1 / 30

BUFFER SOLUTIONS A guide for A level students

BUFFER SOLUTIONS A guide for A level students. © 2004 JONATHAN HOPTON & KNOCKHARDY PUBLISHING. Buffer solutions. INTRODUCTION

lamar
Télécharger la présentation

BUFFER SOLUTIONS A guide for A level students

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. BUFFER SOLUTIONS A guide for A level students © 2004 JONATHAN HOPTON & KNOCKHARDY PUBLISHING

  2. Buffer solutions INTRODUCTION This Powerpoint show is one of several produced to help students understand selected topics at AS and A2 level Chemistry. It is based on the requirements of the AQA and OCR specifications but is suitable for other examination boards. Individual students may use the material at home for revision purposes or it may be used for classroom teaching if an interactive white board is available. Accompanying notes on this, and the full range of AS and A2 topics, are available from the KNOCKHARDY SCIENCE WEBSITE at... www.argonet.co.uk/users/hoptonj/sci.htm Navigation is achieved by... either clicking on the grey arrows at the foot of each page or using the left and right arrow keys on the keyboard

  3. Buffer solutions • CONTENTS • What is a buffer solution? • Uses of buffer solutions • Acidic buffer solutions • Alkaline buffer solutions • Buffer solutions - ideal concentration • Calculating the pH of a buffer solution • Salt hydrolysis • Check list

  4. Buffer solutions • Before you start it would be helpful to… • know that weak acids and bases are only partly ionised in solution • be able to calculate pH from hydrogen ion concentration • be able to construct an equation for the dissociation constant of a weak acid

  5. Buffer solutions - Briefintroduction Definition “Solutions which resist changes in pH when small quantities of acid or alkali are added.” Acidic Buffer (pH < 7) made from a weak acid + its sodium or potassium salt ethanoic acid sodium ethanoate Alkaline Buffer (pH > 7) made from a weak base + its chloride ammonia ammonium chloride Uses Standardising pH meters Buffering biological systems (eg in blood) Maintaining the pH of shampoos

  6. Buffer solutions - uses Definition “Solutions which resist changes in pH when small quantities of acid or alkali are added.” Biological Uses In biological systems (saliva, stomach, and blood) it is essential that the pH stays ‘constant’ in order for any processes to work properly. e.g. If the pH of blood varies by 0.5 it can lead to unconsciousness and coma Most enzymes work best at particular pH values. Other Uses Many household and cosmetic products need to control their pH values. Shampoo Buffer solutions counteract the alkalinity of the soap and prevent irritation Baby lotion Buffer solutions maintain a pH of about 6 to prevent bacteria multiplying Others Washing powder, eye drops, fizzy lemonade

  7. Acidic buffer solutions - action It is essential to have a weak acid for an equilibrium to be present so that ions can be removed and produced. The dissociation is small and there are few ions. CH3COOH(aq) CH3COO¯(aq) + H+(aq) relative concs. HIGH LOW LOW NB A strong acid can’t be used as it is fully dissociated and cannot remove H+(aq) HCl(aq) ——> Cl¯(aq) + H+(aq) Adding acid Any H+ is removed by reacting with CH3COO¯ ions to form CH3COOH via the equilibrium. Unfortunately, the concentration of CH3COO¯ is small and only a few H+ can be “mopped up”. A much larger concentration of CH3COO¯ is required. To build up the concentration of CH3COO¯ ions, sodium ethanoate is added.

  8. Acidic buffer solutions - action It is essential to have a weak acid for an equilibrium to be present so that ions can be removed and produced. The dissociation is small and there are few ions. CH3COOH(aq) CH3COO¯(aq) + H+(aq) relative concs. HIGH LOW LOW NB A strong acid can’t be used as it is fully dissociated and cannot remove H+(aq) HCl(aq) ——> Cl¯(aq) + H+(aq) Adding alkali This adds OH¯ ions which react with H+ ions H+(aq) + OH¯(aq) H2O(l) Removal of H+ from the weak acid equilibrium means that, according to Le Chatelier’s Principle, more CH3COOH will dissociate to form ions to replace those being removed. CH3COOH(aq) CH3COO¯(aq) + H+(aq) As the added OH¯ ions remove the H+ from the weak acid system, the equilibrium moves to the right to produce more H+ ions. Obviously, there must be a large concentration of undissociated acid molecules to be available.

