An aqueous solution of glycine (Mr = 75.1 g/mol) has a molality of 1.50 mol/Kg Calculate molarity of this solution and the mole fraction of glycine in the solution. Assume density of the solution to be 1.00 g/cm³. Mal fraction = 1500,0 1909 √= (1.50 x1000) X 751 Now, M = mol Volume = 1·50x1000 -

An aqueous solution of glycine (Mr = 75.1 g/mol) has a molality of 1.50 mol/Kg Calculate molarity of this solution and the mole fraction of glycine in the solution. Assume density of the solution to be 1.00 g/cm³. Mal fraction = 1500,0 1909 √= (1.50 x1000) X 751 Now, M = mol Volume = 1·50x1000 -

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.84QE

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