- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 1 (35.31 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 2 (28.97 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 3 (25.73 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 4 (25.41 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 5 (23.82 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 6 (67.07 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 7 (67.07 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 8 (48.1 KiB) Viewed 63 times
- Data Write Data In Pen Only Hc 0 0 2016 M Part A Solubility Of Ca Oh 2 Temperature 21 0 C Trial 1 2 3 Initial Bu 9 (26.5 KiB) Viewed 63 times
Page 2 of 5 Part B: Effect of Temperature on Solubility of Ca(OH)2 Temperature of the Boiling Ca(OH)2 solution: Trial 2 3 58.5°C Initial Buret Reading 0.00 m ( 0.00 ml 0.00ml Final Buret Reading 16.50ml 16.30 ml 16.45 ml
Page 3 of 5 TREATMENT OF DATA: 1. From Part A of the experiment, calculate the solubility (in g/L) and Ksp of Ca(OH)₂ for each trial and report the mean both values. Trial Solubility Ksp 1 3 Mean Show your calculations for Trial 1 Below: 2
Page 4 of 5 2. From the titration data in Part B, calculate the solubility of Ca(OH)₂ in units of g/L from the 2 trials as well as the mean. Part B Solubility Trial 1 2 3 Mean Show your calculations for Trial 1 From Part B Below:
Page 5 of 5 3. Comment on the solubility of Ca(OH), at the two different temperatures. Is Ca(OH)2 more soluble or less soluble at higher temperatures? Is the dissolution reaction for Ca(OH); (solid dissolving in water) an endothermic or exothermic reaction? Besides changing temperature, can you suggest one method to INCREASE the solubility of Ca(OH); in water?
Each student will be assigned to one of the 2 parts of the experiment (A or B). Once you have completed your part of the lab, collect the data for the other part from other students in your section. Part A: Solubility of Ca(OH)2 1. Using your spatula, measure 1 large scoop of Ca(OH); and transfer it into a small plastic bottle. Add about 50 mL of deionized water to the bottle. 2. Cap the bottle and swirl it occasionally for about 10 minutes to prepare the saturated calcium hydroxide solution. 3. During the 10 minutes, prepare your gravity filtration setup. Clamp a ring clamp onto your buret stand and place the funnel into the ring clamp. Then place a fluted filter paper into the funnel. Place a 250 ml. Erlenmeyer flask underneath the spout. Make sure that the tip of the spout is just inside the opening of the flask. 4. After 10 minutes, allow the solution in the plastic bottle to settle for 1 minute, then filter the solution. Pour as much of the solution into the funnel without going above the filter paper. Continue to top up the solution in the funnel as it filters. 5. When only a few drops of the liquid remain in the funnel, remove the Erlenmeyer flask and place a watch glass underneath the spout of the funnel to catch the remaining drops. Cover the top of the Erlenmeyer flask with an inverted beaker. 6. Setup a buret with the HCI titrant. Rinse the buret 2 times with a small amount of HCI. Make sure that the tip of the buret is completely filled with the HCI and there are no air bubbles present. 7. The used filter paper may be thrown into the trash. Rinse out the funnel, watch glass and plastic bottle with deionized water. 8. Using a pipet, transfer 10.00 mL of the filtered solution in the 250 ml. Erlenmeyer flask to a clean 125 mL Erlenmeyer flask. Remember to cover the 250 mL flask afterwards. Add 3 drops of bromothymol blue indicator to the solution in the 125 mL Erlenmeyer flask and titrate using the HCI. The endpoint is when the solution turns from a blue to a faint green colour. As you near the endpoint of the titration, the solution will become a lighter blue colour and the yellow colour where the titrant hits the solution spreads out farther and farther. 9. Once you have completed the first titration, clean out the 125 mL Erlenmeyer flask and repeat Step 8 two more times. The solution in the 125 mL flask can be poured down the sink.
10. Once you have completed all 3 trials, wash all glassware with soap and water and return them to the appropriate location. Any glassware with Ca(OH): dried on the side needs to be washed with an acid solution, please see the Lab Instructor or TA. Part B: Solubility of Ca(OH): at an Elevated Temperature. 1. Using your spatula, measure I large scoop of Ca(OH); and transfer it into a small plastic bottle. 2. Warm up a 50 ml graduated cylinder by adding about 50 mL of warm water from a water bath to it and then pouring the water out 3. Using the same graduated cylinder, measure another 50 ml. of warm water and then pour it into the plastic bottle. Cap the bottle. Place the bottle into the warm water bath. Swirl the bottle occasionally for about 5 minutes. 4. During this time, prepare your gravity filtration setup. Clamp a ring clamp onto your buret stand, and place the funnel into the ring clamp. Then place a fluted filter paper into the funnel. Place a 250 ml. Erlenmeyer flask underneath the spout. Make sure that the tip of the spout is just inside the opening of the flask. 5. After the 5 minutes, record the temperature of the solution in the bottle, then filter the solution. Pour as much of the solution into the funnel without going above the filter paper. Continue to top up the solution in the funnel as it filters. 6. When only a few drops of the liquid remain in the funnel, remove the Erlenmeyer flask and place a watch glass underneath the spout of the funnel to catch the remaining drops. Cover the top of the Erlenmeyer flask with an inverted beaker. Let the solution cool for about 5-10 minutes until it is slightly warm to the touch. 7. Setup a buret with the HCI titrant. Rinse the buret 2 times with a small amount of HCL. Make sure that the tip of the buret has no air bubbles inside when filling with the HCI. 8. The used filter paper may be thrown into the trash. Rinse out the funnel, watch glass and plastic bottle with deionized water. 9. Using a pipet, transfer 10.00 mL of the filtered solution in the 250 mL. Erlenmeyer flask to a clean 125 ml. Erlenmeyer flask. Remember to cover the 250 ml. flask afterwards. Add 3 dropsof bromothymol blue indicator to the solution in the 125 mL. Erlenmeyer flask and titrate usingthe HCI. The endpoint is the solution turns from a blue to a faint green colour. As you near theendpoint of the titration, the solution will become a lighter blue colour and the yellow colour where the titrant hits the solution spreads out farther and farther.
10. Once you have completed the first titration, clean out the 125 mL Erlenmeyer flask and repeat Step 9 two more times. The solution in the 125 mL flask can be poured down the sink. 11. Once you have completed all 3 trials, wash all glassware with soap and water and return them to the appropriate location. Any glassware with Ca(OH)2 dried on the side needs to be washed with an acid solution, please see the Lab Instructor or TA.