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Ch4 – Types of Chemical Reaction and Solutions Ch4.1 – 4.3 Water, Electrolytes, and Concentration

Ch4 – Types of Chemical Reaction and Solutions Ch4.1 – 4.3 Water, Electrolytes, and Concentration. This is the process of hydration. Dissociation equation: NaCl (s) H2O Na + (aq) + Cl – (ag) Solubility varies greatly. For ions - depends on who has the greater attraction.

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Ch4 – Types of Chemical Reaction and Solutions Ch4.1 – 4.3 Water, Electrolytes, and Concentration

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  1. Ch4 – Types of Chemical Reaction and Solutions Ch4.1 – 4.3 Water, Electrolytes, and Concentration

  2. This is the process of hydration. Dissociation equation: NaCl(s)H2O Na+(aq) + Cl–(ag) Solubility varies greatly. For ions - depends on who has the greater attraction. For molecules – depends on polarity Solvent – the substance doing the dissolving (water) Solute – the substance that gets dissolved (salt)

  3. Electrolytes Strong electrolytes - conduct current very efficiently - soluble salts, acids, bases

  4. Electrolytes Strong electrolytes - conduct current very efficiently - soluble salts, acids, bases Arrhenius Theory of Acids - produces H+ ions (protons) in water HCl H2O H+(aq) + Cl–(aq) - strong acid – vitrually every H ionizes H2SO4H2O H+(aq) + HSO4–(aq)

  5. Weak electrolytes – only a small degree of ionization Weak Acid Weak Base HC2H3O2H2O H+(aq) + C2H3O2–(aq) NH3H2O NH4+(aq) + OH–(aq) Only about 1 in 100 H’s ionize. The rest stay in their molecules. Nonelectrolytes – dissolve in water, but don’t produce ions. - like sugar

  6. Molarity Units: Molar or M Ex1) Calc the molarity of a solution prepared by dissolving 11.5g NaOH in enough water to make 1.50L soln.

  7. Concentration of Ions Ex2) Give the concentration of ions in a 0.50M Co(NO3)2soln.

  8. Ex3) Calculate the number of moles of Cl– ions in 1.75L of 1.0x10-3M ZnCl2soln. Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)

  9. Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b) 11. Show how each of the following strong electrolytes “ breaks up” into its component ions dissolving in water. d. (NH4)2SO4 e. HI f. FeSO4 g. KMnO4 h. HClO4 13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.

  10. Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b) 11. Show how each of the following strong electrolytes “ breaks up” into its component ions dissolving in water. d. (NH4)2SO4H2O 2NH4+ + SO4-2 e. HI H2O H+ + I- f. FeSO4 H2O Fe+ + SO4- g. KMnO4 H2O K+ + MnO4- h. HClO4 H2O H+ + ClO4- 13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.

  11. Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b) 11. Show how each of the following strong electrolytes “ breaks up” into its component ions dissolving in water. d. (NH4)2SO4H2O 2NH4+ + SO4-2 e. HI H2O H+ + I- f. FeSO4 H2O Fe+ + SO4- g. KMnO4 H2O K+ + MnO4- h. HClO4 H2O H+ + ClO4- 13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water. CaCl2 H2O Ca2+ + 2Cl-

  12. 15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water to make 250 ml of solution. b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.

  13. 15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water to make 250 ml of solution. b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.

  14. 15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water to make 250 ml of solution. b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.

  15. 17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte a. 0.15M CaCl2 b. 0.26M Al(NO3)3

  16. 17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte a. 0.15M CaCl2 0.15M Ca+ ions 0.30MCl- ions b. 0.26M Al(NO3)3

  17. 17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte • a. 0.15M CaCl2 • 0.15M Ca+ ions • 0.30MCl- ions • b. 0.26M Al(NO3)3 • 0.26M Al+3 ions • 0.78M NO3- ions

  18. Ch4.3 More Concentration Calculations Ex1) Blood serum is 0.14M NaCl. What volume of blood contains 1.0mg NaCl?

  19. Ex2) How would I prepare 500 mls of a 0.100M ______ solution, given solid solute?

  20. Dilutions Ex3) How would I prepare 500 mls of a 0.100M H2SO4 solution, given concentrated stock solution of 18M? Ch4 HW#2 p181 21,23(a,b),25

