Answered: A student titrates a weak acid with…

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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A student titrates a weak acid with 0.100 M NaOH, adding 34.84 mL before a dark pink color is seen. Realizing that the end point has been passed, he then adds 3.19 mL 0.0500 M HCl until the solution is neutralized.

How many moles of H⁺ were present in the initial weak acid solution?

Expert Solution

Step 1

Calculation of no. of mol of NaOH:

$\begin{array}{rcl} No . of mol & = & Molarity \times Volume \\ = & 0.100 mol / L \times 34.84 \times 10^{- 3} L \\ = & 3.484 \times 10^{- 3} mol \end{array}$

Calculation of no. of mol of HCl added:

$\begin{array}{rcl} No . of mol & = & Molarity \times Volume \\ = & 0.0500 mol / L \times 3.19 \times 10^{- 3} L \\ = & 0.1595 \times 10^{- 3} mol \end{array}$

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