The image contains a chemistry problem and a response box. The problem is stated as follows:"If the \( K_b \) of a weak base is \( 2.4 \times 10^{-6} \), what is the pH of a 0.47 M solution of this base?"Below the question, there is a response box with the following input:"pH = 0.00511"This answer is marked as "Incorrect."The image does not contain any additional graphs or diagrams.

Given : Initial concentration of weak base B = 0.47 M Kb of base = 2.4 X 10-6 Since B is a weak base. Hence it will undergo hydrolysis as per the reaction, => B (aq) + H2O (l) --------> BH+ (aq) + OH- (aq) Assuming y concentration of B is ionised in the reaction. Hence the concentration of ions produced in the reaction are, => [BH+ ] = y = [OH- ] And the concentration of B remaining in the solution, [B] = Initial - ionised = 0.47 - y Since Kb <<< 1. Hence we can assume negligible concentration of B will ionise. Hence [B] = 0.47 - y = 0.47 M approx.The ionisation constant expression for the reaction can be written as, => Kb = [BH+] [OH-][B]Hence substituting the values we get,=> 2.4 X 10-6 = y X y0.47=> y = [OH- ] = 2.4 X 10-6 X 0.47 = 1.062 X 10-3 M approx. Hence pH = 14 + log[OH- ] = 14 + log(1.062 X 10-3 ) = 11.03 approx.

Answered: If the Kp of a weak base is 2.4 x 10-6,…

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If the Kp of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH 0.00511 Incorrect

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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