  21. Ch4 HW#2 p181 21,23(a,b),25 21. What volume of a 0.100 M solution of NaHCO3 contains 0.350 g of NaHCO3?

  22. Ch4 HW#2 p181 21,23(a,b),25 21. What volume of a 0.100 M solution of NaHCO3 contains 0.350 g of NaHCO3?

  23. 23. Describe how you would prepare 2.00 L of each of the following solutions. a. 0.250MNaOH from solid NaOH b. 0.250MNaOH from 1.00M NaOH stock solution

  24. 23. Describe how you would prepare 2.00 L of each of the following solutions. a. 0.250MNaOH from solid NaOH b. 0.250MNaOH from 1.00M NaOH stock solution

  25. 23. Describe how you would prepare 2.00 L of each of the following solutions. a. 0.250MNaOH from solid NaOH b. 0.250MNaOH from 1.00M NaOH stock solution b. M1.V1 = M2.V2

  26. 25. A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 200.0 mL of stock solution. A 10.0 mL sample of this stock solution is added to 50.0 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

  27. 25. A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 200.0 mL of stock solution. A 10.0 mL sample of this stock solution is added to 50.0 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

  28. Ch4.4 – 4.6 Types of Solution Reactions 1. Precipitation Reactions 2. Acid-base Reactions 3. Oxidation-Reduction Reactions (Redox)

  29. Ch4.4 – 4.6 Types of Solution Reactions 1. Precipitation Reactions solns mixed and an insoluble substance forms, and separates, called a precipitate. AgNO3(aq) and NaCl(ag)

  30. 1. Precipitation Reactions solns mixed and an insoluble substance forms, and separates, called a precipitate. K2CrO4(aq) + Ba(NO3)2(aq)

  31. Simple solubility rules for salts in water: 1. Most nitrates NO3-1 are soluble. 2. Most salts of alkali metals (Li+, Na+, K+, Cs+, Rb+) are soluble. Same for ammonium, NH4+ . 3. Most chloride, bromide, and iodide salts are soluble, but not when with Ag+, Pb2+, Hg22+. 4. Most sulfates are soluble, except BaSO4, PbSO4, Hg2SO4, CaSO4. 5. Most hydroxides are only slightly soluble, except NaOH and KOH very soluble. Ba(OH)2, Ca(OH)2, Sr(OH)2only slightly soluble. 6. Most sulfides (S2–), carbonates (CO32–), phosphates (PO43–), and chromtes (CrO42–) are only slightly soluble.

  32. Ex1) Use rules to predict what will happen if following solutions are mixed: a) KNO3(aq) and BaCl2(aq) b) Na2SO4(aq) and Pb(NO3)2(aq) c) KOH(aq) and Fe(NO3)3(aq)

  33. 3 types of equations are used to describe reactions in solution: 1. molecular eqn – great for doing stoichiometry. 2. complete ionic eqn – all ions listed, great for seeing strong electrolytes. 3. net ionic eqn – only those soln components that undergo change. Spectators not included. Ex2) Aqueous potassium hydroxide is mixed with aqueous iron(III) nitrate to form a ppt of iron(III) hydroxide and aqueous potassium nitrate. Write all 3 eqns. Ch4 HW#3 p181+ 29,31,33,35(a,b)

  34. Ch4 HW#3 p181+ 29,31,33,35(a,b) 29. When the following solutions are mixed together, what precipitation (if any) will form? a. BaCl2(aq) + Na2SO4(aq) b. Pb(NO3)2(aq) + KCl(aq) c. AgNO3(aq) + Na3PO4(aq) d. NaOH(aq) + Fe(NO3)3(aq) 31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”

  35. Ch4 HW#3 p181+ 29,31,33,35(a,b) 29. When the following solutions are mixed together, what precipitation (if any) will form? a. BaCl2(aq) + Na2SO4(aq) BaSO4(s) b. Pb(NO3)2(aq) + KCl(aq) PbCl2(c) c. AgNO3(aq) + Na3PO4(aq) Ag3PO4(s) d. NaOH(aq) + Fe(NO3)3(aq) Fe(OH)3(s) 31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”

