(a) Write the chemical reactions whose equilibrium constants are Kb and Ka for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imidazole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HClO4 are added. (d) How many milliliters of 1.07 M HClO4 should be added to 1.00 g of imidazole to give a pH of 6.993?
CHAPTER 17 ADDITIONALASPECTS FO AQUEOUS EQQUILIBRIA *picture is of yellow stone national park 17.1 THE COMMON ION EFFECT Soluble ionic compounds are strong electrolytes, they dissociate completely Dissociation of the weak acid decreases when a strong electrolyte is added (it has a common ion) Common-ion effect- the extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte the ionization of a weak base is decreased by the addition of a common ion + o ex. NH (a4 from the strong electrolyte NH Cl) ca4ses the base dissociation equilibrium of the NH t3 shift to the left, decreasing equil