a) Use the freezing point depression formula to determine the mass of solute (you see below) to make the solution with your target freezing point depression. 1.5 C = (1.86c/m) (m) (1) b) What are two factors that influence the freezing point of an aqueous solution? c) What is the molar mass of the unknowns listed below if 1.250 g of the compoundwas dissolved in 15.00 mL of water and the ∆T was found to be 1.67 °C?1. Nonelectrolyte2. An electrolyte with a van’t Hoff factor of 2
a) Use the freezing point depression formula to determine the mass of solute (you see below) to make the solution with your target freezing point depression. 1.5 C = (1.86c/m) (m) (1) b) What are two factors that influence the freezing point of an aqueous solution? c) What is the molar mass of the unknowns listed below if 1.250 g of the compoundwas dissolved in 15.00 mL of water and the ∆T was found to be 1.67 °C?1. Nonelectrolyte2. An electrolyte with a van’t Hoff factor of 2
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
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a) Use the freezing point depression formula to determine the mass of solute (you see below) to make the solution with your target freezing point depression.
1.5 C = (1.86c/m) (m) (1)
b) What are two factors that influence the freezing point of an aqueous solution?
c) What is the molar mass of the unknowns listed below if 1.250 g of the compound
was dissolved in 15.00 mL of water and the ∆T was found to be 1.67 °C?
1. Nonelectrolyte
2. An electrolyte with a van’t Hoff factor of 2
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