  36. Ch4 HW#3 p181+ 29,31,33,35(a,b) • 29. When the following solutions are mixed together, • what precipitation (if any) will form? • NIE:a. BaCl2(aq) + Na2SO4(aq) BaSO4(s) • NIE: b. Pb(NO3)2(aq) + KCl(aq) PbCl2(c) • NIE: c. AgNO3(aq) + Na3PO4(aq) Ag3PO4(s) • NIE: d. NaOH(aq) + Fe(NO3)3(aq) Fe(OH)3(s) • 31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. • If no precipitate forms, write “No reaction.” • BME: • a. BaCl2(aq) + Na2SO4(aq) 2Cl-(aq)+2Na+(aq)+ BaSO4(s) • b. Pb(NO3)2(aq) + 2KCl(aq) 2NO3-(aq)+2K+(aq)+ PbCl2(c) • c. 3AgNO3(aq)+Na3PO4(aq) 3NO3-(aq)+3Na+(aq)+Ag3PO4(s) • d. 3NaOH(aq)+Fe(NO3)3(aq) 3NO3-(aq)+3Na+(aq)+ Fe(OH)3(s)

  37. 33. Write net ionic equations for each of the following. a. AgNO3(aq) + KI(aq) b. CuSO4(aq) + Na2S(aq) c. CoCl2(aq)+ NaOH(aq) d. NiCI2(aq) + KNO3(aq)

  38. 33. Write net ionic equations for each of the following. a. AgNO3(aq) + KI(aq) Ag+(aq) + I-(aq)AgI(s) b. CuSO4(aq) + Na2S(aq) Cu2+(aq) + S2-(aq) CuS(s) (only slightly) c. CoCl2(aq)+ NaOH(aq) Co2+(aq)+ 2OH-(aq) Co(OH)2(aq)(only slightly) d. NiCI2(aq) + KNO3(aq) No ppt

  39. 35. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. Ammonium sulfate and barium nitrate (NH4)2(SO4)(aq) + Ba(NO3)2(aq)  b. Lead(II) nitrate and sodium chloride Pb(NO3)2(aq) + NaCl(aq) 

  40. 35. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. Ammonium sulfate and barium nitrate SO42-(aq) + Ba2+(aq)  BaSO4(s) b. Lead(II) nitrate and sodium chloride Pb+2(aq) + 2Cl-(aq)  PbCl2(s)

  41. Ch4.7 Mass of Precipitate Ex1) Calculate the mass of solid NaCl that must be added to 1.50L of a 0.100M AgNO3 solution to precipitate all the Ag+ ions.

  42. Ex2) What mass of PbSO4 precipitates when 2.00L of 0.025M aqueous Na2SO4 and 1.25L of 0.0500M aqueous Pb(NO3)2 are mixed? Ch4 HW#4 p182 39,41,43

  43. Ch4 HW#4 p182 39,41,43 39. What mass of NaCl is required to precipitate all the silver ions from 50.0 mL of a 0.0500 M solution of AgNO3? NaCl + AgNO3 ?g0.0500M 50.0ml

  44. Ch4 HW#4 p182 39,41,43 39. What mass of NaCl is required to precipitate all the silver ions from 50.0 mL of a 0.0500 M solution of AgNO3? NaCl + AgNO3 ?g0.0500M 50.0ml Cl- + Ag+ AgCl(s)

  45. 41. What mass of solid aluminum hydroxide is produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100M KOH? Al(NO3)3 + 3KOH  K+(aq) + NO3-(aq) + Al(OH)3(s) 0.200M 0.100M ?g 50.0ml 200.0ml Al is L.R. x 3 = 0.06 mol

  46. 41. Al(NO3)3 + 3KOH  K+(aq) + NO3-(aq) + Al(OH)3(s) 0.200M 0.100M ?g 50.0ml 200.0ml Al is L.R. x 3 = 0.06 mol

  47. 43. A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.

  48. 43. A 100.0mL aliquot of 0.200 M aqueous potassium hydroxide is mixed • with 100.0 mL of 0.200 M aqueous magnesium nitrate. • a. Write a balanced chemical equation for any reaction that occurs. • b. What precipitate forms? • c. What mass of precipitate is produced? • d. Calculate the concentration of each ion remaining in solution after precipitation is complete. • 2KOH + Mg(NO3)2 2K+ + 2NO3- + Mg2+ + 2OH- • 2KOH + Mg(NO3)2 Mg(OH)2(s) • 0.200M 0.200M • 100ml 100ml • LR

  49. Ch4.8 – Acid-Base Reactions Bronsted-Lowry Theory of acids and bases: Acid – proton donor Base – proton acceptor HCl(aq) + NaOH(aq) HC2H3O2(aq) + KOH(aq) 

  50. Ex1) What volume of a 0.100M HCl solution is needed to neutralize 25.0mL of 0.350M NaOH? HCl(aq) + NaOH(aq)

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