Given, molality of aqueous solution (m) = 0.0222 m
Kb = 0.512° C/m
Kf = 1.86° C/m
Boiling point of water (Tb°) = 100° C
Freezing point of water (Tf°) = 0° C
Using the laws of elevation in boiling point and depression in freezing point, we get
Tb= Kb x m
Tb - Tb° = 0.512° C/m x 0.0222 m = 0.011° C
Tb = 100° C + 0.011° C = 100.011° C
Tf = Kf x m = 1.86° C/m x 0.0222 m = 0.041° C
Tf° - Tf = 0.041° C => Tf = 0° C - 0.041° C = -0.041° C
Answer: 100.011°C, -0.041° C (option second)
Let me know if you have any queries regarding this.
An aqueous solution is 0.0222 m Determine the boiling point and freezing point of the solution....
An aqueous solution has a normal boiling point of 103 c. What is the freezing point of his solution? For Water Kb= 0.51 C/m and Kf= 1.86 C/, I want the answer with datels please!!
What is the normal boiling point of an aqueous solution that has a freezing point of 1.04 degree C. K_f for water 1.86 degree C/m.
a Calculate the freezing point and the boiling point of each of the following aqueous solutions. (Assume complete dissociation. Assume that water freezes at 0.00°C and boils at 100.000ºC.) 0.047 m MgCl2 Kr=-1.86 °C/molal Kb =0.51 °C/molal Tf= °C Tb = °C Submit b Calculate the freezing point and the boiling point of each of the following aqueous solutions. (Assume complete dissociation. Assume that water freezes at 0.00°C and boils at 100.000°C.) 0.047 m FeCl3 Kf=-1.86 °C/molal Kb =0.51 °C/molal...
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 Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in degrees Celsius from a pure solvent can be determined from the equations given here, respectively: AT) = m x K = moles of solute XK K. kilograms of solvent Since pure water boils at 100.00 °C, and since the addition of solute increases boiling point, the boiling point of an aqueous solution, Th, will be T - (100.00+AT) 'C Since pure water freezes at...
Calculate the freezing point of a 11.50 m aqueous solution of propanol. Freezing point constants can be found in the list of colligative constants. Colligative Constants Constants for freezing point depression and boiling point elevation calculations at 1 atm: Solvent Formula Kvalue" Normal freezing ky value Normal bolling (°C/m) point (°C) (°C/m) point (°C) H20 1.86 0.00 0.512 100.00 CGHS 5.12 5.49 CH12 20.8 6.59 CyH60 1.99 -117.3 calu 29.8 -22.9 76.8 water benzene cyclohexane ethanol carbon tetrachloride camphor 2.53...
Calculate the boiling point of a solution of CaCl2 in water. The freezing point depression of the same solution is -1.420 °C (kf = 1.86 °c/m, kb = 0.52°C/m).
Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in degrees Celsius from a pure solvent can be determined from the equations given here, respectively: Value Units moles of solute AT = mx Kb = 7 Submit kilograms of solvent XRb moles of solutex Kf Part B AT: = mx Kf = kilograms of solvent where m is the molality of the solution, and K and K the boiling-point-elevation and freezing-point-depression constants for the solvent,...
Assuming 100% dissociation, calculate the freezing point and boiling point of 2.11 m Na2SO4(aq). Constants may be found here. Solvent Formula Kf value* (°C/m) Normal freezing point (°C) Kb value (°C/m) Normal boiling point (°C) water H2O 1.86 0.00 0.512 100.00 benzene C6H6 5.12 5.49 2.53 80.1 cyclohexane C6H12 20.8 6.59 2.92 80.7 ethanol C2H6O 1.99 –117.3 1.22 78.4 carbon tetrachloride CCl4 29.8 –22.9 5.03 76.8 camphor C10H16O 37.8 176
2. Calculate the temperature of freezing and the boiling point of a 0.030 m FeCl solution. The k of water is 0.51°C/m and the krof water is 1.86°C/m. (4 points)