Answered: A student titrates a weak acid with…

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter4: Stoichiometry Of Chemical Reactions

Section: Chapter Questions

Problem 79E: Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.08 11 M NaOH to reach the end point....

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Question

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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