1. CHEMISTRY 161 Reactions between Ions in Aqueous Solutions Chapter 5

2. CHEMICAL REACTIONS 2 HgO (s) → 2Hg (l) + O 2(g) aq 1. properties of aqueous solutions 2. reactions in aqueous solutions a) precipitation reactions b) acid-base reactions (proton transfer) c) redox reactions (electron transfer) (chapter 6)

3. 1. SOLUTION homogeneous mixture of two or more substances solvent solute substance in a large amount substance in a small amount N 2 gas phase O 2 (air) Ag solid phase Au (alloys) H 2 O liquid phase NaCl (sea water)

4. EXP1 iodine in ethyl alcohol (C 2 H 5 OH) EXP2 table salt in water (H 2 O) does not conduct electricity (molecular solid) I 2 does conduct electricity (ionic solid) Na + Cl - EXP3

5. AQUEOUS SOLUTION solutes solute water (H 2 O) electrolytesnon-electrolytes solution conducts electricity solution does not conduct electricity

6. electrolytesnon-electrolytes solution conducts electricity solution does not conduct electricity

7. non-electrolyte weak electrolyte strong electrolyte methanol sugar ethanol water darkbright ionic compounds (NaCl, KF) NaOH HCl H 2 SO 4 CH 3 COOH HCOOH HF medium

8. SOLUTION EXP4 concentration

9. SOLUTION percentage concentration % = g [solute] / 100 g solvent X 100 12 g of sodium chloride are solved in 150 g of water. Calculate the percentage concentration 8 %

10. solubility of a solute number of grams of solute that can dissolve in 100 grams of solvent at a given temperature SOLUTION 36.0 g NaCl can be dissolve in 100 g of water at 293 K

11. GAS PHASE SOLUTION Saturn solvent H 2 /He solute CH 4, PH 3

12. LIQUID SOLUTION Europa solvent H 2 O solute MgSO 4

13. SOLID SOLUTION Triton solvent N 2 solute CH 4

14. methanol sugar ethanol water ionic compounds (NaCl, KF) NaOH HCl H 2 SO 4 CH 3 COOH HCOOH HF ELECTROLYTES

15. migrating negative and positive charges Kohlrausch NaCl

16. DISSOCIATION ‘breaking apart’ NaCl (s) → Na + (aq) + Cl - (aq) NaOH (s) → Na + (aq) + OH - (aq) HCl (g) → H + (aq) + Cl - (aq) strong electrolytes are fully dissociated Ca(NO 3 ) 2 (s) → Ca 2+ (aq) + 2 NO 3 - (aq)

17. O HH δ-δ- δ+δ+ δ+δ+

18. SOLVATION cationsanions

19. SOLVATION non-electrolyte

20. CH 3 COOH (aq) H + (aq) + CH 3 COO - (aq) weak electrolytes are not fully dissociated reversible reaction (chemical equilibrium) → ← NaCl (s) → Na + (aq) + Cl - (aq) strong electrolytes are fully dissociated

21. CHEMICAL REACTIONS 1.properties of aqueous solutions 2. reactions in aqueous solutions a) precipitation reactions b) acid-base reactions (proton transfer) c) redox reactions (electron transfer) (chapter 6)

22. 2.1. PRECIPITATION REACTIONS solution 1solution 2 solution 1 + solution 2

23. 2.1. PRECIPITATION REACTIONS formation of an insoluble product (precipitate) NaCl(aq) + AgNO 3 (aq) AgCl(s) + NaNO 3 (aq) EXP5

24. insoluble compounds 1.M + compounds (M = H, Li, Na, K, Rb, Cs, NH 4 ) 2. A - compounds (A = NO 3, HCO 3, ClO 3, Cl, Br, I) (AgX, PbX 2 ) 3. SO 4 2- (Ag, Ca, Sr, Ba, Hg, Pb) 4. CO 3 2-, PO 4 3-, CrO 4 2-, S 2- (Ag, Ca, Sr, Ba, Hg, Pb)

25. NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq) balanced molecular equation (table to determine which compound precipitates)

26. balanced ionic equation 1. NaCl(s) → Na + (aq) + Cl - (aq) 2. AgNO 3 (s) → Ag + (aq) + NO 3 - (aq) 3. Na + (aq) + Cl - (aq) + Ag + (aq)+ NO 3 - (aq) → AgCl(s) + Na + (aq) + NO 3 - (aq) spectator ions

27. Ba(NO 3 ) 2 (aq) + Na 3 PO 4 (aq) 1.which compound falls out? 2. balanced molecular equation 3. balanced ionic equations 4. identify spectator ions Cs 2 CrO 4 (aq) + Pb(NO 3 ) 2 (aq) Ba(NO 3 ) 2 (aq) + Na 2 SO 4 (aq)

28. CHEMICAL REACTIONS 1.properties of aqueous solutions 2. reactions in aqueous solutions a) precipitation reactions b) acid-base reactions (proton transfer) c) redox reactions (electron transfer) (chapter 6)

29. ACIDS AND BASES Arrhenius (1883) ACIDS BASES NaOH (s) → Na + (aq) + OH - (aq) MOH → M + (aq) + OH - (aq) HCl (g) → H + (aq) + Cl - (aq) HAc → H + (aq) + Ac - (aq) ionization

