Answered: Calculate the analytical molar…

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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Question

Calculate the analytical molar concentrations of trichloroacetic acid in an aqueous solution that contains 152.9 mg of trichloroacetic acid,Cl₃CCOOH (163.4 g/mol), in 19.3 mL (the acid is 73% ionized in water). Indicate units

Expert Solution

Step 1

Analytical molar concentration of a solution refers to the initial number of moles of a solute in 1 L of the solution. So, it doesn't matter how much the reactant reacts to evaluate the analytical molar concentration.

Step 2

Given:
Mass of solute (chloroacetic acid) in the solution = 152.9 mg = 152.9 X 10^-3 g

Molar mass of solute = 163.4 g/mol

Volume of solution = 19.3 mL = 19.3 X 10^-3 L

Thus, analytical molar concentration of the solution:

$M = \frac{n u m b e r o f m o l e s o f s o l u t e}{V o l u m e o f s o l u t i o n} = \frac{m a s s o f s o l u t e}{m o l a r m a s s o f s o l u t e \times v o l u m e o f s o l u t i o n} = \frac{152.9 \times 10^{- 3} g}{163.4 g / m o l \times 19.3 \times 10^{- 3} L} = 0.048 m o l / L = 0.048 M$

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