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11 Nov 2019
The solute is acetone. The density of acetone is .791g/ml. The solvent is acetic acid. The density of the solvent is 1.049 g/ml.
In an experiment using acetic acid as a solvent the following values were obtained: T_f (acetic acid) = 16.1 degree C T_f (with 3 mL of solute in 10 mL of acetic acid) = 2.5 degree C a. Calculate the molecular mass of this hypothetical solute, using this data. (K acetic acid = 3.9 degree C middot kg/mol) b. You notice that you made a mistake in finding T_f and that the correct value of T_f (with 3 mL of solute) = -3.0 degree C. Calculate the new molecular weight of this solute, what can you conclude about the importance of determining temperature accurately in this experiment? What is the freezing point of a 1.8 (mass/mass)% glucose solution (aqueous)? An aqueous solution of 0.9 (mass/mass)% NaCl this solution? is isotonic with blood. What is the freezing point of this solution?
The solute is acetone. The density of acetone is .791g/ml. The solvent is acetic acid. The density of the solvent is 1.049 g/ml.
In an experiment using acetic acid as a solvent the following values were obtained: T_f (acetic acid) = 16.1 degree C T_f (with 3 mL of solute in 10 mL of acetic acid) = 2.5 degree C a. Calculate the molecular mass of this hypothetical solute, using this data. (K acetic acid = 3.9 degree C middot kg/mol) b. You notice that you made a mistake in finding T_f and that the correct value of T_f (with 3 mL of solute) = -3.0 degree C. Calculate the new molecular weight of this solute, what can you conclude about the importance of determining temperature accurately in this experiment? What is the freezing point of a 1.8 (mass/mass)% glucose solution (aqueous)? An aqueous solution of 0.9 (mass/mass)% NaCl this solution? is isotonic with blood. What is the freezing point of this solution?
Keith LeannonLv2
3 Sep 2019