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 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 =__________%
A 8.5 mass % aqueous solution of ethylene glycol (HOCH2CH2OH) has a density of 1.34 g/mL. Calculate the molarity of the solution. ANSWER: 1.84 +- 2%
An solution of antifreeze is prepared by mixing 21.0mL of ethylene glycol (d = 1.11 g/mL; molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its molarity?
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
You have a 4M aqueous solution of ethylene glycol (62 g / mol molar mass). You want to recover 49 ml of pure ethylene glycol from this solution. What is the minimum amount of aqueous solution required to obtain the desired ethylene glycol. density of ethylene glycol is 1.11 g / ml
A solution of antifreese is prepared by mixting 34.0mL of ethylene glycol (d=1.11g/mL; molar mass =62.07 g/mol) with 50.0 mL H20 (d=1.00 g/mol) at 25 degrees celsius. if the density of the antifreeze solution is 1.07 g/ mL, what is the molarity?
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL;M=62.07 g/mol) and water (d=1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent 50v/v (b) mass percent 52.05w/w (c) molarity 0.0089 (d) molality 0.0083 (e) mole fraction
A solution of antifreeze is prepared by mixing 21.0mL of ethylene glycol (d = 1.11 g/mL; molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its molarity (M)?
1. 1200 mL aqueous solution of 45 g of ethylene glycol and 80 g of sucrose were prepared with a density of 1.37 g/mL. Assume that the solution behaves ideally. Notes: The vapor pressures of water and ethylene glycol at 20 °C are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water are 0.51 K/m and 1.86 K/m, at 25 °C respectively. a. What is the freezing point of this solution? b. What is the vapor pressure,...
Antifreeze is an 50% by mass aqueous solution of the non-electrolyte ethylene glycol (C2H6O2). What is the freezing point of this solution? The Kf for water is 1.86oC∙kg∙mol−1 and assume a density of 1.00g/mL.