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EXPERIMENT 2 CONDUCTOMETRIC TITRATION Introduction Electrical Conductivity measurements can be used to titrate acids, bases and in precipitation titrations. Conductivity meter measures conductance changes during the titration. The equivalence point of the titration is detected by plotting a titration curve using conductance values and volumes of a base added. The principle of conductometric titration is based on the fact that during the titration, the other replaces one of the ions and invariably these two sons differ in the ionic conductivity with the result that conductivity of the solution varies during the course of titration. The equivalence point is located graphically by plotting the change in conductance as a function of the volume of titrant added. First: Neutralization Titration A: determination of the strength of hydrochloric acid solution by a standard solution of sodium hydroxide. (Strong acid with a strong base) THEORY: Neutralization between a strong acid (HCI) and a strong base (NaOH) is represented by: HCI + NaOH → H.0+ NaCI It is evident from the above equation that as NaOH solution is gradually added, the H ion having high ionic conductance is replaced by Na* owing tower ionic conductance and hence the conductivity of the solution gradually decreases. At the equivalent point, the conductivity would be minimum due to replacement of all Hions by Naions. After the equivalence point, both Na and OH will accumulate in the solution and conductivity of the solution will again increase. If the conductance corresponds to the volume of NaOH solution 16

added be plotted, two straight lines having opposite slopes would be obtained. The point of intersection of the two straight lines will represent the end point Figure (1) Electrical conductance G (5) END POINT Volume or Not (m FIGURE 1: TITRATION GRAPH OF A STRONG AODE WITH A STRONG BASE TOOLS AND CHEMICALS: • Conductivity meter • HCI (Unknown) & NaOH (ON) • Beaker 100 ml • (50 ml) Burette and (30 ml) pipette PROCEDURE: 1. Open the conductivity meter, clean the electrodes by deionized or distilled water thoroughly before beginning the experiment. Important tip: Note the unit of the device SmS or us, to convert to the appropriate unit 2. Fill the burette with NaOH solution 3. Using a clean pipette, transfer 30 ml. of HCl solution in a 100 ml beaker 4. Immerse the electrode and read the G of the solution. 5. Add 3 ml of NaOH solution of the burette and record the corresponding G. 6. Make additions of NaOH from the burette as given in data table. After each addition (3 ml each), stir the solution well and read the conductance G 7. Tabulate your result 17 18 of 59 Electrochemistry Lab

Data Table 2 NaOH Volume (ml) G(S)x10 NaOH Volume (ml) G(S) 27.0 6.3 0 33 22.3 7.0 3 36 19.0 7.6 6 39 9 16.1 42 8.2 12 13.7 45 8.6 15 10.9 48 9.1 18 51 8.8 9.5 21 54 6.7 10.1 24 57 4.8 10.5 27 60 4.9 10.8 30 5.5 CALCULATION AND RESULTS: 1. On a graph sheet, draw the relationship between conductance (G) and volume of added NaOH and determine the end point graphically as shown in Figure (1) End point -...2.4........... 2. Calculate normality and the strength of solution. Normality: NaOH CV-CV SV ox24 Hej Strength of HCI solution KeL): Normality x Eq.wt=\ ..0...0.8 HCI 18

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