1. © 2009, Prentice-Hall, Inc. Chapter 4 Aqueous Reactions and Solution Stoichiometry

2. © 2009, Prentice-Hall, Inc. Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other substances are solutes.

3. © 2009, Prentice-Hall, Inc. Dissociation When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them. This process is called dissociation.

4. © 2009, Prentice-Hall, Inc. Dissociation An electrolyte is a substances that dissociates into ions when dissolved in water.

5. © 2009, Prentice-Hall, Inc. Electrolytes An electrolyte is a substances that dissociates into ions when dissolved in water. A nonelectrolyte may dissolve in water, but it does not dissociate into ions when it does so.

6. © 2009, Prentice-Hall, Inc. Electrolytes and Nonelectrolytes Soluble ionic compounds tend to be electrolytes.

7. © 2009, Prentice-Hall, Inc. Electrolytes and Nonelectrolytes Molecular compounds tend to be nonelectrolytes, except for acids and bases.

8. © 2009, Prentice-Hall, Inc. Electrolytes A strong electrolyte dissociates completely when dissolved in water. A weak electrolyte only dissociates partially when dissolved in water.

9. © 2009, Prentice-Hall, Inc. Strong Electrolytes Are… Strong acids Strong bases

10. © 2009, Prentice-Hall, Inc. Strong Electrolytes Are… Strong acids Strong bases Soluble ionic salts

11. Using Solubility Rules Classify the following ionic compounds as soluble or insoluble in water: (a) sodium carbonate (Na 2 CO 3 ), (b) lead sulfate (PbSO 4 ) (c) cobalt(II) hydroxide, (d) barium nitrate, (e) ammonium phosphate. © 2009, Prentice-Hall, Inc.

12. Precipitation Reactions When one mixes ions that form compounds that are insoluble (as could be predicted by the solubility guidelines), a precipitate is formed.

13. © 2009, Prentice-Hall, Inc. Metathesis (Exchange) Reactions Metathesis comes from a Greek word that means “to transpose.” AgNO 3 (aq) + KCl (aq)  AgCl (s) + KNO 3 (aq)

14. © 2009, Prentice-Hall, Inc. Metathesis (Exchange) Reactions Metathesis comes from a Greek word that means “to transpose.” It appears the ions in the reactant compounds exchange, or transpose, ions. AgNO 3 (aq) + KCl (aq)  AgCl (s) + KNO 3 (aq)

15. Predicting a Metathesis Reaction (a)Predict the identity of the precipitate that forms when solutions of BaCl 2 and K 2 SO 4 are mixed. Write the balanced chemical equation for the reaction. (b)What compound precipitates when solutions of Fe 2 (SO 4 ) 3 and LiOH are mixed? *Write a balanced equation for the reaction. (c) Will a precipitate form when solutions of Ba(NO 3 ) 2 and KOH are mixed? © 2009, Prentice-Hall, Inc.

16. Solution Chemistry It is helpful to pay attention to exactly what species are present in a reaction mixture (i.e., solid, liquid, gas, aqueous solution). If we are to understand reactivity, we must be aware of just what is changing during the course of a reaction.

17. © 2009, Prentice-Hall, Inc. Molecular Equation The molecular equation lists the reactants and products in their molecular form. AgNO 3 (aq) + KCl (aq)  AgCl (s) + KNO 3 (aq)

18. © 2009, Prentice-Hall, Inc. Ionic Equation In the ionic equation all strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions. This more accurately reflects the species that are found in the reaction mixture. Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq)  AgCl (s) + K + (aq) + NO 3 - (aq)

19. © 2009, Prentice-Hall, Inc. Net Ionic Equation To form the net ionic equation, cross out anything that does not change from the left side of the equation to the right. Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq)  AgCl (s) + K + (aq) + NO 3 - (aq)

20. © 2009, Prentice-Hall, Inc. Net Ionic Equation To form the net ionic equation, cross out anything that does not change from the left side of the equation to the right. The only things left in the equation are those things that change (i.e., react) during the course of the reaction. Ag + (aq) + Cl - (aq)  AgCl (s)

21. © 2009, Prentice-Hall, Inc. Net Ionic Equation To form the net ionic equation, cross out anything that does not change from the left side of the equation to the right. The only things left in the equation are those things that change (i.e., react) during the course of the reaction. Those things that didn’t change (and were deleted from the net ionic equation) are called spectator ions. Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq)  AgCl (s) + K + (aq) + NO 3 - (aq)

22. © 2009, Prentice-Hall, Inc. Writing Net Ionic Equations 1.Write a balanced molecular equation. 2.Dissociate all strong electrolytes. 3.Cross out anything that remains unchanged from the left side to the right side of the equation. 4.Write the net ionic equation with the species that remain.

