Arrange the following solutions in order of increasing freezing
point depression. [Hint: The corresponding van’t Hoff factor (i) is
given]:
(a) 0.10 m MgCl2 in water, i = 2.7, Kf = 1.86°C/m for the solvent
(water).
(b) 0.20 m toluene in diethyl ether, i = 1.00, Kf = 1.79°C/m for
the solvent (diethyl ether).
(c) 0.20 m ethylene glycol in ethanol, i = 1.00, Kf = 1.99°C/m for
the solvent (ethanol).
Arrange the following solutions in order of increasing freezing point depression. [Hint: The corresponding van’t Hoff...
The following solutions all lower the freezing point of the given solvent.. Arrange them in order of increasing freezing point depression. a. 0.1 m MgCl, in water, i = 2.7, K_f = 1.86 degree C/m b. 0.20 m toluene in diethyl ether, i = 1.00, K_f = 1.79 degree C/m c. 0.20 m glycol methanol, i = 1.00, K_f = 1.99 degree C/m
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
Choose the solvent below that would show the smallest amount of freezing point depression when used to make a 0.20 m nonelectrolyte solution carbon tetrachloride, K = 29.9°C/m chloroform, k, = 4.70"C/m ethanol, K = 1.99"Cim diethyl other, K=1.79"C/m benzene, K = 5.12 Cm
Calculate the molality for each of the following solutions. Then, calculate the freezing-point depression ATF = iKFCm produced by each of the salts. (Assume the density of water is 1.00 g/mL and KF = 1.86°C/m.) (a) 1.8 M NaCl (Assume the density of the solution is 1.00 g/mL.) Cm = 4.9 2.0 m ATF = 49 7.5 ✓ °C (b) 24 g of KCl in 1.6 L of water cm = 49, 0.20 ATF = 49) 0.75 (c) 250 ppm...
Ex. Calculate the boiling point elevation and the freezing point depression of a 250g of ethylene glycol that dissolves in 750g of water. Kb of the solvent is 0.510c/m and its Kf is 1.86oc/m linn. dolta Tbkbimi
The freezing point of water is 0.00°C at 1 atmosphere. How many grams of cobalt(II) bromide (218.7 g/mol), must be dissolved in 287.0 grams of water to reduce the freezing point by 0.350°C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C....
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 10.34 grams of calcium acetate, Ca(CH3COO)2 (158.2 g/mol), in 216.0 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is ________m. The freezing point of the solution is ___________...
The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 12.31 grams of cobalt(II) acetate, Co(CH3COO)2 (177.0 g/mol), in 287.1 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is _____m. The boiling point of the solution is °____C....
The freezing point of water is 0.00°C at 1 atmosphere. How many grams of nickel(II) sulfate (154.8 g/mol), must be dissolved in 210.0 grams of water to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g nickel(II) sulfate.