Lecture 3 - Lecture 3 Chapter 8 Acids and Bases Chapter 9...

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Anal Chem 251 Lect 3 1 Lecture 3 Chapter 8: Acids and Bases Chapter 9: Buffers
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Anal Chem 251 Lect 3 2 Summary of Acids,Bases and Buffers pH = -log [H + ] pOH = -log [OH - ] • pK a = -log [K a ] pH + pOH = pK w = 14 at 25 C pH of a buffer = pK a + log [A-]/[HA]
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Anal Chem 251 Lect 3 3 Classical Definition (Arrhenius) of Acids and Bases In the classical definition, acids and bases are defined according to their formulas and their behavior in water: An acid is a substance that has H in its formula and dissociates in water to yield H 3 O + • A base is a substance that has OH in its formula and dissociates in water to yield OH - When an acid and a base react, they undergo neutralization
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Anal Chem 251 Lect 3 4 The hydrated proton, hydronium ion, H 3 O + . Figure 4.4 The proton bonds covalently to one of the lone pairs of a water molecule’s O atom to form a hydronium ion, H 3 O + , which H bonds to several other water molecules.
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Anal Chem 251 Lect 3 5 Structure of hydronium ion, H 3 O +
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