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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 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:_

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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?
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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