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In the laboratory, a student adds 24.2 g of ammonium chloride to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of ammonium chloride, the ammonium ion and the chloride ion in the solution. [NH4CI] = M [NH4 = M [CI]

In the laboratory, a student adds 24.2 g of ammonium chloride to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of ammonium chloride, the ammonium ion and the chloride ion in the solution. [NH4CI] = M [NH4 = M [CI]

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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In the laboratory, a student adds 24.2 g of ammonium chloride to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of ammonium chloride, the ammonium ion and the chloride ion in the solution. [NH4CI] = M [NH,1 M [CI] ||||
Transcribed Image Text:In the laboratory, a student adds 24.2 g of ammonium chloride to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of ammonium chloride, the ammonium ion and the chloride ion in the solution. [NH4CI] = M [NH,1 M [CI] ||||
Expert Solution
Step 1

Given - mass of ammonium chloride = 24.2 g 

And, mass of the solution = 500 mL 

 

Then , Molarity of the solution can be determined by using following formula - 

Molarity = (mass of Solute×1000)/(molar mass of Solute×volume of Solution) 

 

Mass of solute , ammonium chloride = 24.2 g 

Molar mass of ammonium chloride = 53.491 g/mol 

Volume of Solution = 500 mL

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