Data Set Exp.5 Use the following data to determine the mass percent of the active ingredient in Aspirin a) Preparation of solutions: volume of salicylic acid volume of FECL3 solution SA1 1ml 9ml SA2 3.5ml 6.5ml SA3 6.5ml 3.5ml SA4 1ml 9ml The concentration of salicylic acid= 0.000725M b) Preparation of “STOCK ASA UNKNOWN" The mass of aspirin= 0.135 g The volume of stock solution of aspirin= 100ml The dilution factor for the stock solution= 50/2 Molar mass of SAS = 180.157 g/mole c) Measurements of Absorbance: Solution Absorbance SA1 0.154 SA2 0.524 SA3 0.789 SA4 0.989 The unknown sample 0.259

A:If 100 mL of a 0.15 M Mg(NO3)2(aq) solution has a density of 1.09 g/mL, which of the following statements is false? Group of answer choices The mass of Mg(NO3)2 in this solution can be determined from this information. If the solution density was not given, it is usually reasonable to assume 1.00 g/mL The mass of the water in this solution is 109 g It is possible to determine the mole fraction of water in this solution.   B: In the body, cell membranes act like semipermeable membranes discussed in class.  If a red blood cell is surrounded by fluid with a higher electrolyte concentration than what is inside the cell, which of the following statements is true? Group of answer choices The cell will shrink because water will pass from the inside of the cell to the fluid The surrounding fluid has a lower osmotic pressure than what is inside the cell The cell will swell up because water will pass from the fluid to the inside of the cell Nothing will happen to the…

a 50.0 mL sample of aqueous sodium chloride was analyzed according to the experimental procedure in part E and the following data were obtained. mass of evaporating dish: 37.628 g  mass of evaporating dish + solution: 86.623 g  mass of evaporating dish + solid NaCl: 41.133 g A) Calculate the percent by mass NaCl in the solution. B) Calculate the Molarity of the solution. C) Calculate the molality of the solution.

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