23. Writing a Net Ionic Equation Write the net ionic equation for the precipitation reaction that occurs when solutions of calcium chloride and sodium carbonate are mixed. Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of silver nitrate and potassium phosphate are mixed. © 2009, Prentice-Hall, Inc.

24. Acids Arrhenius defined acids as substances that increase the concentration of H + when dissolved in water. Brønsted and Lowry defined them as proton donors.

25. © 2009, Prentice-Hall, Inc. Acids There are only seven strong acids: Hydrochloric (HCl) Hydrobromic (HBr) Hydroiodic (HI) Nitric (HNO 3 ) Sulfuric (H 2 SO 4 ) Chloric (HClO 3 ) Perchloric (HClO 4 )

26. © 2009, Prentice-Hall, Inc. Bases Arrhenius defined bases as substances that increase the concentration of OH − when dissolved in water. Brønsted and Lowry defined them as proton acceptors.

27. © 2009, Prentice-Hall, Inc. Bases The strong bases are the soluble metal salts of hydroxide ion: Alkali metals Calcium Strontium Barium

28. © 2009, Prentice-Hall, Inc. Acid-Base Reactions In an acid-base reaction, the acid donates a proton (H + ) to the base.

29. Comparing Acid Strengths Imagine a diagram showing 10 Na + ions and 10 OH – ions. If this solution were mixed with the one pictured above for HY, what would the diagram look like that represents the solution after any possible reaction? ( H + ions will react with ions to form H 2 O.) © 2009, Prentice-Hall, Inc. The following diagrams represent aqueous solutions of three acids (HX, HY, and HZ) with water molecules omitted for clarity. Rank them from strongest to weakest.

30. Consider solutions in which 0.1 mol of each of the following compounds is dissolved in 1 L of water: Ca(NO 3 ) 2 (calcium nitrate), C 6 H 12 O 6 (glucose), CH 3 COONa (sodium acetate), and CH 3 COOH (acetic acid). Rank the solutions in order of increasing electrical conductivity, based on the fact that the greater the number of ions in solution, the greater the conductivity. © 2009, Prentice-Hall, Inc.

31. Neutralization Reactions Generally, when solutions of an acid and a base are combined, the products are a salt and water. CH 3 COOH (aq) + NaOH (aq)  CH 3 COONa (aq) + H 2 O (l)

32. © 2009, Prentice-Hall, Inc. Neutralization Reactions When a strong acid reacts with a strong base, the net ionic equation is… HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l)

33. © 2009, Prentice-Hall, Inc. Neutralization Reactions When a strong acid reacts with a strong base, the net ionic equation is… HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l) H + ( aq ) + Cl - ( aq ) + Na + ( aq ) + OH - ( aq )  Na + ( aq ) + Cl - ( aq ) + H 2 O ( l )

34. © 2009, Prentice-Hall, Inc. Neutralization Reactions When a strong acid reacts with a strong base, the net ionic equation is… HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l) H + ( aq ) + Cl - ( aq ) + Na + ( aq ) + OH - ( aq )  Na + ( aq ) + Cl - ( aq ) + H 2 O ( l ) H + (aq) + OH - (aq)  H 2 O (l)

35. Writing Chemical Equations for a Neutralization Reaction (a)Write a balanced molecular equation for the reaction between aqueous solutions of acetic acid (CH 3 COOH) and barium hydroxide, Ba(OH) 2. (b)Write the net ionic equation for this reaction. (a)Write a balanced molecular equation for the reaction of carbonic acid (H 2 CO 3 ) and potassium hydroxide (KOH). (b) Write the net ionic equation for this reaction. © 2009, Prentice-Hall, Inc.

