Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Question: Do you expect ∆S° for the dissolution of borax to be a positive or negative number? Explain your reasoning.

Question: Do you expect ∆S° for the dissolution of borax to be a positive or negative number? Explain your reasoning.

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
100%

 

Question: Do you expect ∆S° for the dissolution of borax to be a positive or negative number?
Explain your reasoning. 

 

Home Study tools My courses Мy books Career Life A student who is performing this experiment pours an 8.50 mL sample of the saturated borax solution into a 10 mL graduated cylinder after the borax solution had cooled to a certain temperature T. The student rinses the sample into a small beaker using distilled water, and then titrates the solution with a 0.500 M HCl solution. 12.00 mL of the HCI solution is needed to reach the endpoint of the titration. Calculate the value of Ksp for borax at temperature T. Expert Answer Chemtutor answered this Was this answer helpful? O 20 23,336 answers B405(OH)42- - + 2 HCI + 3 H2O => 4 B(OH)3 Moles of HCl = volume x concentration of HCI = 12.00/1000 x 0.500 = 0.006 mol Moles of B405(OH)4 = 1/2 x moles of HCl = 1/2 x 0.006 = 0.003 mol = moles/volume of B405(OH)42- = 0.003/0.0085 = 0.35294 M Na2B407.10H20 <=> 2 Na+ + B405(OH)4 + 8 H20 [Na+] = 2 x [B405(OH)4²] = 2 x 0.35294 = 0.70588 M Ksp = [Na+]°[B405(OH)4²] %3D = 0.705882 x 0.35294 = 0.176
Transcribed Image Text:Home Study tools My courses Мy books Career Life A student who is performing this experiment pours an 8.50 mL sample of the saturated borax solution into a 10 mL graduated cylinder after the borax solution had cooled to a certain temperature T. The student rinses the sample into a small beaker using distilled water, and then titrates the solution with a 0.500 M HCl solution. 12.00 mL of the HCI solution is needed to reach the endpoint of the titration. Calculate the value of Ksp for borax at temperature T. Expert Answer Chemtutor answered this Was this answer helpful? O 20 23,336 answers B405(OH)42- - + 2 HCI + 3 H2O => 4 B(OH)3 Moles of HCl = volume x concentration of HCI = 12.00/1000 x 0.500 = 0.006 mol Moles of B405(OH)4 = 1/2 x moles of HCl = 1/2 x 0.006 = 0.003 mol = moles/volume of B405(OH)42- = 0.003/0.0085 = 0.35294 M Na2B407.10H20 <=> 2 Na+ + B405(OH)4 + 8 H20 [Na+] = 2 x [B405(OH)4²] = 2 x 0.35294 = 0.70588 M Ksp = [Na+]°[B405(OH)4²] %3D = 0.705882 x 0.35294 = 0.176
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
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.
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