Additional Aspects of Acid-Base Equilibria

17-2 Buffer Solutions 17-3 Acid-Base Indicators 17-4 Neutralization Reactions and Titration Curves [Pg.789]

17-5 Solutions of Salts of Polyprotic Acids 17-6 Acid-Base Equilibrium Calculations A Summary [Pg.789]

NaOH(aq) is slowly added to an aqueous solution containing HCI(aq) and the indicator phenolphthalein. The indicator color changes from colorless to red as the pH changes from 8.0 to 10.0. The equivalence point of the neutralization is reached when the solution turns a lasting pink (the pink seen here disappears when the flask is swirled to mix the reactants). The selection of indicators for acid-base titrations is one of the topics considered in this chapter. [Pg.789]

1 Explain what is meant by the common-ion ettect and how it relates to Le Chatelier s principle. [Pg.789]

2 Explain how a buffer solution is able to resist attempts to change its pH. [Pg.789]

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