1 / 330

Acid- base Theory

Acid- base Theory. Applied to aqueous solutions only. Acids : Substances that produce hydrogen ions, H + (aq) when dissolved in water. . 1. Arrhenius (1880s) : -. E.g. HCl. Bases : Substances that produce hydroxide ions, OH  (aq) when dissolved in water. . E.g. NaOH.

drago
Download Presentation

Acid- base Theory

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Acid-baseTheory Applied to aqueous solutions only Acids : Substances that produce hydrogen ions, H+(aq) when dissolved in water. 1. Arrhenius (1880s) : - E.g. HCl Bases : Substances that produce hydroxide ions, OH(aq) when dissolved in water. E.g. NaOH

  2. 2. Brnsted / Lowry (1923) : - Applied to aqueous and non-aqueous solutions Acids : Proton donors E.g. Molecule – HCl, H2O, CH3COOH Cation – H3O+, NH4+ Anion – HSO4-

  3. Bases: Proton acceptors e.g. Molecule - H2O, NH3 Anion - Cl, OH, CH3COO, SO42 Each contains at least one lone pair to form a dative bond with a proton (H+)

  4. 3. Lewis (1930s) : - More widely applied to systems with and without solvents Acids : electron pair acceptors, e.g. H+, BF3, AlCl3, BeCl2 (electron-deficient species)

  5. H+(aq) + OH(aq)  BF3 + NH3 Lewis acids Lewis bases Bases: electron pair donors e.g. NH3, OH species containing lone pair(s)

  6. HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) Loss of H+ A conjugate acid-base pair is a pair of species that can be inter-converted by transfer of proton. acid Conjugate base

  7. Gain of H+ HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) A conjugate acid-base pair is a pair of species that can be inter-converted by transfer of proton. Conjugate acid base

  8. Gain of H+ HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) A conjugate acid-base pair is a pair of species that can be inter-converted by transfer of proton. base Conjugate acid

  9. Loss of H+ HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) A conjugate acid-base pair is a pair of species that can be inter-converted by transfer of proton. Conjugate base Acid An acid-base equilibrium system consists of TWO inter-convertible conjugate acid-base pairs.

  10. Acid Base Conjugate base Conjugate acid HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) H2O(l) + NH3(aq) OH(aq) + NH4+(aq) A species can behave as an acid or a base depending on the situation.

  11. H2SO4(aq) NH4+(aq) H2O(l) HSO4(aq) SO42(aq) NH2(aq) NH3(aq) OH(aq) O2(aq) 1. Give the conjugate acid and conjugate base of each of the following species

  12. HCl(aq) + H2O(l)Cl(aq) +H3O+(aq) H2O(l) + NH3(aq)OH(aq) + NH4+(aq) CH3COOH(aq) + H2O(l)CH3COO(aq) + H3O+(aq) H2O(l) + H2O(l)OH(aq) + H3O+(aq) HSO4(aq) + H2O(l)SO42(aq) + H3O+(aq) Concept of Conjugate Acid-base Pairs Acid Base Conjugate base Conjugate acid

  13. stronger + stronger weaker + weaker acid base conjugate conjugate base acid Relative Strengths of Conjugate Acid-base Pairs Stronger acid/base produces weaker conjugate base/acid more completely. The forward reaction is more complete. The equilibrium position lies to the right.

  14. weaker + weaker stronger + stronger acid base conjugate conjugate base acid Relative Strengths of Conjugate Acid-base Pairs Weaker acid/base produces stronger conjugate base/acid less completely. The forward reaction is less complete. The equilibrium position lies to the left.

  15. Relative strength Relative strength Acid Conjugate base

  16. HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) stronger acid stronger base weaker base weaker acid For a strong acid The equilibrium position lies far to the right. Strong acids at the top left of Table 1 almost ionize completely to give H3O+(aq) ,

  17. HCl(aq) + H2O(l) Cl(aq) + H3O+(aq) stronger acid stronger base weaker base weaker acid For a strong acid ∴ the strongest acid present in aqueous solutions is hydronium ions, H3O+(aq)

  18. CH3COOH(aq) + H2O(l) CH3COO(aq) + H3O+(aq) weaker acid weaker base stronger base stronger acid For a weak acid The equilibrium position lies far to the left.

  19. CH3(aq) + H2O(l) CH4(aq) + OH-(aq) Stronger base stronger acid weaker acid weaker base For a strong base The equilibrium position lies far to the right. Strong bases at the bottom right of Table 1 react almost completely with water to give OH(aq),

  20. CH3(aq) + H2O(l) CH4(aq) + H3O+(aq) weaker acid weaker base stronger base stronger acid For a strong base ∴ the strongest base present in aqueous solutions is hydroxide ions, OH(aq).

  21. HSO4(aq) + H2O(l) H2SO4(aq) + OH(aq) weaker base weaker acid stronger acid stronger base For a weak base The equilibrium position lies far to the left.