36. Gas-Forming Reactions Some metathesis reactions do not give the product expected. In this reaction, the expected product (H 2 CO 3 ) decomposes to give a gaseous product (CO 2 ). CaCO 3 (s) + HCl (aq)  CaCl 2 (aq) + CO 2 (g) + H 2 O (l)

37. © 2009, Prentice-Hall, Inc. Gas-Forming Reactions When a carbonate or bicarbonate reacts with an acid, the products are a salt, carbon dioxide, and water. CaCO 3 (s) + HCl (aq)  CaCl 2 (aq) + CO 2 (g) + H 2 O (l) NaHCO 3 (aq) + HBr (aq)  NaBr (aq) + CO 2 (g) + H 2 O (l)

38. © 2009, Prentice-Hall, Inc. Gas-Forming Reactions Similarly, when a sulfite reacts with an acid, the products are a salt, sulfur dioxide, and water. SrSO 3 (s) + 2 HI (aq)  SrI 2 (aq) + SO 2 (g) + H 2 O (l)

39. © 2009, Prentice-Hall, Inc. Gas-Forming Reactions This reaction gives the predicted product, but you had better carry it out in the hood, or you will be very unpopular! But just as in the previous examples, a gas is formed as a product of this reaction. Na 2 S (aq) + H 2 SO 4 (aq)  Na 2 SO 4 (aq) + H 2 S (g)

40. © 2009, Prentice-Hall, Inc. Oxidation-Reduction Reactions An oxidation occurs when an atom or ion loses electrons. A reduction occurs when an atom or ion gains electrons. One cannot occur without the other.

41. © 2009, Prentice-Hall, Inc. Oxidation Numbers To determine if an oxidation-reduction reaction has occurred, we assign an oxidation number to each element in a neutral compound or charged entity.

42. © 2009, Prentice-Hall, Inc. Oxidation Numbers Elements in their elemental form have an oxidation number of 0. The oxidation number of a monatomic ion is the same as its charge.

43. © 2009, Prentice-Hall, Inc. Oxidation Numbers Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions.  Oxygen has an oxidation number of −2, except in the peroxide ion in which it has an oxidation number of −1.  Hydrogen is −1 when bonded to a metal, +1 when bonded to a nonmetal.

44. © 2009, Prentice-Hall, Inc. Oxidation Numbers Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions.  Fluorine always has an oxidation number of −1.  The other halogens have an oxidation number of −1 when they are negative; they can have positive oxidation numbers, however, most notably in oxyanions.

45. © 2009, Prentice-Hall, Inc. Oxidation Numbers The sum of the oxidation numbers in a neutral compound is 0. The sum of the oxidation numbers in a polyatomic ion is the charge on the ion.

46. Determining Oxidation Numbers Determine the oxidation number of sulfur in each of the following: (a) H 2 S, (b) S 8, (c) SCl 2, (d) Na 2 SO 3, (e) SO 4 2–. What is the oxidation state of the boldfaced element in each of the following: (a) P 2 O 5, (b) NaH, (c) Cr 2 O 7 2–, (d) SnBr 4, (e) BaO 2 ? © 2009, Prentice-Hall, Inc.

47. Displacement Reactions In displacement reactions, ions oxidize an element. The ions, then, are reduced.

48. © 2009, Prentice-Hall, Inc. Displacement Reactions In this reaction, silver ions oxidize copper metal. Cu (s) + 2 Ag + (aq)  Cu 2+ (aq) + 2 Ag (s)

49. © 2009, Prentice-Hall, Inc. Displacement Reactions The reverse reaction, however, does not occur. Cu 2+ (aq) + 2 Ag (s)  Cu (s) + 2 Ag + (aq) x

50. © 2009, Prentice-Hall, Inc. Activity Series

51. Writing Molecular and Net Ionic Equations for Oxidation-Reduction Reactions Write the balanced molecular and net ionic equations for the reaction of aluminum with hydrobromic acid. Write the balanced molecular and net ionic equations for the reaction between magnesium and cobalt(II) sulfate. – What is oxidized and what is reduced in the reaction? Will an aqueous solution of iron(II) chloride oxidize magnesium metal? If so, write the balanced molecular and net ionic equations for the reaction. Which of the following metals will be oxidized by Pb(NO 3 ) 2 : Zn, Cu, Fe? © 2009, Prentice-Hall, Inc.

