CHM 131A Lab 12-2021SP 1. HCl is a strong acid, which means that it dissociates completely in water. What is the pH of a 0.01M solution of HCI? Show your work. Explanation: 0.010 M HCl consist of: 0.010 M [H*] ions AND 0.010 M [CI ] ions 0.010M [H*]+ 0.010 M [CI' ] is not equal to total 0.010 M HCI. This is o.k.- molarity has no additive property. To obtain pH, you need [H'] ions. We established that [H']= 0.010 M. Since pH = -log[H*] ions, then what is pH? %3D Your answer:_
CHM 131A Lab 12-2021SP 1. HCl is a strong acid, which means that it dissociates completely in water. What is the pH of a 0.01M solution of HCI? Show your work. Explanation: 0.010 M HCl consist of: 0.010 M [H*] ions AND 0.010 M [CI ] ions 0.010M [H*]+ 0.010 M [CI' ] is not equal to total 0.010 M HCI. This is o.k.- molarity has no additive property. To obtain pH, you need [H'] ions. We established that [H']= 0.010 M. Since pH = -log[H*] ions, then what is pH? %3D Your answer:_
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.21QP: Aqueous Solutions of Acids, Bases, and Salts a For each of the following salts, write the reaction...
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![CHM 131A Lab 12- 2021SP
1. HCl is a strong acid, which means that it dissociates completely in water. What is the pH of a
0.01M solution of HCI? Show your work.
Explanation: 0.010 M HCI consist of: 0.010 M [H*] ions AND 0.010 M [CI' ] ions
0.010M [H*] + 0.010 M [CI ] is not equal to total 0.010 M HCI. This is o.k. – molarity has no
additive property.
To obtain pH, you need [H*] ions. We established that [H*] = 0.010 M.
Since pH = -log[H*] ions, then what is pH?
Your answer:
В.
Buffers
The purpose of a buffer is to neutralize small amounts of acid or base that is added to
maintain a certain pH. Buffers are made from weak conjugate acid-base pairs. While buffers can
maintain a neutral pH, they can also maintain any other pH depending on the salts that are used to
make it.
Set up three small Erlenmeyer flasks, one with about 10 mL of water and the others with the
same amount of buffer. Record the initial pH of each. Add about 10 drops of 0.1M HCI to each
solution and swirl to mix. Take a final pH of each solution and record the value.
After watching the Experiment fill the table:
Final pH
Change in pH
Solution
Initial pH
Water
Low pH Buffer
UCLuas added?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb1e40381-1dad-4a2e-9ce1-f1ef8f4ebc92%2Fab16481e-21c4-4d1a-ba94-3d9bd3d488f2%2Ftyzwkrg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:CHM 131A Lab 12- 2021SP
1. HCl is a strong acid, which means that it dissociates completely in water. What is the pH of a
0.01M solution of HCI? Show your work.
Explanation: 0.010 M HCI consist of: 0.010 M [H*] ions AND 0.010 M [CI' ] ions
0.010M [H*] + 0.010 M [CI ] is not equal to total 0.010 M HCI. This is o.k. – molarity has no
additive property.
To obtain pH, you need [H*] ions. We established that [H*] = 0.010 M.
Since pH = -log[H*] ions, then what is pH?
Your answer:
В.
Buffers
The purpose of a buffer is to neutralize small amounts of acid or base that is added to
maintain a certain pH. Buffers are made from weak conjugate acid-base pairs. While buffers can
maintain a neutral pH, they can also maintain any other pH depending on the salts that are used to
make it.
Set up three small Erlenmeyer flasks, one with about 10 mL of water and the others with the
same amount of buffer. Record the initial pH of each. Add about 10 drops of 0.1M HCI to each
solution and swirl to mix. Take a final pH of each solution and record the value.
After watching the Experiment fill the table:
Final pH
Change in pH
Solution
Initial pH
Water
Low pH Buffer
UCLuas added?
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