17_Lab_113

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sDetermining K sp of Calcium Hydroxide with Hydrogen Concentrations Introduction: The purpose of the experiment is to calculate the K sp value of calcium hydroxide through experimentation with primary standards and saturated solutions while understanding the solubility of slightly soluble salts (French et al. 97). The hypothesis is that this will be determined through finding the hydrogen concentration in a saturated calcium hydroxide solution. According to French et al. “a saturated solution is one in which the maximum amount of solute has been dissolved.” A saturated solution can be made over a long period of time hence why the lab is split up into two weeks. Once the maximum amount has been dissolved, one must filter the solution to rid it of excess solute. Filtering is crucial in this as excess calcium hydroxide will result in a skewed equilibrium as increased HCl will need to be added to establish equilibrium. This is indicative of Le Châtelier’s principle as removing OH - from an unfiltered solution dissolved more Ca(OH) 2 to restore equilibrium (French et al. 98). Filtering will also aid in assuring the titration results are accurate. The titration relationship of calcium hydrogen with hydrochloric avid is denoted by equation 1: Ca(OH) 2 + 2 HCL  CaCl 2 + 2 H 2 O (French et al. 98). To obtain K sp , equal to K sp = [Ca 2+ ][OH - ] 2 , it is imperative to standardize the concentration of HCl through primary standard experimentation. In this experiment, the primary standard will be composed of sodium carbonate denoted in relationship 2: Na 2 CO 3 + 2 HCl  CO 2 +H 2 O + 2 NaCl (French et al. 98).

According to French et al. “Once the exact concentration of HCl has been found, the concentration of hydroxide in the solution can be found,” which will allow for the K sp to be solved for of the reaction denoted in relationship 1. Methods: List of Materials (French et al. 99):  Na 2 CO 3  HCl solution  Ca(OH) 2  Storage bottles (2)  pH sensor  Drop counter  MeasureNet  Glassware as needed  Funnel  Filter paper  Buffers (pH: 4 & 10)  Burette and clamp  Ring stand Procedure (French et al. 98-99):

Day 1 Experimentation: 1. MeasureNet Calibration: a. Power On b. MAIN MENU c. pH/mV d. pH vs. Volume e. CALIBRATE f. Enter 22 for room temperature g. Place pH in beaker and flush with DI water h. Set 4 for the buffer, place probe in the pH 4 buffer solution and then press enter. i. Flush the probe with DI water and place in the pH 10 buffer solution then press enter j. Flush probe with DI water and place in storage solution k. Press DISPLAY on MeasureNet, flush the probe with DI water and insert into the buffer solution. 2. Preparing Calcium Hydroxide Solution a. Obtain large beaker and fill with water, at least 100 mL b. Stir in the solute to the water adding more than one would think could be dissolved while ensuring not to add more than 4g/L of water. c. Obtain storage container and label with section #, TA, name(s) and “NOT FOR HUMAN CONSUMPTION” d. Add solution to the storage container and let sit 3. Standardization of HCl

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a. Prepare three Na 2 CO 3 solutions using ~.2 grams of Na 2 CO 3 and 20ml of water each and mix in a beaker while ensuring to record the exact mass of Na 2 CO 3 b. Set up a burette stand filled with 0.2 HCl while recording the initial level of the burette c. Preform MeasureNet calibration as explained in Step 1 d. Enter initial volume of HCl and start the recording of data e. Run the titration until all equivalence point(s) have been reached f. Stop the Measurenet, record the final volume in mL and save the file as “001” g. Repeat steps b-f with the two other Na 2 CO 3 solutions and saving the files as “002” and “003” respectively h. Clean the work station and pour neutral solutions with excess water down the drain Day 2 Experimentation: 1. MeasureNet Calibration a. Repeat steps 1(a-k) from Day 1 Experimentation 2. Determination of [OH - ] a. Obtain the prepared Ca(OH) 2 solution while ensuring not to shake. b. Set up a 125mL flask with filter paper and slowly pouring the solution into the flask c. Repeat step b to decant the solution until clear d. Set up a burette with the 0.2M HCl e. Repeat Step 3 (b-f) of day 1 with the Ca(OH) 2 samples while saving the files as “004,” “005,” and “006” respectively

f. Clean work station Discussion: The purpose of this experiment is to determine the K sp of calcium hydroxide through the determination of hydroxide concentration in a saturated solution. Through the standardization of HCl and titration of Ca(OH) 2 , the average concentration was found to be .1751 M and .01751 M respectively. The K sp value was found to be 2.147E-5 experimentally compared to an accepted value of 6.5E-6. This resulted in a percent error of 230.7%. The results support the hypothesis and purpose of the experiment as the K sp was determined through determination of hydrogen concentration in a series of saturated calcium hydroxide solutions. However, it is important to note that due to the relatively high percent error, the K sp value was not accurately calculated as it was not close to the accepted value of 6.5E-6. A potential source of error in the experiment could result from shaking the storage container housing the calcium hydroxide. As the solution needs a week to develop, shaking the solution would negate any progress that was made through preventing the ability to properly filter the solution. A way to mitigate this, is to ensure the label is accurately labeled to prevent other students from mishandling the labeled solution. Safely transporting the solution from the materials shelf to the workstation is also crucial to protecting the integrity of the solution. However, it is nearly impossible to fully prevent other people from touching one’s solution, but labeling the solution would help to mitigate risk. Another possible source of error within the experiment is adding too much Ca(OH) 2 to the beaker and/or storage container. As stated in the lab manual, it is imperative to not add more

than 4g/L of water. Adding more than this would result in an over concentrated solution which would negatively impact the concentration values while also preventing the ability to filter correctly. This could be mitigated through weighing out the amount of Ca(OH) 2 to be certain, or to ask a TA if the solution needs more Ca(OH) 2 while adding it slowly to the container. A final possible source of error within the experiment is adding too little Ca(OH) 2 to the storage container with the water. This would result in an undersaturated solution and would result in altered outcomes of the equivalence point. This could be mitigated by adding as much solute as possible while asking a TA for oversight. Conclusion: In this experiment I learned about how I can determine the K sp of a saturated solution which fulfills one of the intended purposes of the lab. I was also able to strengthen my experimental techniques while learning of the importance of standard solutions. Solubility product constants are integral to many fields in chemistry for preparing solutions. One application is in pharmaceuticals where an understanding of solubility of compounds is integral to understand dosage forms as well as interactions between different medicine. I have no suggestions to improve the lab.

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Works Cited French, April, Allison Soult, M. Mearl Savas, Francois Botha, Carolyn Brock, Charles Griffith, Darla Hood, Robert Kiser, Penny O’Connor, William Plucknett, Donald Sands, Diane Vance, William Wagner. “Experiment 17 Solubility of Calcium Hydroxide” General Chemistry II Laboratory Manual . Plymouth, MI: Hayden-Mcneil, 2020. 97-100. Web. 1 December 2021.

https://www3.chem21labs.com/labfiles/36194_48_Exp%2017_FrenchA%202187- 1%20W20..pdf?rf=3392 French, April, Allison Soult, M. Mearl Savas, Francois Botha, Carolyn Brock, Charles Griffith, Darla Hood, Robert Kiser, Penny O’Connor, William Plucknett, Donald Sands, Diane Vance, William Wagner. “Using MeasureNet and Probes.” General Chemistry II Laboratory Manual . Plymouth, MI: Hayden-Mcneil, 2020. 37-50. Web. 1 December 2021. https://www3.chem21labs.com/labfiles/36194_48_1-4_FrenchA%202187- 1%20W20..pdf?rf=7702

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