  9. Alkaline buffer solutions - action Alkaline buffer Very similar but is based on the equilibrium surrounding a weak base; AMMONIA NH3(aq) + H2O(l) OH¯(aq) + NH4+(aq) relative concs. HIGH LOW LOW but one needs ; a large conc. of OH¯(aq) to react with any H+(aq) added a large conc of NH4+(aq) to react with any OH¯(aq) added There is enough NH3 to act as a source of OH¯ but one needs to increase the concentration of ammonium ions by adding an ammonium salt. Use AMMONIA (a weak base) + AMMONIUM CHLORIDE (one of its salts)

  10. Buffer solutions - ideal concentration The concentration of a buffer solution is also important If the concentration is too low, there won’t be enough CH3COOH and CH3COO¯ to cope with the ions added. Summary For an acidic buffer solution one needs ... large [CH3COOH(aq)] - for dissociating into H+(aq) when alkali is added large [CH3COO¯(aq)] - for removing H+(aq) as it is added This situation can’t exist if only acid is present; a mixture of the acid and salt is used. The weak acid provides the equilibrium and the large CH3COOH(aq) concentration. The sodium salt provides the large CH3COO¯(aq) concentration. One uses a WEAK ACID + its SODIUM OR POTASSIUM SALT

  11. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3.

  12. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3. Ka = [H+(aq)] [A¯(aq)] [HA(aq)]

  13. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3. Ka = [H+(aq)] [A¯(aq)] [HA(aq)] re-arrange [H+(aq)] = [HA(aq)] x Ka [A¯(aq)]

  14. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3. Ka = [H+(aq)] [A¯(aq)] [HA(aq)] re-arrange [H+(aq)] = [HA(aq)] x Ka [A¯(aq)] from information given [A¯] = 0.1 mol dm-3 [HA] = 0.1 mol dm-3

  15. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3. Ka = [H+(aq)] [A¯(aq)] [HA(aq)] re-arrange [H+(aq)] = [HA(aq)] x Ka [A¯(aq)] from information given [A¯] = 0.1 mol dm-3 [HA] = 0.1 mol dm-3 If the Ka of the weak acid HA is 2 x 10-4 mol dm-3. [H+(aq)] = 0.1 x 2 x 10-4 = 2 x 10-4 mol dm-3 0.1

  16. Calculating the pH of an acidic buffer solution Calculate the pH of a buffer whose [HA] is 0.1 mol dm-3 and [A¯] of 0.1 mol dm-3. Ka = [H+(aq)] [A¯(aq)] [HA(aq)] re-arrange [H+(aq)] = [HA(aq)] x Ka [A¯(aq)] from information given [A¯] = 0.1 mol dm-3 [HA] = 0.1 mol dm-3 If the Ka of the weak acid HA is 2 x 10-4 mol dm-3. [H+(aq)] = 0.1 x 2 x 10-4 = 2 x 10-4 mol dm-3 0.1 pH = - log10 [H+(aq)] = 3.699

  17. Calculating the pH of an acidic buffer solution Calculate the pH of the solution formed when 500cm3 of 0.1 mol dm-3 of weak acid HX is mixed with 500cm3 of a 0.2 mol dm-3 solution of its salt NaX. Ka = 4 x 10-5 mol dm-3.

  18. Calculating the pH of an acidic buffer solution Calculate the pH of the solution formed when 500cm3 of 0.1 mol dm-3 of weak acid HX is mixed with 500cm3 of a 0.2 mol dm-3 solution of its salt NaX. Ka = 4 x 10-5 mol dm-3. Ka = [H+(aq)] [X¯(aq)] [HX(aq)]

  19. Calculating the pH of an acidic buffer solution Calculate the pH of the solution formed when 500cm3 of 0.1 mol dm-3 of weak acid HX is mixed with 500cm3 of a 0.2 mol dm-3 solution of its salt NaX. Ka = 4 x 10-5 mol dm-3. Ka = [H+(aq)] [X¯(aq)] [HX(aq)] re-arrange [H+(aq)] = [HX(aq)] Ka [X¯(aq)]

  20. Calculating the pH of an acidic buffer solution Calculate the pH of the solution formed when 500cm3 of 0.1 mol dm-3 of weak acid HX is mixed with 500cm3 of a 0.2 mol dm-3 solution of its salt NaX. Ka = 4 x 10-5 mol dm-3. Ka = [H+(aq)] [X¯(aq)] [HX(aq)] re-arrange [H+(aq)] = [HX(aq)] Ka [X¯(aq)] The solutions have been mixed; the volume is now 1 dm3 therefore [HX] = 0.05 mol dm-3 and [X¯] = 0.10 mol dm-3

