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 wotor
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 wotor
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
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Chapter16: Acids And Bases
Section: Chapter Questions
Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...
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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 HCI pH values in the table.
HCI Solution Molarity: 0.1 M
0.001 M
Experimental pH (given) 1.20
Calculated pH
Answer these questions.
1. As the H+ Molarity increases what happens to the pH2
2. AST + Molarity in
basic?
alues are
a pH meter.
0.01 M
2.15
3.08
ore
AYWhich solution is more acidic and how do you know that, based on the pH
easurements)?
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,
with
B) Explain why the solutions are of different acidity based on the fact that in water
HCI is a strong acid whereas CH3COOH is a weak acid and their relative extent of
ionization(dissociation) is quite different. A strong acid is 100% ionized to H+ and its
HA → H+. + A-. A weak acid is only ionized
conjugate base as represented
slightly.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3c0144e-0a71-4a75-9786-affbea18251d%2F722a282c-910d-48a5-9e58-0759d8c5fe9e%2F9ldd31nq_processed.jpeg&w=3840&q=75)
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 HCI pH values in the table.
HCI Solution Molarity: 0.1 M
0.001 M
Experimental pH (given) 1.20
Calculated pH
Answer these questions.
1. As the H+ Molarity increases what happens to the pH2
2. AST + Molarity in
basic?
alues are
a pH meter.
0.01 M
2.15
3.08
ore
AYWhich solution is more acidic and how do you know that, based on the pH
easurements)?
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,
with
B) Explain why the solutions are of different acidity based on the fact that in water
HCI is a strong acid whereas CH3COOH is a weak acid and their relative extent of
ionization(dissociation) is quite different. A strong acid is 100% ionized to H+ and its
HA → H+. + A-. A weak acid is only ionized
conjugate base as represented
slightly.
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