I\'m familiar with titrating an acid with a base, but when titrating a base with

Question

I'm familiar with titrating an acid with a base, but when titrating a base with an acid how do I find the pH of the half equivalence point if I have only the Kb value of the base I'm starting with? I know that ph at half equivalence point is equal to the pka.

11) You titrate a 50.0 mL sample of 0.150 M ethylamine, CH,CH2Nusing 0.100 M HCL. Calculate the solution pH at each of the following points in the titration: a) At the beginning, before any HCl is added b) At the halfway point of the titration; this is the point when the ethylamine is exactly half neutralized by acid addition. c) At the point when 75.0% of the ethylamine has been neutralized. d) At the equivalence point of the titration, when all of the ethylamine has been to its conjugate acid. e) After an additional 10.00 mL of HCI solution, 10.00 mL more than was necessary to completely convert the ethylamine ot its conjugate acid, have been added to the flask. Using your calculated results, sketch the titration curve for this sample. Suggest an appropriate indicator for the titration. (28 points total) Kb NH, H,o

Explanation / Answer

A:- before Pka, we would calculate Ka from the Kb value, as Ka * Kb = Kw, Ka = Kw / Kb,( Kw = 1.0 * 10-14),

so that we go for Pka value from Ka, as Pka = -logKa.

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