52. Molarity Two solutions can contain the same compounds but be quite different because the proportions of those compounds are different. Molarity is one way to measure the concentration of a solution. moles of solute volume of solution in liters Molarity (M) =

53. Calculating Molarity Calculate the molarity of a solution made by dissolving 23.4 g of sodium sulfate (Na 2 SO 4 ) in enough water to form 125 mL of solution. How many grams of Na 2 SO 4 are required to make 0.350 L of 0.500 M Na 2 SO 4 How many grams of Na 2 SO 4 are there in 15 mL of 0.50 M Na 2 SO 4 ? How many milliliters of 0.50 M Na 2 SO 4 solution are needed to provide 0.038 mol of this salt? What are the molar concentrations of each of the ions present in a 0.025 M aqueous solution of calcium nitrate? © 2009, Prentice-Hall, Inc.

54. Mixing a Solution To create a solution of a known molarity, one weighs out a known mass (and, therefore, number of moles) of the solute. The solute is added to a volumetric flask, and solvent is added to the line on the neck of the flask.

55. © 2009, Prentice-Hall, Inc. Dilution One can also dilute a more concentrated solution by –Using a pipet to deliver a volume of the solution to a new volumetric flask, and –Adding solvent to the line on the neck of the new flask.

56. © 2009, Prentice-Hall, Inc. Dilution The molarity of the new solution can be determined from the equation M c  V c = M d  V d, where M c and M d are the molarity of the concentrated and dilute solutions, respectively, and V c and V d are the volumes of the two solutions.

57. © 2009, Prentice-Hall, Inc. Using Molarities in Stoichiometric Calculations

58. Preparing A solution by Dilution 1. How many milliliters of 3.0 M H 2 SO 4 are needed to make 450 mL of 0.10 M H 2 SO 4 ? 2. What volume of 2.50 M lead(II) nitrate solution contains 0.0500 mol of Pb 2+ ? 3. How many milliliters of 5.0 M K 2 Cr 2 O 7 solution must be diluted to prepare 250 mL of 0.10 M solution? 4. If 10.0 mL of a 10.0 M stock solution of NaOH is diluted to 250 mL, what is the concentration of the resulting stock solution? © 2009, Prentice-Hall, Inc.

59. Titration Titration is an analytical technique in which one can calculate the concentration of a solute in a solution.

60. Using Mass Relations In a Neutralization Reaction 1.How many grams of Ca(OH) 2 are needed to neutralize 25.0 mL of 0.100 M HNO 3 ? 2. How many grams of NaOH are needed to neutralize 20.0 mL of 0.150 M H 2 SO 4 solution? 3.How many liters of 0.500 M HCl(aq) are needed to react completely with 0.100 mol of Pb(NO 3 ) 2 (aq), forming a precipitate of PbCl 2 (s)? © 2009, Prentice-Hall, Inc.

61. Determining the Quality of Solute by Titration 1. The quantity of Cl – in a municipal water supply is determined by titrating the sample with Ag +. The reaction taking place during the titration is The end point in this type of titration is marked by a change in color of a special type of indicator. (a) How many grams of chloride ion are in a sample of the water if 20.2 mL of 0.100 M Ag + is needed to react with all the chloride in the sample? (b) If the sample has a mass of 10.0 g, what percent Cl – does it contain? 2. A sample of an iron ore is dissolved in acid, and the iron is converted to Fe 2+. The sample is then titrated with 47.20 mL of 0.02240 M MnO 4 – solution. The oxidation-reduction reaction that occurs during titration is as follows: (a) How many moles of MnO 4 – were added to the solution? (b) How many moles of Fe 2+ were in the sample? (c) How many grams of iron were in the sample? (d) If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? © 2009, Prentice-Hall, Inc.

62. One more! 3. One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concentration of NaOH is normally in the range of 3 to 6 M. The NaOH is analyzed periodically. In one such analysis, 45.7 mL of 0.500 M H 2 SO 4 is required to neutralize a 20.0-mL sample of NaOH solution. What is the concentration of the NaOH solution? © 2009, Prentice-Hall, Inc.