pH and Buffers

Mr. Andersen explains the importance of maintaining a specific pH range in blood to prevent protein denaturation. He describes how buffer systems, composed of weak acids and their conjugate bases, help stabilize pH levels. The video covers the relationship between pH and pKa, the role of equilibrium constants, and the application of Le Chatelier's principle. It also discusses the significance of buffer capacity and the biological importance of buffers, using examples like acid/base indicators and amino acids.

How does Le Chatelier's principle apply when adding strong acids or bases to a buffer solution?

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What is the significance of equal concentrations of weak acid and its conjugate base in a buffer?

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How do changes in pH relate to the behavior of amino acids in proteins?

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