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Solubility Product Of Calcium Hydroxide Lab Report

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Solubility Product Of Calcium Hydroxide Lab Report
Experiment 10: Solubility Product for Calcium Hydroxide
GOAL AND OVERVIEW A saturated solution of Ca(OH)2 will be made by reacting calcium metal with water, then filtering off the solids: Ca(s) + H2O → Ca(OH)2(s) Ca2+(aq) + 2OH-(aq) The concentration of dissolved hydroxide will be determined by acid-base titration with standardized HCl solution. The Ksp for Ca(OH)2 will be calculated from the experimentally determined saturation concentration of hydroxide. Objectives of the data analysis understand solubility equilibria, acid-base neutralization, and the chemistry of lime (Ca(OH)2), limewater, and calcium carbonate (called limestone when occurring naturally as a mineral) manipulate equations for saturation equilibria, acid-base titrations, …show more content…
The equilibrium constant for the reaction is the solubility product constant, Ksp, given by Ksp = [Ca2+][OH-]2 (2) The concentration of Ca(OH)2(s) does not appear the equilibrium constant expression because it is always present as the pure solid (constant concentration, or amount per …show more content…
How, if at all, would it have affected the results if you did the experiment without filtering out the solid Ca(OH)2 that was present in the vessel? 2. A saturated solution of AB3 was titrated to determine the Ksp for AB3. AB3 has the following dissociation equilibrium: AB3(s) A3+(aq) + 3B-(aq). By titration, it was determined that 0.0013 moles of B- was present in 100 ml of the filtered saturated solution. What is the Ksp for AB3? Would you consider AB3 to be a soluble or insoluble compound? 3. How did the acid titration allow you to determine the solubility constant in this experiment (hint: What information does acid/base titrations give you?) 4. Why will it skew your results if you wash the precipitate after filtring of the calcium hydroxide? 5. The Ksp for Fe(OH)3 = 2.5x10-20. Write down the Ksp equation in terms of Fe3+ and OH- concentrations. Second, given 5.0×10-5M HCl, how many mL acid would you need in order to neutralize a 30. mL aliquot of the saturated Fe(OH)3 solution? 6. Will a very soluble solid have a large or small Ksp? Explain. 7. How is ‘saturation’ of a given ion related to ‘solubility’ of a given
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