A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is _______ degrees celsius. The freezing point of pure ethanol is -114.6 degrees celsius at 1atm. The molal-freezing point depression constant (Kf) for ethanol is 1.99 degrees celsius/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.
A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3) in 201 g of ethanol...
2. A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is __________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant (Kf) for ethanol is 1.88 °C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.
A solution is prepared by dissolving 5.00 g of glycerin () in 201 g of ethanol The freezing point of the solution is ________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant () for ethanol is 1.99 °C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively. -115.1 -119.4 0.537 -109.8 -114.1
9. 65) A soltion is prepared by dissolving 7.00 g of gycerin (C3Hg03) in 201 g of ethanol (C2HsOH). The freezing point of the solution isoC freezing-point-depression constant (Kp for ethanol is 1.99°C/m. The molar °C. The feezing point of pure ethanol is -114.6°C at 1 atm. The molal- masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol respectively.
Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m. A) -3.33°C B) 0.887°C C) -1.65°C D) 3.33°C E) 0.654°C
Benzaldehyde ( MM = 106.18 g/mol) also known as oil of almonds is used in the manufracture of dyes and perfume and in flavorings. what would be the freezing point of a solution prepared by dissolving 106.345 g of benzaldehyde in 1.687 kg of ethanol? kf=1.99, freezing point of pure ethanol = -117.3 degree Celsius a) moles of benzaldehyde b) kg of ethanol c) molality d) freezing point depression : delta Tf= kf×m e) freezing point of the solution
What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Masses: Ca = 40, N = 14, O = 16. Also, the molal freezing point depression constant for water is 1.86 °C/m.]
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point of the solution. The molar mass of palmitic acid is 256.48 g/ mol. The molal freezing point constant , Kf for stearic acid is 4.5 degrees C/ m and pure stearic acid freezes at 69.3 degrees Celsius.
Given the following information. Determine the freezing points of a solution which contains 76.5 g of a sodium carbonate (Na2CO3) in 500.0 g of ethanol (C2H6O). Kf for ethanol 1.99 °C / m Normal freezing point for ethanol -114.6 °C
A solution was made by adding 800 g of ethanol, C2H5OH, to 8 x 103 g of water. How much would this lower the freezing point? Kf of H2O is 1.86 degrees Celsius/m The answer is supposed to be 4.1 degrees Celsius, but I got 3.98287 degrees Celsius. What did I do wrong?
Question 1 5 pts A solution is prepared by dissolving 35.35 g ethanol (C2H5OH; Molar mass = 46.08 g/mol) in 42.2 g water. What is the molality (mol/kg) of C2H5OH in the solution? 4361 m 4.36 m 0.767 m 18.2 m 0.0182 m Question 2 5 pts Which observation correctly reflects colligative property? A KOH solution has a high vapor pressure than pure water Adding NaCl to ice will increase its melting point. A 0.5 m NaOH solution boils at...