  21. Calculating the pH of an acidic buffer solution Calculate the pH of the solution formed when 500cm3 of 0.1 mol dm-3 of weak acid HX is mixed with 500cm3 of a 0.2 mol dm-3 solution of its salt NaX. Ka = 4 x 10-5 mol dm-3. Ka = [H+(aq)] [X¯(aq)] [HX(aq)] re-arrange [H+(aq)] = [HX(aq)] Ka [X¯(aq)] The solutions have been mixed; the volume is now 1 dm3 therefore [HX] = 0.05 mol dm-3 and [X¯] = 0.10 mol dm-3 Substituting [H+(aq)] = 0.05 x 4 x 10-5 = 2 x 10-5 mol dm-3 0.1 pH = - log10 [H+(aq)] = 4.699

  22. SALT HYDROLYSIS Many salts dissolve in water to produce solutions which are not neutral. This is because the ions formed react with the hydroxide and hydrogen ions formed when water dissociates. There are four distinct systems. All dissociated ions are aqueous ions. When mixed, the ions of strong acids and bases remain apart. Ions of weak acids and bases associate.

  23. SALT HYDROLYSIS Many salts dissolve in water to produce solutions which are not neutral. This is because the ions formed react with the hydroxide and hydrogen ions formed when water dissociates. There are four distinct systems. All dissociated ions are aqueous ions. When mixed, the ions of strong acids and bases remain apart. Ions of weak acids and bases associate. Salts of strong acids and strong bases - SODIUM CHLORIDE NaCl dissociates completely in water Na+ Cl¯ ——> Na+ + Cl¯ Water only ionises to a very small extent H2O OH¯ + H+ Na+ and OH¯ are ions of a strong base so remain apart H+and Cl¯ are ions of a strong acidso remain apart all the OH¯ and H+ ions remain in solution therefore [H+] = [OH¯] and the solution will be NEUTRAL

  24. SALT HYDROLYSIS Many salts dissolve in water to produce solutions which are not neutral. This is because the ions formed react with the hydroxide and hydrogen ions formed when water dissociates. There are four distinct systems. All dissociated ions are aqueous ions. When mixed, the ions of strong acids and bases remain apart. Ions of weak acids and bases associate. Salts of strong acids and weak bases - AMMONIUM CHLORIDE NH4Cl dissociates completely in water NH4+ Cl¯ ——> NH4+ + Cl¯ Water only ionises to a very small extent H2O OH¯ + H+ NH3 + H2O Na+ and OH¯ are ions of a strong base so tend to be associated H+and Cl¯ are ions of a strong acidso remain apart all the H+ions remain in solution therefore [H+] > [OH¯] and the solution will be ACIDIC

  25. SALT HYDROLYSIS Many salts dissolve in water to produce solutions which are not neutral. This is because the ions formed react with the hydroxide and hydrogen ions formed when water dissociates. There are four distinct systems. All dissociated ions are aqueous ions. When mixed, the ions of strong acids and bases remain apart. Ions of weak acids and bases associate. Salts of weak acids and strong bases - SODIUM ETHANOATE CH3COONa dissociates completely in water CH3COO ¯ Na + ——> Na+ + CH3COO¯ Water only ionises to a very small extent H2O OH¯ + H+ CH3COOH Na+ and OH¯ are ions of a strong base so remain apart H+and CH3OO¯ are ions of a weak acid so tend to be associated all the OH¯ ions remain in solution therefore [OH¯] > [H+] and the solution will be ALKALINE

  26. SALT HYDROLYSIS Many salts dissolve in water to produce solutions which are not neutral. This is because the ions formed react with the hydroxide and hydrogen ions formed when water dissociates. There are four distinct systems. All dissociated ions are aqueous ions. When mixed, the ions of strong acids and bases remain apart. Ions of weak acids and bases associate. Salts of weak acids and weak bases - AMMONIUM ETHANOATE CH3COONH4 dissociates completely in water CH3COO ¯ NH4+ ——> NH4+ + CH3COO¯ Water only ionises to a very small extent H2O OH¯ + H+ NH3 + H2O CH3COOH Na+ and OH¯ are ions of a weak base so tend to be associated H+and CH3OO¯ are ions of a weak acid so tend to be associated the solution might be alkaline or acidic i.e. APPROXIMATELY NEUTRAL

  27. REVISION CHECK What should you be able to do? Recall the definition of a buffer solution Recall the difference between an acidic and an alkaline buffer solution Recall the uses of buffer solutions Understand the action of buffer solutions Calculate the pH of an acidic buffer solution Recall and understand the reactions due to salt hydrolysis CAN YOU DO ALL OF THESE? YES NO

  28. You need to go over the relevant topic(s) again Click on the button to return to the menu

  29. WELL DONE! Try some past paper questions

  30. BUFFER SOLUTIONS THE END © 2004 JONATHAN HOPTON & KNOCKHARDY PUBLISHING

More Related