A college student is trying to determine the freezing point of an aqueous solution. He know it will be less than 0°C because of the concept of freezing point depression (water has a freezing point of 0°C, so the solution will have one lower). Here is the information he has: · Solute: Ammonium phosphate, (NH4)3PO4 , molar mass of approximately 149 g/mol . i = 4 • KĘ for water = -; -1.86 °C/m · Amount of solute: 74.5 g (NH4)3PO4 · Amount of water (solvent): 425 g H20 1) Calculate the molality (m = mol solute / kg solvent). 2) Determine the freezing point of the solution; show your work. 3) Suppose he switched the ammonium phosphate for a different solute, potassium chloride. Explain how that change would alter the freezing point. Justify your answer mathematically.
A college student is trying to determine the freezing point of an aqueous solution. He know it will be less than 0°C because of the concept of freezing point depression (water has a freezing point of 0°C, so the solution will have one lower). Here is the information he has: · Solute: Ammonium phosphate, (NH4)3PO4 , molar mass of approximately 149 g/mol . i = 4 • KĘ for water = -; -1.86 °C/m · Amount of solute: 74.5 g (NH4)3PO4 · Amount of water (solvent): 425 g H20 1) Calculate the molality (m = mol solute / kg solvent). 2) Determine the freezing point of the solution; show your work. 3) Suppose he switched the ammonium phosphate for a different solute, potassium chloride. Explain how that change would alter the freezing point. Justify your answer mathematically.
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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![A college student is trying to determine the
freezing point of an aqueous solution. He
know it will be less than 0°C because of the
concept of freezing point depression (water
has a freezing point of 0°C, so the solution will
have one lower). Here is the information he
has:
· Solute: Ammonium phosphate,
(NH4)3PO4, molar mass of approximately
149 g/mol
. i = 4
Kf for water = -1.86 °C/m
· Amount of solute: 74.5 g (NH4)3PO4
· Amount of water (solvent): 425 g H20
1) Calculate the molality (m = mol solute / kg
%3D
solvent).
2) Determine the freezing point of the
solution; show your work.
3) Suppose he switched the ammonium
phosphate for a different solute, potassium
chloride. Explain how that change would alter
the freezing point. Justify your answer
mathematically.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F169a4cfd-e6ee-4fa5-bcdd-fbf8acd2169d%2F2e966520-f36f-4f7a-b3ba-acff9bb2848b%2Fbk1e43n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A college student is trying to determine the
freezing point of an aqueous solution. He
know it will be less than 0°C because of the
concept of freezing point depression (water
has a freezing point of 0°C, so the solution will
have one lower). Here is the information he
has:
· Solute: Ammonium phosphate,
(NH4)3PO4, molar mass of approximately
149 g/mol
. i = 4
Kf for water = -1.86 °C/m
· Amount of solute: 74.5 g (NH4)3PO4
· Amount of water (solvent): 425 g H20
1) Calculate the molality (m = mol solute / kg
%3D
solvent).
2) Determine the freezing point of the
solution; show your work.
3) Suppose he switched the ammonium
phosphate for a different solute, potassium
chloride. Explain how that change would alter
the freezing point. Justify your answer
mathematically.
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