A sample of 12 grams of a substance that does not dissociate is dissolved in 80...
A sample of 12 grams of a substance that does not dissociate is dissolved in 80 g of water. The solution freezes at -1.94 ° C. What is the molecular weight of the substance if the cryoscopic constant for water is 1.86 ° C / m?
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A sample of 12 grams of a substance that does not dissociate is
dissolved in 80...
REVIEW QUESTIONS 1. How many grams of ethylene glycol, C,H,(OH)2, are needed per kilogram of water to protect radia...
REVIEW QUESTIONS 1. How many grams of ethylene glycol, C,H,(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -15°C? For water, the freezing point constant, Kp, is 1.86°C kg mol-! CH (OH), does not dissociate in aqueous solution, i = 1. 2. For benzene, CH, the freezing point constant, K, is 5.12°C kg mol-1 and its normal freez- ing point is 5.5°C. What is the freezing point of a solution containing 100.0 g of...
How many grams of CH_4N_2O are dissolved in a solution containing 150 grams of water which...
How many grams of CH_4N_2O are dissolved in a solution containing 150 grams of water which freezes at - 2.07 degree C? (k_f H_2O = -1.86 degree C/m)
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute...
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...
A 93.728 grams sample of compound ionized into one cation and three anions when dissolved in...
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...
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 1.20 g sample of an unknown compound is dissolved in 60.0 g of benzene. The...
A 1.20 g sample of an unknown compound is dissolved in 60.0 g of benzene. The resulting solution freezes at 4.92 degree C. Calculate the molecular weight of the unknown. Pure benzene freezes at 5.45 degree C\ K_f for benzene is 5.12 degree C/m
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g...
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing...
4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solu- tion decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why. 5. Calculate the freezing point of a 0.2 m CaCl, aqueous solution, assuming it dissociates completely to form ions in solution.
Calculate the molecular weight of a substance. In which the solution of this substance in the...
Calculate the molecular weight of a substance. In which the solution of this substance in the water has a concentration of 7 percent by weight, has a freezing point Equal to -0.89 ° C, set Kf value of water = 1.86 ° C / m
23. (10 pts.) A 93.728 grams sample of compound ionized into one cation and three anions...
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.
REVIEW QUESTIONS 1. How many grams of ethylene glycol, C,H,(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -15°C? For water, the freezing point constant, Kp, is 1.86°C kg mol-! CH (OH), does not dissociate in aqueous solution, i = 1. 2. For benzene, CH, the freezing point constant, K, is 5.12°C kg mol-1 and its normal freez- ing point is 5.5°C. What is the freezing point of a solution containing 100.0 g of...
How many grams of CH_4N_2O are dissolved in a solution containing 150 grams of water which freezes at - 2.07 degree C? (k_f H_2O = -1.86 degree C/m)
A 1.20 g sample of an unknown compound is dissolved in 60.0 g of benzene. The resulting solution freezes at 4.92 degree C. Calculate the molecular weight of the unknown. Pure benzene freezes at 5.45 degree C\ K_f for benzene is 5.12 degree C/m
4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solu- tion decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why. 5. Calculate the freezing point of a 0.2 m CaCl, aqueous solution, assuming it dissociates completely to form ions in solution.
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.
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