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follows that weak bases are weak electrolytes. ─
As with weak acids, the concentration of hydroxide ions , OH , in a solution of a weak base is much smaller than if the same amount of strong base had been dissolved. Although the Arrhenius definitions of acids and bases have proved very useful, the theory is restricted to the situation of aqueous solutions. 4 Chemistry 52 EXPERIMENT #2 In 1923 new definitions of acids and bases were proposed simultaneously by Bronsted and Lowry. The Bronsted/Lowry theory of acids and bases extends the Arrhenius definitions to more general situations, which explain the behavior of weak bases and do not require the solvent to be water. According to the Bronsted/Lowry theory: AN ACID: +
Is a proton, H , donor A BASE: +
Is a proton, H , acceptor AN ACIDBASE REACTION (NEUTRALIZATION REACTION) IS THE +
TRANSFER OF A H +
H ACID + BASE ¾¾¾¾¾> SALT + WATER +
H HCl(aq) + NaOH(aq) ¾¾¾¾¾> NaCl(aq) + H2O(l) In summary, both acids and bases have characteristic properties and can either strong or weak, as shown below: ACIDS BASES...
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