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.
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A 93.728 grams sample of compound ionized into one cation and three anions when dissolved in...
23. (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.
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.
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
6. A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor. The resulting solution melted at 176.0 C. What is the molecular mass of the compound? The melting point of pure camphor is 179.5 C. The freezing-point-depression constant for camphor Kf is 40.0 C/m. 7. A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at...
(6 pt) 4 A 1.07-mg sample of a non-ionic compound was dissolved in 78.1 mg of camphor, a solvent that melts at 179.5°C and has an unusually high Kr of 40.0 mola If the freezing point of the solution is 176.0°C: a) Calculate AT, then determine the molality (m) of this solution: b) Calculate the moles of solute in this solution: e) Calculate the molar mass ()of e coound:
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1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...
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...