Answered: Consider the titration of 15.0 mL of…

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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Consider the titration of 15.0 mL of 0.140 M Na A (a weak base) and 0.100 M H Cl. Calculate the pH of the solution after 44.0 mL of H Cl has been added. The K b of the base is 1.01E-4

To avoid rounding errors report your answer with two decimal places.

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Step 1

Number of moles of NaA = 0.015 × 0.14 = 0.0021 mol

Number of moles of HCl = 0.1 × 0.044 = 0.0044 mol

0.0021 mol of NaA reacts with 0.0021 mol of HCl to form 0.0021 mol of HA (weak acid) and 0.0021 mol of NaCl (neutral). The remaining number of moles of HCl in the final solution is equal to 0.0044 – 0.0021 = 0.0023 mol. The pH value of the solution is due to the hydrogen ion released from the weak acid HA and strong acid HCl.

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