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3. Give a specific reason(other than general human error) why the calculated pH values are not exactly the same as the experimental values obtained by measuring with a pH meter.

3. Give a specific reason(other than general human error) why the calculated pH values are not exactly the same as the experimental values obtained by measuring with a pH meter.

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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This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCl pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 Calculated pH Answer these questions. 2.15 3.08 As the H+ Molarity increases, what to the pH ? As the H+ Molarity increases does the solution become more acidic or more basic? 3. Give a specific reason(other than general human error) why the calculated pH values are not exactly the same as the experimental values obtained by measuring with a pH meter.
Transcribed Image Text:This is a Dry Lab since we cannot meet on Campus. You would have first calibrated a pH meter and then measured the pH of four different Acid Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong acid HCI solutions by assuming that the HCI is 100% ionized or dissociated when dissolved in water and thus Molarity HCI equals the Molarity H+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 power M HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function of your calculator to get the answer. Create a data table like this one and put your calculated HCl pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 Calculated pH Answer these questions. 2.15 3.08 As the H+ Molarity increases, what to the pH ? As the H+ Molarity increases does the solution become more acidic or more basic? 3. Give a specific reason(other than general human error) why the calculated pH values are not exactly the same as the experimental values obtained by measuring with a pH meter.
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