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CSU CHEM 113 - Bronsted-Lowry acid-base definition

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CHEM 113 1nd Edition Lecture 18 Outline of Last Lecture I. Arrhenius Acid-Base EquilibriaII. Strong and Weak AcidsIII. Strong and Weak BasesIV. Acid Dissociation ConstantV. Autoionization of waterVI. The pH ScaleOutline of Current Lecture - Bronsted-Lowry acid-base definitiono Acido Baseo Conjugate Acid-Base PairsCurrent Lecture- Bronsted-Lowry acid-base definitiono Many substances that yield OH- ions in water do not contain OH in their formula. Therefore the Arrhenius definition does not encompass all acids and bases so we have another definition.o An acid is a proton donor, any species that donates an H+ ion. An acid must contain H in its formulao A base is a proton acceptor, any species that accepts and H+ ion A base must contain a lone pair of electrons to bond to H+o An acid-base reaction is a proton-transfer processThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute. This process occurs when an acid dissolves in water because the water molecules act as a proton acceptor. The process also occurs when a base is dissolved in water except the water molecules act as proton donors- See Figure 18.7 on page 729o This definition is a new way to look at these reactions because it focuses on both the reactants and the products as acids and bases.  Conjugate Acid-Base Pairs- Every acid has a conjugate base and every base has a conjugate acid- The conjugate base has one fewer H and one more minus charge than the acid.- The conjugate acid has one more H and one fewer minus charge than the base. - See Table 18.4 for a visual representation of pairing- Sample Problem 18.4 is good practice of this


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