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.
dTf = Kf*m
molality = moles / kg of solvent
moles of glycerine = 7.00 / 92.1 = 0.0760 mol
molality = 0.0760 / 0.201 = 0.378 mol/kg
?Tf = 1.99*0.378 = 0.75
2. A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of...
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 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
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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
A solution is prepared by dissolving 0.107 g of an unknown non-electrolyte in 88.1 g of camphor. The freezing point of the solution was measured to be 178.0�C. What is the molecular weight of the compound? (The freezing point of pure camphor is 179.5�C and kf= 40�C/m)?
A solution is prepared by dissolving 3.04 g of an unknown nonelectrolyte in 16.00 g of cylcohexane (tf = 6.6 oC and kf = 20.0 oC/m). What is the molar mass of the unknown compound if the solution has a freezing point of -6.7 oC? Please see https://youtu.be/lwWZ5hdB61M for assistance. Mm = g/mol
1. A solution was prepared by dissolving 2.20g of urea (H2NCONH2) in 50.00g of water. If for H2O Tb = 100C, Tf = 0C, Kb = 0.52C / m and Kf = 1.86C / m, determine the freezing and boiling point of the solution. 2. A solution is prepared by dissolving 17.41g of a substance X in 600g of benzene and the resulting solution is frozen at 4.00C. If the freezing point of pure benzene is 5.55C and its Kf...
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...