1. Equal numbers of moles of two soluble substances; A & B, are dissolved into 1 L of water separately. Explain the following: a) The Water samples are cooled down. Solution A freezes at -0.5°C and B at -1°C. How these solutions can have different freezing points? b) Compare the freezing point of 500 mL of solution B with the 1 L of solution A. c) Calculate the molality of the solution A & B assuming i=1 for substance A.
1. Equal numbers of moles of two soluble substances; A & B, are dissolved into 1 L of water separately. Explain the following: a) The Water samples are cooled down. Solution A freezes at -0.5°C and B at -1°C. How these solutions can have different freezing points? b) Compare the freezing point of 500 mL of solution B with the 1 L of solution A. c) Calculate the molality of the solution A & B assuming i=1 for substance A.
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
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1. Equal numbers of moles of two soluble substances; A & B, are dissolved into 1 L of water
separately. Explain the following:
a) The Water samples are cooled down. Solution A freezes at -0.5°C and B at -1°C. How
these solutions can have different freezing points?
b) Compare the freezing point of 500 mL of solution B with the 1 L of solution A.
c) Calculate the molality of the solution A & B assuming i=1 for substance A.
d) Describe the change of freezing point if you add 1 Kg of water into solution B.
e) What would be the concentrations of A & B if they have the freezing point of -0.05°C?
f) Compare the all-other colligative properties of the original solutions of A & B.
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