Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question

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.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Analyzing and Predicting Spectroscopic Data
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS