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Expt04_ElectrolytesAndNon-electrolytes - container 2 For...

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Date Performed: Experiment No. 4 Electrolytes and Non-electrolytes I. Objectives: >To be able to note down which ions are better conductors than others. >To be able to see determine which of the solutions used are strong or weak electrolytes. II. Diagrams/ Figures for special set-ups: Conductance set-up III. Outline/Schematic Diagram of procedure: MATERIALS: 100-mL beakers 50-mL graduated cylinder Conductance set-up Distilled water Reagents needed (10-15 mL each): 1.00 M solutions of HCl, CH 3 COOH, NaOH, NH 3 , NaCl, NaC 2 H 3 0 2 , sucrose 2.00 M solutions of NH 3 , HCl, CH 3 COOH Glacial acetic acid PROCEDURE: IV. Special Notes: Note 1: Wash the electrodes with distilled water prior to each test. Wipe the electrodes separately with a piece of tissue paper. Note 2: Stop adding water when there is no more change in the intensity of the light bulb. WASTE DISPOSAL: 1. Dispose all acidic solns into the “ Inorganic Waste”
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Unformatted text preview: container. 2. For the solutions of salts, sugar, NH 3 + HCl and NH 3 + CH 3 COOH, dilute with water before directly flushing down the sink with copious running water. IV. Tabulation of Data: Place approx. 10 mL of assigned solution in a 100 mL beaker and test for consuctance. (Group assigned with distilled water will be the first one to test for conductance.) Immerse the electrodes one cm apart into the liquid or solution (Note 1). Note the intensity of the glow of the light bulb. Describe the glow as being: bright, dim or none. The conductance of the other 1.00 M solutions will then be tested. For 2.00 M solutions, combine NH 3 and HCl in equal volumes. Do the same for NH and CH COOH. Observe what happens to the conductance of the glacial CH 3 COOH upon successive dilutions with 10 mL of distilled water (Note 2). Record your results....
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