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QCC CHM 124 - Determination of a Solubility Product Constant

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Alferid Hussin ShifaCHM (Course 124) (Section 01)Lab (6)Oct 27/2019Lab 6: Determination of a Solubility Product ConstantObjective: The purpose of this experiment is to perform a titration to determine the concentration and thus its Ksp value of calcium hydroxide. List of chemicals, & hazard:- calcium hydroxide - Ca(OH)2- 0.05 M Hydrochloric acid - HCl (highly hazardsList of Chemicals with Safety Hazard: There are Hazards chemicals in this experiment.I. Safety Precautions:- Be cation when handling the HCl solutionII. Waste Disposal:- Disposal the mixtures in the sink, or into the appropriate waste beaker.List of Equipment:Erlenmeyer flask (250 mL) Pipet aid & disposable pipet’s (Three of 10 mL)Beaker (two of 250 mL) Burets (two 50 mL)Distilled water Filter paper Phenolphthalein indicator solution Universal StandTitration Clamp graduated cylinder ( 25 mL) Pre-Lab Questions:None1Procedure in short: 1. First, measure initial temperature of the stock calcium hydroxide solution, because a saturated solution is only saturated at a given temperature.2. Slowly titrate the Ca(OH)2 into a flask with HCL, distilled water, and phenolphthalein as an indicator. 3. Titrate until the solution begin to have a light pink color. This is the endpoint of the titration, and record the volume of Ca(OH)2 required to reach the endpoint of the titration. 4. Initiate the trituration with two wash cycles of the titrant solution. Then begin the trituration.5. Repeat the titration until 3 accurate trials have been completed. ResultVolume of 0.0M HCl Volume of saturated Ca(OH)2Volume distilled WaterTitration 1 20ml 32.5ml 25mlTitration 2 20ml 32.7ml 25ml Average volume of saturated Ca(OH)2: 32.6ml2Post lab 1. Since Ca(OH)2 follows a exothermic process, any temperature increase will increase the production of the OH- ions. Also, since this an equilibrium reaction, the equilibrium shifts to counteract the imposed change and a new equilibrium is established according to Le Chatelier’s principle. Hence, a decrease in solubility as the temperature increases, due to it backward shifts.2. The Ksp is a constant value, that stand for k constant of the solubility produce. Since the formula of constant kSP, is found by multiplying the concentration of ion to the power of their stoichiometric Coefficient. Hence −¿O H¿¿¿Ksp=[C a+2]¿3. Dilute solution- A concentrated solution mixed with something else to bring downpotencyConcentrated solution- Just one substance present in very high proportionSaturated solution- A solution contains the greatest amount of atoms mixed into a solution at a given temperature.Any specific observations:- No specific observations were madeConclusion:- The purpose of this lab was to determine experimentally the solubility product constant of calcium hydroxide and its molar solubility by finding the amount of OH-in a saturated Ca(OH)2 solution. The Ksp values found was 6.39 x 10^-5. In the other hand, the concentration of the hydroxide ion was approximately value of 0.05


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