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calculate the Ph of 1.00L of the buffer solution 0.80M CH3NO2/ 1.0M CH3NH3CL before and after the addition of a) 0.070 mol NaOh and b) 0.11 mol HCl.

calculate the Ph of 1.00L of the buffer solution 0.80M CH3NO2/ 1.0M CH3NH3CL before and after the addition of a) 0.070 mol NaOh and b) 0.11 mol HCl.

Chemistry
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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calculate the Ph of 1.00L of the buffer solution 0.80M CH3NO2/ 1.0M CH3NH3CL before and after the addition of a) 0.070 mol NaOh and b) 0.11 mol HCl. 

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Step 1

Solution -

According to the question -
Given -
pH of the buffer before the addition of base oracid
Kb of CH3NH2 =4.4*10-4
Ka = 1.0*10-14/ 4.4*10-4 =2.27*10-11
pKa = -logKa = 10.643
pH = pKa + log[base] / [acid]
        = 10.643 +log[0.80]/[1.0M] = 10.643-0.0969 = 10.546
After the addition of NaOH
               CH3NH3+(aq) +OH-(aq) ------> CH3NH2(aq) +H2O(l)
Initial mol 1.0                     0.070                   0.80
final          -0.070               -0.070                +0.070
eq         0.93                            0                    0.870
Ka = [ CH3NH2][H+] /[CH3NH3+]
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