  22. Formation of hydronium ion

  23. H Lone pair + N H Empty 1s orbital H H + H Ammonium ion N H H H Formation of ammonium ion

  24. Hydrated Hydronium ion, H3O+(H2O)20

  25. pH and Its Calculation Definition : pH is the negative power of the molarity of Hydronium ion

  26. H2O(l) + H2O(l) H3O+(aq) + OH(aq) Self-ionization of Water ∵ [H2O(l)]  55.5 M It is in large excess  treated as a constant  Kc[H2O(l)]2 = Kw = [H3O+(aq)][OH(aq)]

  27. ionic product of water Temperature dependent Kw = [H3O+(aq)][OH(aq)] At 298 K

  28. In neutral solution, [H3O+(aq)] = [OH(aq)] ∴ pH = log10(1.00107) = 7.00

  29. In acidic solution, [H3O+(aq)] > [OH(aq)]  [H3O+(aq)] > 1.00107 mol dm3 pH < 7.00

  30. In alkaline solution, [H3O+(aq)] < [OH(aq)]  [H3O+(aq)] < 1.00107 mol dm3 pH > 7.00

  31. Temp/oC 18.0 25.0 40.0 75.0 Kw / mol2 dm6 0.610 1014 1.00 1014 2.92 1014 16.9 1014 Q.2 Given the following Kw values at different temperatures,

  32. Temp/oC 18.0 25.0 40.0 75.0 Kw / mol2 dm6 0.610 1014 1.00 1014 2.92 1014 16.9 1014 (a) An increase in T increases the value of Kw  the equilibrium position shifts to the right  the system absorbs heat by shifting to the right  the forward reaction is endothermic

  33. 2.(b) In neutral solution, [H3O+(aq)] = [OH(aq)] pH = log10(1.71107) = 6.77

  34. Example 1 Calculate the pH of (a) 0.200 M HCl and (b) 0.200 M KOH at 298 K Given : Kw at 298 K = 1.001014 mol2 dm6 • Assumptions : • (i) HCl ionizes completely when dissolved in water. • (ii) [H3O+(aq)] from H2O(l) is negligible. ∵ [HCl(aq)] = 0.200 M ∴ [H3O+(aq)] = 0.200 M assumption (i) pH = log10[H3O+(aq)] = log100.200 assumption (ii) = 0.699

  35. assumption (ii) (b) Assumptions : (i) KOH dissociates completely when dissolved in water. (ii) [OH(aq)] from H2O(l) is negligible. ∵ [KOH(aq)] = 0.200 M ∴ [OH(aq)] = 0.200 M assumption (i) At 298 K pH = log10(5.001014) = 13.3

  36. = 1.001014 mol2 dm6 Alternatively, log10[H3O+(aq)][OH(aq)] = 14.0 log10[H3O+(aq)] + (log10[OH(aq)]) = 14.0 pH + pOH = 14.0 (at 298 K) pH = 14.0 – pOH = 14.0 – (log100.200) = 14.0 – (0.699) = 13.3

  37. Relationships of [H3O+(aq)] and [OH(aq)] at 298 K

  38. Q.3 Calculate the pH values of the following solutions at 298 K. Given : Kw at 298 K = 1.001014 mol2 dm6 (a) Assumptions : (i) HCl ionizes completely when dissolved in water. (ii) [H3O+(aq)] from H2O(l) is negligible. [H3O+(aq)] = [HCl(aq)] = 2.00 M pH = log102.00 = 0.301

  39. (b) Assumptions : (i) NaOH dissociates completely when dissolved in H2O. (ii) [OH(aq)] from H2O(l) is negligible. [OH(aq)] = [NaOH(aq)] = 2.00 M pH = log10(5.0010-15) = 14.3 pH values can be > 14 or < 0

  40. 2H2O(l) OH(aq) + H3O+(aq) (c) [H3O+(aq)] from H2O should be considered 1.0010-7 1.0010-7 1.0010-7 1.0010-7 + 1.0010-9 (1.0010-7 – x) (1.0010-7 + 1.0010-9 – x) Kw = (1.0010-7 – x)(1.0010-7 + 1.0010-9 – x)= 1.0010-14 x = 5.0010-10 M or 2.0010-7 M(rejected) [H3O+(aq)] = (1.0110-7  5.0010-10) = 1.005107 M  pH = 6.997 < 7 (acidic)

  41. At very low acid / base concentrations (<106 M), the [H3O+(aq)] / [OH(aq)] from H2O(l) cannot be ignored. At very high acid / base concentrations (>6 M), the ionization of strong acids / bases is no longer complete.

  42. [H3O+] = 1106 M Variation of [H3O+(aq)] with [HCl(aq)]

  43. [OH] = 1106 M Variation of [OH(aq)] with [NaOH(aq)]

  44. Measurement of pH TWO ways : - Universal indicator / pH paper pH meter

  45. Universal indicator / pH paper Universal indicator : - a mixture of dyeswhich shows different colours at different pH values. pH paper : - paper coated with universal indicator

  46. Procedures of using universal indicator Apply a few drops of universal indicator to the sample. Apply a few drops of sample to a piece of pH paper. This method gives only a rough estimation of the pH of the sample.

  47. A pH sensor (probe)

  48. pH meter Probe : A glass electrode coupled with a reference electrode Glass electrode : The electrode potential varies linearly with the pH of the solution in which it is immersed. At 298 K, The electrode potential is given by E1 = C – 0.0592pH, where C is a constant Reference electrode : An electrode with a fixed electrode potential, E2 E.g. Ag /AgCl electrode

More Related