Suppose a student wants to determine the color change interval of an unknown indicator. Her results are given in the table. Tube # pH Unknown indicator 4 6.39 red 5 7.11 red 7.87 purple 7 8.81 purple 8 9.07 blue 9. 10.10 blue What is the interval of the unknown indicator? The color change interval is between pH 7.11 and pH 7.87. The color change interval is between pH 7.11 and pH 9.07. The color change interval is between pH 9.07 and pH 10.10. The color change interval is between pH 6.39 and pH 10.10.

Suppose a student wants to determine the color change interval of an unknown indicator. Her results are given in the table. Tube # pH Unknown indicator 4 6.39 red 5 7.11 red 7.87 purple 7 8.81 purple 8 9.07 blue 9. 10.10 blue What is the interval of the unknown indicator? The color change interval is between pH 7.11 and pH 7.87. The color change interval is between pH 7.11 and pH 9.07. The color change interval is between pH 9.07 and pH 10.10. The color change interval is between pH 6.39 and pH 10.10.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.9QE

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Similar questions

A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.
When might a pH meter be better than an indicator to determine the end point of an acid-base titration?