1. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions Dr. Ron Rusay

2. © Copyright 1995-2010 R.J. 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 3) Oxidation-Reduction (Redox) there is a change in oxidation numbers between reactants and products

3. © Copyright 1995-2010 R.J. Rusay Solution Test Apparatus for Electrolytes

4. © Copyright 1995-2010 R.J. Rusay 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. © Copyright 1995-2010 R.J. Rusay Electrolytes  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) + H 2 O (l) ---> NaCl (aq) ---> 0.10MNa + (aq) + Cl - (aq) 0.00M 0.10M 0.10M Molarity (M) = Moles solute / Liter solution

7. © Copyright 1995-2010 R.J. Rusay Electrolytes � Concentrations: � 2 2 � CaCl 2 (s) + H 2 O (l) ---> CaCl 2(aq) ---> 0.10MCa 2+ (aq) + 2 Cl - (aq) 0.00M 0.10M 0.20M Molarity (M) = Moles solute / Liter solution

8. © Copyright 1995-2010 R.J. Rusay Electrolytes  Sugars like sucrose are non-ionic, molecular compounds that dissolve but produce no ions. C 12 H 22 O 11 (S) + H 2 O (l) ----> C 12 H 22 O 11 (aq)  Some molecular compounds like acetic acid ionize partially (dissociate) in water HC 2 H 3 O 2 (l) + H 2 O (l) H 3 O + (aq) + 0.1000M C 2 H 3 O 2 - (aq) 0.9987M 0.0013M Molarity (M) = Moles solute / Liter solution

9. © Copyright 1995-2010 R.J. Rusay 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. © Copyright 1995-2010 R.J. Rusay Electrolytes � How would the conductivity of acetic acid compare to hydrochloric acid?

11. HCl Completely Ionized Acetic Acid (HC 2 H 3 O 2 )

12. © Copyright 1995-2010 R.J. Rusay 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. NH 3 (g) + H 2 O (l) NH 3 (aq) NH 4 + (aq) + OH - (aq)

13. An Aqueous Solution of Sodium Hydroxide NH 3 in Water

15. QUESTION

16. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Neutralization

17. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Neutralization Net Ionic Equations HCl (aq) + NaOH (aq) ---> NaCl (aq) + H 2 O (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) + H 2 O (l) _______________________________________________________ H + (aq) + OH - (aq) ---> H 2 O (l)

18. An aqueous solution of H 2 SO 4 is added to aqueous Ba(OH) 2. The reaction is monitored using a conductivity tester. Predict the correct statement(s). I) Both H 2 SO 4 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 IVQUESTION

19. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Acid-Base

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

21. QUESTION

22. Pb(NO 3 ) 2 (aq) + NaI (aq)  NaNO 3 (aq) + PbI 2 (s) How do you know the state of the products: (s) vs. (aq)? What type of reaction is it? Double Displacement & Precipitation Write a balanced equation for the reaction. 2 2

24. QUESTION Given the insoluble compound Al 2 (CO 3 ) 3 predict the ions and coefficients that would be necessary to complete the following net ionic equation: __ _____ + ____ _____  Al 2 (CO 3 ) 3 A.2 AlCl 3 + 3 Na 2 CO 3 also include 6 NaCl on right B.3 Al 3+ + 2 CO 3 2– C.2 Al 3+ + 3 CO 3 2– D.2 Al 3+ 6 Cl – + 3 CO 3 2– + 6 Na +

25. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Precipitation Net 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: ?Na 2 SO 4(aq) + ?AgNO 3(aq) ---> ?Na 2 SO 4(aq) + ?AgNO 3(aq) ---> ?Ag 2 SO 4(s) + ?NaNO 3(aq) 1 2 12

26. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Precipitation Net Ionic Equations Na 2 SO 4(aq) + 2 AgNO 3(aq) -->Ag 2 SO 4(s) + 0.1M0.2M 2 NaNO 3(aq) Ionic Reaction (Reactants): Na 2 SO 4(aq)  2 Na + (aq) + SO 4 2- (aq) 2 AgNO 3(aq)  2 Ag + (aq) + 2 NO 3 1- (aq) 2 AgNO 3(aq)  2 Ag + (aq) + 2 NO 3 1- (aq) 2 Na + (aq) + SO 4 2- (aq) + 2 Ag + (aq) + 2 NO 3 1- (aq) 0.2M0.1M0.2M 0.2M 0.2M0.1M0.2M 0.2M

27. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Precipitation Net Ionic Equations Na 2 SO 4(aq) + 2 AgNO 3(aq) -->Ag 2 SO 4(s) + 0.1M0.2M 2 NaNO 3(aq) Ionic Reaction (Products): 2 NaNO 3(aq)  2 Na + (aq) + 2 NO 3 1- (aq) Ag 2 SO 4(s)  Does not dissolve (ionize) Ag 2 SO 4(s)  Does not dissolve (ionize) 2Na + (aq) + 2NO 3 1- (aq) + Ag 2 SO 4(s) 0.2M 0.2M solid 0.2M 0.2M solid

28. © Copyright 1995-2010 R.J. Rusay Aqueous Reactions: Precipitation Net Ionic Equations Na 2 SO 4(aq) + 2 AgNO 3(aq) -->Ag 2 SO 4(s) + 2 NaNO 3(aq) Overall Ionic Reaction: 2Na + (aq) + SO 4 2- (aq) +2Ag + (aq) + 2NO 3 1- (aq)  2Na + (aq) + Ag 2 SO 4(s) + 2NO 3 1- (aq) Net Ionic Equation: (Subtract Spectator Ions) 2Ag + (aq) + SO 4 2- (aq)  Ag 2 SO 4(s) = M Na2SO4 xV Na2SO4 / 1:1 stoichiometry = 0.10M x 0.050 L/ 1 = 0.0050 mol How many moles? M x V solution = mol

29. QUESTION

30. Pb(NO 3 ) 2 (aq) + NaI (aq)  NaNO 3 (aq) + PbI 2 (s) Write a balanced Net Ionic equation for the reaction. 2 2 Pb 2+ ( aq) + 2 I 1- (aq)  PbI 2 (s) What are the spectator ions in the reaction? 2 Na 1+ ( aq) ; 2 NO 3 1- (aq)

31. QUESTION

32. 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 + + 2PO 4 3– + 3Fe 2+ + 6NO 3 –  A.3Na + + PO 4 3– + Fe 2+ + 2NO 3 –  No Reaction B.6Na + + 2PO 4 3– + 3Fe 2+ + 6NO 3 –  Fe 3 (PO 4 ) 2 (s)+ 6NaNO 3 C.3Na + + PO 4 3– + Fe 2+ + 2NO 3 –  Fe 3 (PO 4 ) 2 (s)+ 6 Na + + 6 NO 3 – D.2PO 4 3– + 3Fe 2+  Fe 3 (PO 4 ) 2 (s)

33. © Copyright 1995-2010 R.J. Rusay 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).

34. © Copyright 1995-2010 R.J. Rusay 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?

36. © Copyright 1995-2010 R.J. Rusay

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