The freezing point depression constant (Kf) of acetic acid is 3.90 \deg Ckg/mol. Using this value and the freezing point data (remember that what we care about is the difference in freezing point!) calculate the molality of the 2nd trial.
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- COLLIGATIVE PROPERTIES: SMART WORKSHEET PART I. DETERMINING THE FREEZING POINT OF WATER PART 1.1 The expression for the freezing point depression of a solution relative to that of the pure solute is shown by the following equation: ATƒ = i × Kƒ × m From solutions of known concentrations of sodium chloride in water, you determine Kƒ, the freezing point depression constant of water. What assumption is necessary in order to do these calculations? Necessary assumption for these calculations i=1 AWhen 2.43 g of a certain molecular compound X are dissolved in 65. g of formamide (NH₂COH), the freezing point of the solution is measured to be -0.4 °C. Calculate the molar mass of X. If you need any additional information on formamide, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 43.33 g L.. The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 3.1 g.1.¹. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Round each of your answers to 2 significant digits. 0% 0.8 X 5
- May you please do question one and two.In the determination of molecular weight through freezing point depression analysis. The volume of cyclohexane is 29.1 mL. Calculate the mass of cyclohexane(d=0.7786g/mL in grams.2. You have a solution that contains 4.0g of oxalic acid dissolved in 100 mL of water. This solution is placed in a separatory funnel, and then 100 mL of diethyl ether is added to the separatory funnel and an extraction is performed. (Diethyl ether and water are immiscible solvents.) Use the following constants to calculate how much oxalic acid is in each solvent after the extraction. Solubility of oxalic acid in water = 9.5 g / 100 mL Solubility of oxalic acid in ether = 16.9 g/100 mL
- Calculate the values for log Kow and the saturated aqueous solubility (Cw$sat) for bisphenol A. The value for log Kow is 3.62 ; enter your answer as X.XX The value for Cwsat is ; report your answer in units of moles/liter and enter it as X.XX×10(-X). Bisphenol A is closest to "phthalates" H3C CH3 HO HO,Using a solution freezing point to calculate a molar mass.When 5.31 g of a certain molecular compound X are dissolved in 70. g of formamide (NH,COH ), the freezing point of the solution is measured to be 1.9 °C. Calculate the molar mass of X. If you need any additional information on formamide, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. 미미
- Can you please do question number 2A CHM 126 student followed a modified procedure similar to the one described in the "Determination of Molar Mass by Freezing Point Depression" experiment. The student's data is listed below. Using the data, determine the molar mass of the solute. freezing point depression constant for solvent = 8.1186 °C/m mass of solvent = 4.8810 g mass of solute 0.2100 g !! freezing point of pure solvent 24.231 °C freezing point of solution = 21.571°C Type your answer in the space below without the units.What is the freezing point (°C) of a solution prepared by dissolving 13.5 g of (NH4)2SO4 (formula weight = 132 g/mol) in 100 g of water? The molal freezing point depression constant for water is 1.86°C/m. Assume complete dissociation in solution. Express your answer in decimal notation and to 2 decimal places, without units.