The Solubility of Calcium Hydroxide

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The Solubility of Calcium Hydroxide Introduction: Experiment 16 was done to get an understanding of the solubility of calcium hydroxide, or the slightly soluble salts, gather the knowledge to calculate the Ksp using a primary standard for determining the concentration of an acid, and learning the knowledge to prepare a saturated solution of a slightly soluble salt. This experiment has a few different parts to complete to gather all the information needed to get the experimental values that are seen in the text books used every day. Those values were at some point one by one experimentally calculated as in this experiment. For the first part of this experiment is –saturated solution, for each pair of students should prepare the saturated Ca(OH)2 solution. Of course the saturated solutions take time this experiment is done in a two day lab setting part one should be completed during the first day and ready for use on day two. Remember because Le Châtelier’s principle if you don’t filter the solution will rise. The removal of OH- from the UN filtered solution will cause more Ca(OH)2 to be dissolved for the equilibrium to restore. The second part of this lab takes knowledge from past experiments done in this laboratory. Using the Primary method used to standardize the concentration of HCl, this will bring much lower percent error in the Ksp For this standardization sodium carbonate should be used for determining the amount of hydroxide in the solution. For this the equation used will be Na2CO3+2 HCl→H2O+2 NaCl The third part of this experiment uses the prepared saturated solution from part one. This part used the value for exact concentration of the HCl. Part three is done to determine the concentration of hydroxide in the solution, allowing the students to determine a value of Ksp for Ca(OH)2 completing the lab. The equation used for part three is: 2

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