aq)+ 0.1000M C2H3O2 -(aq) 0.9987M 0.0013M

  9. Aqueous Acids • Any compound that provides a proton can be considered an acid. Strong acids are sulfuric acid, nitric acid, perchloric acid, HI, HBr and HCl.

  10. Electrolytes • How would the conductivity of acetic acid compare to hydrochloric acid?

  11. HCl Completely Ionized Acetic Acid (HC2H3O2)

  12. Aqueous Bases • Any compound that accepts a proton is a base. • The common bases are group IA & IIA metal hydroxide compounds. They are strong bases, dissociating completely in water. • An example of a weak base is ammonia. NH3 (g) + H2O(l) NH3 (aq) NH4+(aq)+ OH-(aq)

  13. An Aqueous Solution of Sodium Hydroxide NH3 in Water

  14. QUESTION

  15. Aqueous Reactions:Neutralization

  16. Aqueous Reactions:NeutralizationNet Ionic Equations HCl(aq) +NaOH(aq)NaCl(aq) + H2O(l) ___________________________________________________ • HCl(aq)H+(aq) + Cl-(aq) • NaOH(aq)Na+(aq)+ OH-(aq) • NaCl(aq)Na+(aq)+ Cl-(aq) ________________________________________________ Na+(aq)+ OH-(aq) +H+(aq) + Cl-(aq) Na+(aq)+ Cl-(aq) + H2O(l) _______________________________________________________ H+(aq) + OH -(aq)H2O(l)

  17. QUESTION An aqueous solution of H2SO4 is added to aqueous Ba(OH)2. The reaction is monitored using a conductivity tester. Predict the correct statement(s). I) Both H2SO4 and Ba(OH)2 are strong electrolytes. II) This is a neutralization reaction. III) This is a precipitation reaction. IV) The light bulb will glow at the neutralization point. A) II B) I and II C) I, II and III D) I, II, III and IV

  18. Aqueous Reactions:Acid-Base

  19. QUESTION If an antacid contains Al(OH)3 it will form AlCl3 upon neutralization of stomach acid. How many moles of Cl– ions are in 100.0 mL of 0.010 M AlCl3? 0.0010 M 0.010 M 0.0030 M 0.030 M Molarity (M) = Moles solute / Liter solution

  20. QUESTION

  21. What type of reaction is it? Write a balanced equation for the reaction. How do you know the state of the products?

  22. QUESTION Given the insoluble compound Al2(CO3)3 predict the ions and coefficients that would be necessary to complete the following net ionic equation: __ _____ + ____ _____ Al2(CO3)3 2 AlCl3 + 3 Na2CO3 also include 6 NaCl on right 3 Al3+ + 2 CO32– 2 Al3+ + 3 CO32– 2 Al3+ 6 Cl – + 3 CO32– +6 Na+

  23. Aqueous Reactions: PrecipitationNet Ionic Equations • 50mL of a 0.1M solution of sodium sulfate is mixed with 50mL of a 0.2M solution of silver nitrate. What is the result? • Molecular Equation: ?Na2SO4(aq)+ ?AgNO3(aq) ?Ag2SO4(s) + ?NaNO3(aq) 1 2 1 2

  24. Aqueous Reactions: Precipitation Net Ionic Equations Na2SO4(aq)+ 2 AgNO3(aq) Ag2SO4(s)+ 2 NaNO3(aq)0.1M0.2M Ionic Reaction (Reactants): Na2SO4(aq)2Na+(aq) + SO42-(aq) 2 AgNO3(aq)2Ag+(aq) + 2 NO31-(aq) 2 Na+(aq)+ SO42-(aq)+ 2 Ag+(aq)+ 2 NO31-(aq) 0.2M 0.1M 0.2M 0.2M

  25. Aqueous Reactions: Precipitation Net Ionic Equations Na2SO4(aq)+ 2 AgNO3(aq) Ag2SO4(s)+ 2 NaNO3(aq) 0.1M0.2M Ionic Reaction (Products): 2 NaNO3(aq)2Na+(aq) + 2 NO31-(aq) Ag2SO4(s)Does not dissolve (ionize) 2Na+(aq)+ 2NO31-(aq) + Ag2SO4(s) 0.2M 0.2M solid

  26. Aqueous Reactions: Precipitation Net Ionic Equations Na2SO4(aq)+ 2 AgNO3(aq) Ag2SO4(s)+ 2 NaNO3(aq) Overall Ionic Reaction: 2Na+(aq)+ SO42-(aq) +2Ag+(aq)+ 2NO31-(aq) 2Na+(aq) + Ag2SO4(s) + 2NO31-(aq) Net Ionic Equation: (Subtract Spectator Ions) 2Ag+(aq)+ SO42-(aq) Ag2SO4(s) How many moles? = MNa2SO4 xVNa2SO4 / 1:1stoichiometry M x Vsolution= mol = 0.10M x 0.050 L/ 1 = 0.0050 mol

  27. QUESTION

  28. Pb(NO3)2(aq) + NaI (aq) 2 NaNO3(aq) + PbI 2(s) 2 Write a balanced Net Ionic equation for the reaction. What are the spectator ions in the reaction?

  29. QUESTION

  30. QUESTION If you began a reaction with the following ions in solution (all would be written with an (aq) subscript how would you represent the proper final net ionic equation? (Consult a solubility Table.) 6Na+ + 2PO43– + 3Fe2+ + 6NO3– 3Na+ + PO43– + Fe2+ + 2NO3– No Reaction 6Na+ + 2PO43– + 3Fe2+ + 6NO3– Fe3(PO4)2 (s)+ 6NaNO3 3Na+ + PO43– + Fe2+ + 2NO3– Fe3(PO4)2 (s)+ 6 Na+ + 6 NO3– 2PO43– + 3Fe2+  Fe3(PO4)2 (s)

  31. Oxidation-Reduction • Oxidation is the loss of electrons. • Reduction is the gain of electrons. • The reactions occur together. One does not occur without the other. • The terms are used relative to the change in the oxidation state or oxidation number of the reactant(s).

  32. Aqueous Reactions:Oxidation - Reduction • In the following reaction, identify what is being oxidized and what is being reduced. What is the total number of electrons involved in the process?

  33. Oxidation Reduction Reactions

  34. QUESTION In a redox reaction, oxidation and reduction must both occur. Which statement provides an accurate premise of redox chemistry? The substance that is oxidized must be the oxidizing agent. The substance that is oxidized must gain electrons. The substance that is oxidized must have a higher oxidation number afterwards. The substance that is oxidized must combine with oxygen.

  35. QUESTION

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