deltaTf = Kf*m
Kf = 1.86K/molkg-1
m = molality = moles of solute/mass of solvent in kg = 2.32mol/2.00kg= 1.16mol/kg
deltatf = 1.86K/molkg * 1.16mol/kg = 2.16C
Tf = -2.16C (decrease in freezing point)
186 kmolka"), what is the The amount of 2.32 mol of a sugar is added to...
Saccharin is an artificial sweetner used in the absence of sugar. When saccarin is added to pure water, the freezing point of the resulting solution drops to -5 C. Calculate the freezing point depression the aqueous saccharin solution.
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water to produce an antifreeze solution with a freezing point of-19.0°C? (The density of ethylene glycol is 1.11 g/cm°, and the density of water is 1.00 g/cm³. K, for water is 0.51°C•kg/mol and Kf is 1.86°C kg/mol.) Volume %3D What is the boiling point of this solution? Boiling point °C %3D 5 item attempts remaining Submit Answer Try Another Version [References] Consider an aqueous solution...
A sugar solution is prepared by adding 3.50 g of sugar to 22.5 mL of a pure liquid and the freezing point of the sugar solution was determined to be -99.84 C. If the normal freezing point of the pure liquid is -97 C and the density is .792g/mL, what is the freezing point depression constant in degrees celsius?
8. What is the final boiling point of a 1.25 molal solution of sugar in water? The Kb for water is 0.512 C/m. (For sugar i = l.) 9. A solution was prepared by dissolving 0.52 mol hexane into 400g CCl4. What is the change in freezing point of this solution? Carbon tetrachloride has a freezing point depression constant of 29.8 Cm,and freezes at-23。. 10. A solution was prepared by dissolving 0.26 moles of ethanol (C2HsOH) into 750g Diethyl ether....
You obtained the following
graphical data from two experimental runs to determine the freezing
point depression constant for a pure solvent. The solution was made
up by adding 3.025 g of naphthalene, C10H8,
to 45.320 g of pure solvent.
1.What is the freezing point temperature of the pure solvent (in
oC)?
2.What is the solution freezing point temperature (in
oC)?
3.What is the freezing point depression, Tfp (in
oC)?
4.What is the molar mass of naphthalene (in g/mol)?
5.How many...
What amount of sucrose (C12H22O11) should be added to 5.83 mol water to lower the vapor pressure of water at 50 °C to 72.0 torr? The vapor pressure of pure water at 50 °C is 92.6 torr.
50 grams each of water (18.015 g/mol) and ethylene glycol (C2H6O2) (62.07 g/mol) are mixed. At what temperature will the mixture freeze? The freezing point depression constant for water is 1.86 ºC/m can i get it step my step please
What is the freezing point of water made by dissolving 46.62 g of sugar (C12H22O11) in 91.32 g of water? The freezing-point depression constant of water is 1.86 oC/m.
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
Hi, I need some help with Chemistry.
Q1:
Q2:
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You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...