Lecture 2 pH and its Relevance to Biochemistry PDF
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Summary
This lecture covers pH and its importance in biochemistry, focusing on the ionization of water and the dissociation constant (Kw). It explains how [H+] and [OH-] are related in pure water, with calculations provided.
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According to the law of mass action, the ionization of water can be described by a dissociation constant, K, which is equivalent to the concentrations of the reaction products divided by the concentration of un-ionized water: Kw is the ionization constant of water: Kw is 10-14. In a sample of pure w...
According to the law of mass action, the ionization of water can be described by a dissociation constant, K, which is equivalent to the concentrations of the reaction products divided by the concentration of un-ionized water: Kw is the ionization constant of water: Kw is 10-14. In a sample of pure water, [H+] = [OH-], so [H+] and [OH-] must both be equal to 10-7M:
