What is the boiling point of a mixture composed of 90.0 g HOCH2CH2OH (ethylene glycol, MM=...
What is the boiling point of a mixture composed of 90.0 g HOCH2CH2OH (ethylene glycol, MM= 62.068 g/mol) and 120.0 g H2O? The boiling point elevation constant for H2O is 0.512 °C/m. Boiling point of a pure water under the same condition is 100.0°C.
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What is the boiling point of a mixture composed of 90.0 g
HOCH2CH2OH (ethylene glycol, MM=...
What is the freezing point and boiling point in Celsius of a solution 400 g of...
What is the freezing point and boiling point in Celsius of a solution 400 g of ethylene glycol (MW=62 g/mol) dissolved in 500 g of water? The molal freezing point depression constant for water is 1.86 C/m The molal boiling point elevation constant of water is 0.512 C/m Please explain steps
A solution is prepared by dissolving 7.8 g of ethylene glycol (HOCH2CH2OH) in 50.0 g of...
A solution is prepared by dissolving 7.8 g of ethylene glycol (HOCH2CH2OH) in 50.0 g of water to produce 56.9 mL of solution. Ethylene glycol is non-volatile. a. What is the vapor pressure of the solution at 100oC? b. What is the boiling point of the solution? Kb = 0.51 oC/m
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of...
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of ethylene glycol with a density of 1.0087 g/mL. The freezing point depression constant for water (which you can assume is the solvent for all solutions) is K1.86°C kg/mol and the boiling point elevation constant is Kb the following: 0.512°C kg/mol. The density of neat water at 20.0°C is 0.9982 g/ml. Answer 1. What is the molarity of the solution? 2. What is the molality...
A 1.00 kg sample of ethylene glycol (C_2 H_6 O_2) is added to 4450 g of...
A 1.00 kg sample of ethylene glycol (C_2 H_6 O_2) is added to 4450 g of water in a car radiator. What is the boiling point of the resulting solution? K_b of water is 0.512 degree C kg mol^-1, T_b for water = 100.0 degree C.
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of...
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
What is the boiling point elevation of a solution containing 17.1 g of sucrose in 100.0...
What is the boiling point elevation of a solution containing 17.1 g of sucrose in 100.0 g of water? The molal elevation constant of water is 0.512°C/m and the molar mass of sucrose is 342 g/mol.
Some ethylene glycol, HOCH2CH2OH , is added to your car’s cooling system along with 5.0 kg of water. If the freezing po...
Some ethylene glycol, HOCH2CH2OH , is added to your car’s cooling system along with 5.0 kg of water. If the freezing point of the water–glycol solution is −13.0 °C, what mass of HOCH2CH2OH must have been added? (Kfp for H2O is −1.86 °C/m.)
An aqueous ethylene glycol (HOCH2CH2OH, FW=62.07 g/mol) solution with a mass of 220.7 mg is titrated...
An aqueous ethylene glycol (HOCH2CH2OH, FW=62.07 g/mol) solution with a mass of 220.7 mg is titrated with 45.3 mL of 0.0671 M Ce4 in 4 M HClO4. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4+ is titrated with 11.73mL of 0.0449 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? mass percent =__________%
What volume of ethylene glycol (HOCH2CH2OH, density = 1.12 g mL-1) must be added to 20.0...
What volume of ethylene glycol (HOCH2CH2OH, density = 1.12 g mL-1) must be added to 20.0 L of 112 of water (Kf = 1.86 °C kg mol-1) to produce a solution that freezes at -10 °C?
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 253.1 mg is titrated with 49.5 mL of...
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 253.1 mg is titrated with 49.5 mL of 0.0895 M Ce4+ in 4 M HCIO4. The solution is held at 60°C for 15 minutes to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4+ is titrated with 10.81 mL of 0.0439 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? Number
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of ethylene glycol with a density of 1.0087 g/mL. The freezing point depression constant for water (which you can assume is the solvent for all solutions) is K1.86°C kg/mol and the boiling point elevation constant is Kb the following: 0.512°C kg/mol. The density of neat water at 20.0°C is 0.9982 g/ml. Answer 1. What is the molarity of the solution? 2. What is the molality...
A 1.00 kg sample of ethylene glycol (C_2 H_6 O_2) is added to 4450 g of water in a car radiator. What is the boiling point of the resulting solution? K_b of water is 0.512 degree C kg mol^-1, T_b for water = 100.0 degree C.
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 253.1 mg is titrated with 49.5 mL of 0.0895 M Ce4+ in 4 M HCIO4. The solution is held at 60°C for 15 minutes to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4+ is titrated with 10.81 mL of 0.0439 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? Number
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