# Question 1: Arrange the six solutions tested from the...

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Experiment 14 Part 1 Section A. Conductimetry and the Strength of Acids and Bases Goal: To conduct and analyze acid-base reactions, through titrations, for their equilibria. Procedure: Thompson, S. PSU Chemtrek: Expt. 16 Carbon Dioxide Scrubbers; Keiser, J., Hayden- McNeil Publishing: Plymouth, MI, 2020, pp 16-1 - 16-13. Watch the video and follow along with the steps in your lab manual. In the space below, please summarize the procedure for this section and record any observations you are able to make watching the video. Using a conductivity probe, test the conductivity of distilled water, tap water, 0.1 M C H 3 COOH , 0.1 M N H 3 / N H 4 OH , 0.1 M NaOH , 0.1 M HCl . The distilled water will not have any conductivity because of its lack of dissolved ions. Tap water has a conductivity of ~ 5/10. Acetic Acid ( C H 3 COOH ) has a conductivity of ~ 4/10. N H 3 / N H 4 OH has a conductivity of ~ 5/10 with some fluctuation. NaOH has a conductivity of ~ 8/10. HCl has a conductivity of ~ 9/10 with a bit more fluctuation.
Question 1: Arrange the six solutions tested from the lowest to the highest conductivity. Explain the order observed—i.e., why do solutions of the same concentration have different conductivities? If you cannot differentiate between them, explain why not. HCl
Question 2: The conductivity of an H 2 SO 4 solution was followed as it was titrated with the strong base Ba(OH) 2 . Predict the relative conductivities of: (a) the starting solution very high (b) the solution at the equivalence point none (c) the solution well past the equivalence point increases (excess titrant) HINT: First write a balanced reaction. Remember that BaSO 4 is insoluble.