Homework Help is Here – Start Your Trial Now!
Science
Chemistry
This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to the -4 power= 1.0 X 10 to the 10 power. pH= -log (1.0 X 10 to the -10 power)= 10 I Calculate the expected pH of these three NaOH solutions, complete the table, answer the questions and email it to me at jpanek@mc3.edu. NaOH Aqueous Solution 0.10 M 0.010 M ▼ 0.0010 M Calculated expected pH Experimental pH (typical) 12.85 11.95 Answer these Questions. #1 What happens to the pH as OH- Molarity increases ? 11.05 tion hocomo

This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to the -4 power= 1.0 X 10 to the 10 power. pH= -log (1.0 X 10 to the -10 power)= 10 I Calculate the expected pH of these three NaOH solutions, complete the table, answer the questions and email it to me at jpanek@mc3.edu. NaOH Aqueous Solution 0.10 M 0.010 M ▼ 0.0010 M Calculated expected pH Experimental pH (typical) 12.85 11.95 Answer these Questions. #1 What happens to the pH as OH- Molarity increases ? 11.05 tion hocomo

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter13: Acids And Bases
Section: Chapter Questions
Problem 9RQ: What is a salt? List some anions that behave as weak bases in water. List some anions that have no...
See similar textbooks
icon
Related questions
icon
Concept explainers
Question
First read the text sections 10.5 and 10.6 on pH. This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to the -4 power= 1.0 X 10 to the 10 power. pH= -log (1.0 X 10 to the -10 power)= 10 I Calculate the expected pH of these three NaOH solutions, complete the table, answer the questions and email it to me at jpanek@mc3.edu. NaOH Aqueous Solution 0.10 M Calculated expected pH Experimental pH (typical) 0.010 M more acidic or more basic? 0.0010 M 12.85 11.95 11.05 Answer these Questions. #1 What happens to the pH as OH- Molarity increases ? #2 As OH- Molarity increases, does the solution become
Transcribed Image Text:First read the text sections 10.5 and 10.6 on pH. This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to the -4 power= 1.0 X 10 to the 10 power. pH= -log (1.0 X 10 to the -10 power)= 10 I Calculate the expected pH of these three NaOH solutions, complete the table, answer the questions and email it to me at jpanek@mc3.edu. NaOH Aqueous Solution 0.10 M Calculated expected pH Experimental pH (typical) 0.010 M more acidic or more basic? 0.0010 M 12.85 11.95 11.05 Answer these Questions. #1 What happens to the pH as OH- Molarity increases ? #2 As OH- Molarity increases, does the solution become
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
Ionic Equilibrium
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: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
Chemistry
ISBN:
9781133109655
Author:
Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:
Brooks / Cole / Cengage Learning
SEE MORE TEXTBOOKS