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5th bullet point. We dissolved a solid in a liquid so I would think the Delta S would be positive but it turned out to be negative.. Having a hard time understanding why.

5th bullet point. We dissolved a solid in a liquid so I would think the Delta S would be positive but it turned out to be negative.. Having a hard time understanding why.

EBK A SMALL SCALE APPROACH TO ORGANIC L
EBK A SMALL SCALE APPROACH TO ORGANIC L
4th Edition
ISBN:9781305446021
Author:Lampman
Publisher:Lampman
Chapter79: Solubility
Section: Chapter Questions
Problem 1P
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5th bullet point. We dissolved a solid in a liquid so I would think the Delta S would be positive but it turned out to be negative.. Having a hard time understanding why. 

ration.) Filter the saturated solution to remove any undissolved solid, and measure out 5.0 mL of the filtered saturated solution for each titration. Keep the temperature as close to 100 °C as possible when filtering, but it can be titrated at a cooler temperature. (Why?) Perform at least two titrations at both temperatures. Discard all waste into a waste beaker, then neutralize before disposal in the sink. Calculations/Questions to address in the Discussion Section Calculate the molar solubility and Ksp of Ca(OH)2 at room temperature and at 100 °C. Calculate AG° for the dissolution of Ca(OH)2 at room temperature and at 100 °C. Assuming that they are constant with temperature, calculate AH° and AS° for the dissolution of calcium hydroxide in water. How does your value of Ksp at 25 °C compare to the literature value? (use the textbook) How do you account for any difference? experimental Ksp: 2.3 × 10-5 Ksp from textbook = 1.3 x 10-6 using the Compare your experimental values for AH°, AS°, and AGO to the theoretical values calculated thermodynamic data in Appendix G. Discuss what the sign of each value tells you about the process of dissolving Ca(OH)2 in water. Carbon dioxide (CO2) is a component of air that readily dissolves in water, where it will react with Ca(OH)2 to form CaCO3. Why was it a good idea to boil the water for the high temperature determination before adding the solid calcium hydroxide? Would you expect that dissolved CO2 would have any effect on your Ksp measurements? Previous studies have shown that the complex ion Ca(OH)* can be present in a solution of calcium hydroxide at fairly significant concentrations (20-40% those of Ca²+). How would this affect your solubility measurements? between the have solid owe so tha not what yo Wempette ers graphs or c bserations, tren relat cedure of t and on a se hat they me pport your re your find investiga te your un at.
Transcribed Image Text:ration.) Filter the saturated solution to remove any undissolved solid, and measure out 5.0 mL of the filtered saturated solution for each titration. Keep the temperature as close to 100 °C as possible when filtering, but it can be titrated at a cooler temperature. (Why?) Perform at least two titrations at both temperatures. Discard all waste into a waste beaker, then neutralize before disposal in the sink. Calculations/Questions to address in the Discussion Section Calculate the molar solubility and Ksp of Ca(OH)2 at room temperature and at 100 °C. Calculate AG° for the dissolution of Ca(OH)2 at room temperature and at 100 °C. Assuming that they are constant with temperature, calculate AH° and AS° for the dissolution of calcium hydroxide in water. How does your value of Ksp at 25 °C compare to the literature value? (use the textbook) How do you account for any difference? experimental Ksp: 2.3 × 10-5 Ksp from textbook = 1.3 x 10-6 using the Compare your experimental values for AH°, AS°, and AGO to the theoretical values calculated thermodynamic data in Appendix G. Discuss what the sign of each value tells you about the process of dissolving Ca(OH)2 in water. Carbon dioxide (CO2) is a component of air that readily dissolves in water, where it will react with Ca(OH)2 to form CaCO3. Why was it a good idea to boil the water for the high temperature determination before adding the solid calcium hydroxide? Would you expect that dissolved CO2 would have any effect on your Ksp measurements? Previous studies have shown that the complex ion Ca(OH)* can be present in a solution of calcium hydroxide at fairly significant concentrations (20-40% those of Ca²+). How would this affect your solubility measurements? between the have solid owe so tha not what yo Wempette ers graphs or c bserations, tren relat cedure of t and on a se hat they me pport your re your find investiga te your un at.
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