Question

Determine the K_b of a weak base if a 0.52 M solution of the base has a pH of 10.68 at 25°C.

K_b = ? × 10 ?
(Enter your answer in scientific notation.)

Answer 1

Answer given pH = 10.68 pol = 14-10.68 = 3132 .: [OH] = 10 3:32 = 4178x169 cm ase B. who Let the us considen dissociation the weak of B is B + H2O 6652 0 - initial. BH+ + OH- 0 0 tac tac ac me degree Change . -ac Equlibrinm c(1-2) ac Lago dissociation i Kb = ad/x&C (1-2) Kb = Since & <<<1 so lani 1-2 ar, Kb = are w, a = the Now, [OH-] = armoire ar cs Scanned with = VKDCE koxc = [OH-] ? Ko = [OH-] CamScanner

given . c = 0.52 M a kb 2 (4.78*10-4.72 is 0.52 = 4.39 X 107 oko= 4:39 x 107 cs Scanned with CamScanner