Lab Report #8 .docx - EXPERIMENT 8 Electrical Conductivity...

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Electrical Conductivity of Aqueous Solution Sabrina Castro ∙ April 13th, 2020 Dr. Q Meng ∙ Chemistry 1105 S51 Objective: The goal of this experiment observe the electrical conductivity of substances in aqueous solutions. Observing the electrical conductivity of substances will reinforce the ability to determine whether an aqueous solution is a strong or weak electrolyte. Through the observations of the aqueous solution conductivity, chemical reactions will be able to be interpreted. This experiment will enhance proficiency in writing net equations. Introduction: Electrical conductivity is based on the flow of electrons. Metals are good conductors of electricity because they allow electrons to flow through the metal. Distilled water is a very weak conductor because very little electricity passes through pure water. However, when a substance dissolves in water and forms ions, the ions are capable of conducting an electric current. If the substance is highly ionized, the solution is a strong conductor of electricity. If the substance is only slightly ionized the solution is a weak conductor. Strong acids and salts are strong electrolytes because they completely ionize (dissociate or separate) in solution. The ions carry the electric charge through the solution thus creating an electric current. The current, if sufficient enough, will light one or both LEDs on a conductivity meter, shown at right. This experiment will involve the testing of electrical conductivity. Substances will be tested by the use of the EXPERIMENT 8
conductivity apparatus. A bright glowing light will mean the solution has strong electrolytes, while a dim light will signify weak electrolytes. Materials: Conductivity apparatus Small, dry beakers (6) Glass stirring rod Wash bottle with distilled water Sodium chloride, solid NaCl Calcium carbonate, solid, CaCO3 Calcium chloride, solid CaCl2 Hydrochloric acid, 0.1 M HCl Acetic Acid, 0.1 M HC2H3O2 Nitric acid, 0.1 M HNO3 Sodium hydroxide, 0.1 M NaOH Ammonium hydroxide, 0.1 M NH4OH Potassium iodide, 0.1 M KI Aluminum nitrate, 0.1 M Al(NO3)3 Magnesium Hydroxide, Mg(OH)2 Copper (II) Sulfate, 0.1 M CuSO4 Calcium Nitrate, 0.1 M Ca(NO3)2 Sulfuric Acid, 0.1 M H2SO4 Barium hydroxide, 0.1 M Ba(OH)2 Straw Procedure: A. Conductivity Testing – Evidence for Ions in Aqueous Solution 1. Pour 25 mL of distilled water in a small dry beaker and test the conductivity. Pour about 25 mL of tap water in a small dry beaker and test the conductivity.

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