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 HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 3.08 Calculated pH Answer these questions. hat happens to the pH ? As the HF Molarity increases does the solution become basic? 2.15 Melarity i V a primeter. calculated pri not exactly the same as the experimental values obtained by measuring with 4. Given that the experimental pH of a 0.1 Molar Acetic Acid (CH3COOH) solution is 2.89 compared to the experimental pH of 1.20 for the 0.1 Molar HCI solution, A) Which solution is more acidic and how do you know that, based on the pH measurements)?

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 HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.01 M 0.001 M Experimental pH (given) 1.20 3.08 Calculated pH Answer these questions. hat happens to the pH ? As the HF Molarity increases does the solution become basic? 2.15 Melarity i V a primeter. calculated pri not exactly the same as the experimental values obtained by measuring with 4. Given that the experimental pH of a 0.1 Molar Acetic Acid (CH3COOH) solution is 2.89 compared to the experimental pH of 1.20 for the 0.1 Molar HCI solution, A) Which solution is more acidic and how do you know that, based on the pH measurements)?

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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