Homework Help is Here – Start Your Trial Now!
Science
Chemistry
How will Le Chatlier’s Principle be used to?      a. Cause a color change for an indicator in Part A      b. Cause an insoluble salt to become more soluble

How will Le Chatlier’s Principle be used to?      a. Cause a color change for an indicator in Part A      b. Cause an insoluble salt to become more soluble

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

How will Le Chatlier’s Principle be used to?
     a. Cause a color change for an indicator in Part A
     b. Cause an insoluble salt to become more soluble

A. Acid-Base Indicators There is a large group of chemical substances, called acid-base indicators, which change color in solution when [H] changes. A typlcal substance indicator like this is called methyl violet, which we will give the formula HMV. In solution HMV dissociates as follows: HMV(aq) yellow H(aq) + MV (aq) violet (5) HMV has an intense yellow color, while the anion MV is violet. The color of the indicator in solution depends very strongly on [H"]. 1. Add about 5 mL of distilled water to a regular (18 x 150 mm) test tube. Add 3-5 drops. of methyl violet indicator. Record the color of the solution in your notebook. 2. How could you force the equilibrium system to go to the other form (color)? Select a reagent (something that adds H or removes H") that should do this and add it to the solution, drop by drop, until the color change is complete. Record your observations in your notebook. If there is no color change, try another until reagent you find one that does. Work with 6 M reagents if they are available. . 3. Equilibrium systems are reversible. That is, the reaction can be driven to the left and right by changing the conditions in the system. How can you force the system in Step 2 to revert to its original color? Select a reagent that should do this and add it drop by drop until the color has become the original one. Again, if your first choice was incorrect, try another reagent. Record everything in your notebook. 4. Answer all the questions for Part A in the data section before going on to Part B.
Transcribed Image Text:A. Acid-Base Indicators There is a large group of chemical substances, called acid-base indicators, which change color in solution when [H] changes. A typlcal substance indicator like this is called methyl violet, which we will give the formula HMV. In solution HMV dissociates as follows: HMV(aq) yellow H(aq) + MV (aq) violet (5) HMV has an intense yellow color, while the anion MV is violet. The color of the indicator in solution depends very strongly on [H"]. 1. Add about 5 mL of distilled water to a regular (18 x 150 mm) test tube. Add 3-5 drops. of methyl violet indicator. Record the color of the solution in your notebook. 2. How could you force the equilibrium system to go to the other form (color)? Select a reagent (something that adds H or removes H") that should do this and add it to the solution, drop by drop, until the color change is complete. Record your observations in your notebook. If there is no color change, try another until reagent you find one that does. Work with 6 M reagents if they are available. . 3. Equilibrium systems are reversible. That is, the reaction can be driven to the left and right by changing the conditions in the system. How can you force the system in Step 2 to revert to its original color? Select a reagent that should do this and add it drop by drop until the color has become the original one. Again, if your first choice was incorrect, try another reagent. Record everything in your notebook. 4. Answer all the questions for Part A in the data section before going on to Part B.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Basics of Titrimetric Analysis
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
  • SEE MORE 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