30. IDENTIFICATION Litmus Paper acid base red blue Säure Base EXP2 and 3

31. ACIDS AND BASES ACIDS BASES HCl (aq) + NaOH (aq) → NaCl (aq) + H 2 O HAc (aq) + MOH (aq) → MAc (aq) + H 2 O and NEUTRALIZE EACH OTHER acid + base salt + water

32. H+H+ ≈ 10 -15 m Na+ ≈ 10 -10 m ACIDS AND BASES

33. HCl (g) → H + (aq) + Cl - (aq) H + (aq) + H 2 O H 3 O + (aq) HCl (g) + H 2 O → H 3 O + (aq) + Cl - (aq) one step hydronium ion

34. (aq)(l)(aq) hydronium ion acid base

35. cationhydronium ion

36. PROPERTIES OF ACIDS 1.acids have a sour taste vinegar – acetic acid lemons – citric acid 2. acids react with some metals to form hydrogen 2 HCl(aq) + Mg(s) → MgCl 2 (aq) + H 2 (g) 3. acids react with carbonates to water and carbon dioxide 2 HCl(aq) + CaCO 3 (s) → CaCl 2 (aq) + [H 2 CO 3 ] H 2 CO 3 → H 2 O(l) + CO 2 (g) EXP4 EXP5

37. BASES 1.bases have a bitter taste 2. bases feel slippery soap 3. aqueous bases and acids conduct electricity

38. EXAMPLES KOH(aq) and HF(aq) Mg(OH) 2 (aq) and HCl(aq) Ba(OH) 2 (aq) and H 2 SO 4 (aq) NaOH(aq) and H 3 PO 4 (aq) (stepwise)

39. Bronsted (1932) ACIDS HAc → H + (aq) + Ac - (aq) proton donors BASES proton acceptor B + H + (aq) → BH + (aq)

40. weak electrolyte CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO - (aq) NH 3 (aq) + H 2 O(l) NH 4 + + OH - strong electrolyte HCl(aq) + H 2 O(l) → H 3 O + (aq) + Cl - (aq) HNO 3 (aq) + H 2 O(l) → H 3 O + (aq) + NO 3 - (aq) donor versus acceptor

42. CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO - (aq) NH 3 (aq) + H 2 O(l) NH 4 + (aq)+ OH - (aq) H 2 O(l) + H 2 O(l) H 3 O + (aq) + OH - (aq) water can be either an acid or a base AUTO DISSOCIATION

43. monoprotic acids diprotic acid HF, HCl, HBr, HNO 3, CH 3 COOH H 2 SO 4 → H + (aq) + HSO 4 - (aq) HSO 4 - (aq) H + (aq) + SO 4 2- (aq) triprotic acid H 3 PO 4 H + (aq) + H 2 PO 4 - (aq) H 2 PO 4 - (aq) H + (aq) + HPO 4 2- (aq) HPO 4 2- (aq) H+(aq) + PO 4 3- (aq)

44. CHEMICAL PROPOERTIES 1. Non-metal oxides react with water to form an acid (acetic anhydrides) Cl 2 O 7, SO 2, Br 2 O 5 + H 2 O

45. CHEMICAL PROPOERTIES 2. Soluble metal oxides react with water to form a base (base anhydrides) MgO, Al 2 O 3 + H 2 O

46. NAMING ACIDS AND BASES prefix hydro- the suffix –ic to the stem of the nonmetal name followed by the word acid binary acids

47. NAMING ACIDS AND BASES oxo acids acids contain hydrogen, oxygen, plus another element main group 5 HNO 3 nitric acid HNO 2 nitrous acid H 3 PO 4 phosphoric acid H 3 PO 3 phosphorous acid

48. H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid main group 6 main group 7 HClO 4 perchloric acid HClO 3 chloric acid HClO 2 chlorous acid HClO hypochlorous acid

49. Acids in the Solar System Venus H 2 SO 4 (g) Europa H 2 SO 4 (s)

50. Acids in the Interstellar Medium

51. Orion NH 3, H 2 O, H 2 S CH 3 COOH HCOOH HF, HCl

52. STOCHIOMETRY (CONCENTRATION) molar concentration Molarity (M) =

53. How many grams of AgNO 3 are needed to prepare 250 mL of 0.0125 M AgNO 3 solution?

54. How many mL of 0.124 M NaOH are required to react completely with 15.4 mL of 0.108 M H2SO4? 2 NaOH + H 2 SO 4 Na 2 SO 4 + 2H 2 O

55. How many mL of 0.124 M NaOH are required to react completely with 20.1 mL of 0.2 M HCl? NaOH + HCl NaCl + H2O EXP6

56. EXP7 How many grams of iron(II)sulfide have to react with hydrochloric acid to generate 12 g of hydrogen sulfide?

57. How many moles of BaSO4 will form if 20.0 mL of 0.600 M BaCl2 is mixed with 30.0 mL of 0.500 M MgSO4? BaCl 2 + MgSO 4 BaSO 4 + MgCl 2 This is a limiting reagent problem

58. How many ml of a 1.5 M HCl will be used to neutralize a 0.2 M Ba(OH) 2 solution? How many ml of a 1.5 M HCl will be used to prepare 500 ml of a 0.1 M HCl? XX=