logging in or signing up Potentiometric and Diazotization Titrations ppt gvrr416 Download Post to : URL : Related Presentations : Let's Connect Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Copy embed code: Embed: Flash iPad Dynamic Copy Does not support media & animations Automatically changes to Flash or non-Flash embed WordPress Embed Customize Embed URL: Copy Thumbnail: Copy The presentation is successfully added In Your Favorites. Views: 2680 Category: Science & Tech.. License: All Rights Reserved Like it (2) Dislike it (0) Added: February 21, 2010 This Presentation is Public Favorites: 0 Presentation Description No description available. Comments Posting comment... By: syedshabbar08 (35 month(s) ago) Nice one Saving..... Post Reply Close Saving..... Edit Comment Close Premium member Presentation Transcript A Seminar on Potentiometric and Diazotization Titrations : A Seminar on Potentiometric and Diazotization Titrations 1 BY G.V.RAMANA REDDY DEPT.OF PHARMACEUTICAL ANALYSIS KARPAGAM UNIVERSITY COIMBATORE Diazotization Titrations : 2 Diazotization Titrations Aromatic primary amines react with sodium nitrite in acidic solutions to form diazonium salts. C6H5NH2 + NaNO2+HCl C6H5N2Cl+ NaCl + 2H2O End point is indicated by the presence of small amounts of nitrous acid. Slide 3: 3 End point detection by two methods, Visual end point Amperometrically Visual end point is indicated using starch iodide paper according to the formula KI + HCl HI + KCl 2HI + 2HNO2 I2 + 2NO + 2H2O Slide 4: 4 Amperometric method is using bright platinum electrodes. At the end point, permanent deflection of the galvanometer is observed. Usually 30 – 50mV of potential is applied. Applications : 5 Applications Used in the determination of primary aromatic amines. May be used for the analysis of drugs such as benzocaine, dapsone, primaquine etc. Potentiometry : 6 Potentiometry In potentiometric titrations the change in the electrode potential upon the addition of titrant are noted against the volume of titrant added. Ecell = Eref + Eindicator + Ejunction Theory – Nernst Equation : 7 Theory – Nernst Equation Nernst equation is the basis for the relationship between the voltage generated by an electrochemical cells a result of the two half cell reactions and the relevant concentration at each electrode. Nernst equation for a redox electrode may be given as E = E°ox,red + (RT/zF).ln(aox/ared) Types of Potentiometric Titrations : 8 Types of Potentiometric Titrations Acid-base titrations Complexometric Titrations Oxidation-Reduction Titrations Precipitation Titrations Non-Aqueous solvents Acid – Base Titrations : 9 Acid – Base Titrations Here hydrogen electrode may be employed and the reference electrode may be N – Calomel electrode The potential of any hydrogen electrode may be given by the equation, E = E° - 0.0591 log aH+ at 25°C. Where E° is the standard electrode potential. Slide 10: 10 It can be concluded from the graph that the change in the electrode potential or EMF is proportional to the change in pH during titration. The point where the EMF increases rapidly gives the end point. Complexometric Titrations : 11 Complexometric Titrations Complexometric titrations can be followed with an electrode of the metal ion whose ion is involved in complex formation. After the end point, addition of further ions does not affect the concentration of the complex so that the titration curve has almost horizontal portion after the equivalence point. Oxidation – Reduction Titrations : 12 Oxidation – Reduction Titrations These type of reactions can be followed by inert indicator electrodes. The electrode assumes a potential proportional to the logarithm of concentration ratio of the two oxidation states of the reactant or the titrant which ever is capable of properly poising the electrodes. Equivalence point is indicated by a marked deflection in the titration curve. Slide 13: 13 These may be used in monitoring procedures such as monitoring cyanide wastes from metal plating industries or chlorine compounds in bleach compound manufacturing, etc. Precipitation Titrations : 14 Precipitation Titrations Here, the solubility product of the almost insoluble material formed during a precipitation reaction determine the ionic concentration at the equivalence point. The indicator electrodes must readily come into equilibrium with one of the ions. Non – Aqueous Solvents : 15 Non – Aqueous Solvents Here, the ordinary glass calomel electrode system can be used. In non-aqueous titrations, usually, the milli volt scale of potentiometer is used rather than pH scale since the potential of the non-aqueous systems exceed the pH scale. Reference Electrodes : 16 Reference Electrodes Calomel Electrodes – potential of 250, 286 and 338 mV in saturated, 1 M and 0.1M KCl respectively at 20°C Silver – Silver chloride electrode – potential of 200, 235.5 and 288 mV at 25°C Mercury (I) Sulphate electrode – potential of 682 mV Salt Bridge : 17 Salt Bridge Salt bridge of potassium chloride, potassium nitrate or ammonium nitrate is used to prevent the possible contamination of the reference electrode with test solution. Usually the salts are solidified with 3% agar. Indicator Electrodes : 18 Indicator Electrodes Hydrogen Electrodes Glass Electrodes Ion Selective Electrodes (ISE) Hydrogen Electrode : 19 Hydrogen Electrode Consists of a small piece of Pt foil coated with Pt black, over which hydrogen gas is passing. Thus the electrode will act as if it were an electrode of metallic hydrogen. Glass Electrode : 20 Glass Electrode Advantage of rapid response, unaffected by the presence of oxidizing and reducing agents, or salts in moderate concentrations. Disadvantage of fragility, imperfections in the bulb may cause error. Rejuvenation required over a period of time to avoid any errors. Ion Selective Electrode : 21 Ion Selective Electrode Generally consists of a thin layer of an electrically conducting material called the membrane across which a potential develops. Classified as solid state, heterogeneous, liquid ion exchanger and glass type. ISE – Characteristics and Usage : 22 ISE – Characteristics and Usage Response Limits of Detection Interference pH effects Electrode lifetime Measurement of pH : 23 Measurement of pH The activity of hydrogen ions in solution is variable in the Nernst equation for an electrode reversible to these ions, and therefore such an electrode can produce an EMF related to solution pH as of definitions, pH = -log10aH3O+ pOH = -log10aOH- Slide 24: 24 2H2O H3O++OH- Or H2O H++OH- By law of mass action, for pure water, [H+][OH-]=Kw Taking log on both sides and rearranging, pH+ pOH = pKw =14 Applying this to Nernst equation, Slide 25: 25 E = E°H+,H2 - 0.0592 pH Since E°H+,H2 is defined as zero, E = - 0.0592 pH Applications : 26 Applications For the measurement of the endpoint of the titrations which may not be feasible for visual end point detection using indicators. For the measurement of pH In Non-aqueous titrations In complexometric and precipitation titrations. In redox titrations Slide 27: 27 For the determination of ferrous ammonium sulphate (redox titrations), titration of potassium bromide with silver nitrate ( precipitation titration), back titrations of reagents such as pyridine, glycine, PABA with HCl followed by NaOH etc. THANK YOU : THANK YOU 28 You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.