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Ch. 25 Fluid, Electrolyte, and Acid-Base Homeostasis
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All textbooksErin C. Amerman 2nd EditionCh. 25 Fluid, Electrolyte, and Acid-Base HomeostasisProblem 25.13a

Chapter 25, Problem 25.13a

Explain what happens to the pH of a buffered solution when hydrogen ions are added. Why does this happen?

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Hi, everyone. Let's take a look at this question together in a buffer containing a weak acid and its conjugate base. The hydrogen ions will react with the conjugate base to form. What is it? Answer choice. A, a strong acid. Answered choice B A strong base. Answer choice C A weak acid or answer choice D A weak base. Let's work this problem out together to try to figure out which of the following answer choices will be formed when the hydrogen ions react with the conjugate baits. So in order to solve this question, we have to recall what we have learned about buffer solutions and the reaction between the hydrogen ions and the conjugate base, which we can recall that buffer solutions work to help resist changes in Ph. And here we have a buffer solution containing a weak acid and a conjugate base in which the weak acid or the H A donates protons or hydrogen ions to the solution and the conjugate base accepts protons. So in the case of hydrogen ions reacting with the conjugate base, we know that when we have additional hydrogen ions in the solution, those additional hydrogen will react with the conjugate base to form a weak acid. As the weak acid donates protons, the conjugate base will accept those protons and form a weak acid. Which means that answer choice. C weak acid is the correct answer. And all other answer choices are incorrect. I hope you found this video to be helpful. Thank you and goodbye.
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