cacodylic acid, (CH3)2AsO2H, a weak acid, is used in preparing buffered solutions. for the reaction pKa=6.19: (CH3)2AsO2H+H2O->H3O+(CH3)2AsO2- , calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500mL of a buffer at pH=6.6 that has a total concentration of all arsenic-containing species equal to .25M. that is (CH3)2AsO2H+(CH3)2AsO2-=.25M
one method for determining the purity of aspirin is to hydrolyze it with NaOh solution and the titrate the remaining NaOh. aspirin molar mass = 180.16g/mol. it is reacted with 2OH- and let boil for 10 min. then saliculate ion and acetate ion and water forms. a sample of aspirin with a mass of 1.427g was boiled in 50mL of .5M NaOH. after the solution was cooled, it took 31.92mL of .289M HCLto titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? why?
2007-03-06 18:57:37 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
You're not even pretending to think about this question, or posting a possible answer asking someone to check it. You're asking people to do your homework. Do your own.
2007-03-10 06:34:56 · answer #1 · answered by Some Body 4 · 0⤊ 2⤋