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vance Study Assignment: pH, Its Measurement and Applications 1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet violet Thymol blue orange Methyl yellow red What is the approximate pH of the solution? Congo red Bromcresol green violet yellow 2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH,) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.) Chapter 4: pH Measurements-Buffers and Their Properties

vance Study Assignment: pH, Its Measurement and Applications 1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet violet Thymol blue orange Methyl yellow red What is the approximate pH of the solution? Congo red Bromcresol green violet yellow 2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH,) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.) Chapter 4: pH Measurements-Buffers and Their Properties

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...
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vance Study Assignment: pH, Its Measurement and Applications 1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet Thymol blue violet orange red Methyl yellow What is the approximate pH of the solution? C. a. What is [H*] in that solution? Section 2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH,) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.) 3. The pH of a 0.10 M HOBr solution is 4.8. What Congo red Bromcresol green b. What is [OBr-]? What is [HOBr]? (Where do the H* and OBr ions come from?) violet yellow the value of K, for HOBr? What is the value of pK,? 41 M; M M 4. Formic acid, HFor, has a K, value equal to about 1.8 x 10+. A student is asked to prepare a buffer having a pH of 3.90 from a solution of formic acid and a solution of sodium formate having the same molarity. How many milliliters of the NaFor solution should she add to 20. mL of the HFor solution to make the buffer? (See discussion of buffers.) mL 5. How many mL of 0.10 M NaOH should the student add to 20 mL 0.10 M HFor if she wished to prepare a buffer with a pH of 3.90, the same as in Problem 4? mL Chapter 4: pH Measurements-Buffers and Their Properties
Transcribed Image Text:vance Study Assignment: pH, Its Measurement and Applications 1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet Thymol blue violet orange red Methyl yellow What is the approximate pH of the solution? C. a. What is [H*] in that solution? Section 2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH,) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.) 3. The pH of a 0.10 M HOBr solution is 4.8. What Congo red Bromcresol green b. What is [OBr-]? What is [HOBr]? (Where do the H* and OBr ions come from?) violet yellow the value of K, for HOBr? What is the value of pK,? 41 M; M M 4. Formic acid, HFor, has a K, value equal to about 1.8 x 10+. A student is asked to prepare a buffer having a pH of 3.90 from a solution of formic acid and a solution of sodium formate having the same molarity. How many milliliters of the NaFor solution should she add to 20. mL of the HFor solution to make the buffer? (See discussion of buffers.) mL 5. How many mL of 0.10 M NaOH should the student add to 20 mL 0.10 M HFor if she wished to prepare a buffer with a pH of 3.90, the same as in Problem 4? mL Chapter 4: pH Measurements-Buffers and Their Properties
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