The document provides instructions for an experiment to determine the solubility of calcium hydroxide. The experiment involves preparing a saturated calcium hydroxide solution, standardizing hydrochloric acid, and then titrating the calcium hydroxide solution with the standardized acid. Students are advised to review solubility and the solubility product constant (Ksp) in their textbook before setting up calculations involving Ksp. The titration will have two equivalence points but sometimes only one will be visible, and students are told to continue titrating until their data plateaus.

1. Solubility of Calcium Hydroxide

2. PreparationWrite the procedure for the experimentProcedure should contain enough detail so someone else could replicate it without additional informationDetermine the approximate mass of Ca(OH)2 to use for your saturated solutionBoth must be done before you come to class

3. ExperimentThree partsPreparing saturated solutionStandardization of HClDetermine [OH¯]

4. Saturated SolutionPrepare saturated solution on Day 1Save for Day 2 to complete titrations

5. Standardization of HClRecord exact mass of Na2CO3 used for each trialDo not refill HCl bottle during experimentSave HCl solution for next week’s lab

6. Titration: HCl and Ca(OH)2Filter Ca(OH)2 before usingTitration will have two equivalence points; sometimes only one will show

7. KspReview solubility and Kspin your textbookSetting up a Ksp expressionCalculations involving Ksp

8. Experiment TipsNeed three good titrations for each partTitration curves may only show one equivalence point even though there are twoFirst one is sometimes hard to seeContinue until data plateaus

9. Experiment TipsRecord exact volumes used for all masses and volumesWhen using buret, estimate the second decimal placeMix after every addition to get accurate pH values