|MadSci Network: Chemistry|
I had some trouble with this one problem because it is more wordy then most problems we are used to doing and i don't know where to start:We are asked to find the molar mass of the acid and the calculated value for the second dissociation constant for the acid given the following information. A 225- mg sample of a diprotic acid is dissolved in enough water to make 250 ml of solution. The pH of this solution is 2.06. A saturated solution of calcium hydroxide (Ksp=5.5*10^-6) is prepared by adding excess calcium hydroxide to pure water and then removing the undissolved solid by filtration. Enough of the calcium hydroxide solution is added to the solution of the acid to reach the second equivalence point(as determined by a pH meter) is 7.96. The first dissotiation constant for the acid is 5.90 * 10^-2. Assume that the volumes of the solution are additive, all solutions are at 25 degrees C and that Ka1 is at least 1000 times greater than Ka2. If you could help me through the steps i would really appreciate it. We have a test on it and i would really like to understand it
Re: Application of Aqueous Equilibria
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