Question

In: Chemistry

Calculate the molality for each of the following solutions. Then, calculate the freezing-point depression ?TF =...

Calculate the molality for each of the following solutions. Then, calculate the freezing-point depression

?TF = KFcm

produced by each of the salts. (Assume the density of water is 1.00 g/mL and

KF = 1.86

Solutions

Expert Solution

We will use the following relation for freezing point depression,

Delta Tf = m x Kf

m = molality = moles of solute / kg of solvent

moles = g of solute / molar mass

Given are,

b. 27 g of KCl in 1.8 L of water

molar mass of KCl = 74.55 g/mol

mass of water in kg = L of water x density of water

kg of water = 1.8 x 1.0

                   = 1.8 kg

Then,

moles of KCl = 27 / 74.55

                      = 0.362 moles

molality of KCl solution Cm = 0.362 / 1.8

                                      = 0.201 m

Because the KCl salt is an ionic compound that dissociate in water to yield two ions per formula unit of KCl thus, the actual concentration of the dissolved species in the saturated solution will be

Actual concentration = 2


Related Solutions

Constants | Periodic Table Calculate the freezing point of each of the following solutions: Part A...
Constants | Periodic Table Calculate the freezing point of each of the following solutions: Part A 0.560 mole of lactose, a nonelectrolyte, added to 1.00 kg of water Express your answer to three significant figures and include the appropriate units. nothingnothing SubmitRequest Answer Part B 44.0 g of KCl, a strong electrolyte, dissolved in 1.00 kg of water Express your answer to three significant figures and include the appropriate units. nothingnothing SubmitRequest Answer Part C 1.3 moles of K3PO4, a...
Calculate boiling point depression and freezing point depression. Make sure to include correctly written dissociation equation....
Calculate boiling point depression and freezing point depression. Make sure to include correctly written dissociation equation. A. 0.25 m ethylene glycol -C2H6O2 B. 0.25 m NaCl
9. Calculate the freezing point and boiling point of the following aqueous solutions, assuming complete dissociation:...
9. Calculate the freezing point and boiling point of the following aqueous solutions, assuming complete dissociation: (a) 10.5 g FeCl3 in 1.50
What is the molality of a solution of naphthalene in benzene if the freezing point of...
What is the molality of a solution of naphthalene in benzene if the freezing point of pure benzene is 5.5°C and the freezing point of the solution is 4.0°C. The freezing point depression constant for benzene is 5.12°C m-1.
calculate the molar mass? calculate the value of the freezing point depression constant, Kf, for acetic...
calculate the molar mass? calculate the value of the freezing point depression constant, Kf, for acetic acid. Trail 1 Trail 2 Mass of acetic acid 1.735g 2.195g Mass of acetylsalicylic acid 0.06g 0.09g Freezing point 14.247C 14.247 Change in temperature 0.852C 0.852C
Calculate the molality of each of the following solutions. 1) 583g of H2SO4 in 1.50 kg...
Calculate the molality of each of the following solutions. 1) 583g of H2SO4 in 1.50 kg of water. 2) 0.86g of NaCl in 1.00x10^2g of water. 3) 46.85g of codeine, C18H21NO3, in 125.5g of ethanol, C2H5OH. 4) 25g of I2 in 125g of ethanol, C2H5OH.
Calculate the molality of each of the following aqueous solutions: (a) 2.01 M NaCl (density of...
Calculate the molality of each of the following aqueous solutions: (a) 2.01 M NaCl (density of solution = 1.08 g/mL) m (b) 51.8 percent by mass KBr solution
Molar Mass Determination by Depression of the Freezing Point A student determines the freezing point of...
Molar Mass Determination by Depression of the Freezing Point A student determines the freezing point of a solution of 0.630 g of mandelic acid in 20.78 g of tbutanol. He obtains the following temperature-time readings: Time (min) Temp (C) Time (min) Temp (C) Time (min) Temp (C) 0.0 34.9 3.0 22.3 6.0 21.8 0.5 33.3 3.5 21.4 6.5 21.7 1.0 29.7 4.0 22.3 7.0 21.6 1.5 27.1 4.5 22.2 7.5 21.5 2.0 25.2 5.0 22.1 8.0 21.3 2.5 23.6 5.5...
The formula that governs the depression of freezing point and elevation of boiling point for a...
The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: ΔT = i × kb × m where: ΔT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions; i = 2...
What is the concentration of each of the following solutions? (a) The molality of a solution...
What is the concentration of each of the following solutions? (a) The molality of a solution prepared by dissolving 25.0 g of H2SO4 in 1.30 L of water (b) The mole fraction of each component of a solution prepared by dissolving 2.25 g of nicotine, C10H14N2, in 80.0 g of CH2Cl2
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT