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23. (10 pts.) A 93.728 grams sample of compound ionized into one cation and three anions...
23. m(10 pts.) A 93.728 grams, sample of compound ionized into one cation and three anions when dissolved in 125.214 grams of water. The freezing point of the resulting solution was found to be -6.26 °C. The freezing point constant of water is 1.86 °C /m. (a) Calculate the concentration of dissolved solutes, in molality. (b) Calculate the molar mass of the solute, in grams/mole.
A 93.728 grams sample of compound ionized into one cation and three anions when dissolved in 125.214 grams of water. The freezing point of the resulting solution was found to be -6.26 °C. The freezing point constant of water is 1.86 °C /m. (a) Calculate the concentration of dissolved solutes, in molality. (b) Calculate the molar mass of the solute, in grams/mole.
When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor, a solvent that melts at 179.5 *C and has an unusually high Kfp of 40.0 *C/molal. The freezing point of the resulting solution dropped to 176.0 *C. a. Calculate delta t fp b. Calculate the molality of the solution c. Calculate the moles of solute in the solution d. Calculate the molar mass of the compound
A researcher dissolved 1.50 grams of an unknown compound in 75.0 grams of pure cyclohexane. The freezing point of the solution was measured to be 2.70 °C. Knowing the freezing point of cyclohexane is 6.50 °C and the freezing point constant is -20.2 °C kg/mol, calculate the molar mass of the unknown compound.
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
When 12.6-grams of an unknown compound is placed in 0.116-kg of benzene, the freezing point is changed by 2.34°C. The value of Kf= 4.90°C/m for benzene. Determine the molar mass of the unknown compound. Answer to 1 decimal place and include your units. Answer: Determine the molality of a solution when 32.3 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) is dissolved in 0.947 kg of water. Answer to 2 decimal places. Answer: Find the freezing point of a...
1a: The solubility of a compound with a molecular weight of 196.7 is determined to be 24.0 g in 300.0 g of water at 398 K. Express this concentration in terms of molality. 1b: Express the concentration of the solute from the problem above as a mole fraction. 1c: The molal freezing point constant for copper is 23 °C/m. If pure copper melts at 1083°C, what will be the melting point of a brass made of 16.8 mass percent Zn...
Question #2 -/1 points How many grams of calcium nitrate need to be dissolved in 75 mL of water to form a solution that has a freezing point of -3.2 deg C? grams of calcium nitrate Evaluate Question #3 -/1 points What is the freezing point in °C) of a solution of 8.0 g of carbon tetrachloride, CCl4, in 80.0 g of benzene, C6H6. For benzene, Tp = 5.5°C and Kf = 5.12 deg kg mole?? Freezing point of solution...
Question 1. A 2.700×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL. a.)Calculate the molality of the salt solution. B.) Calculate the mole fraction of salt in this solution. C.) Calculate the concentration of...