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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 -

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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dl 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 √= (1.50×1000) X 75-1 = 19019 78. Now, M = moj Volume =1.50×1000
Transcribed Image Text:dl 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 √= (1.50×1000) X 75-1 = 19019 78. Now, M = moj Volume =1.50×1000
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