Colligative Properties

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Questions

• How are colligative properties determined?
• How do you calculate freezing point depression?
• How can freezing point depression determine purity?
• How does the nature of the solute affect boiling point?
• How do colligative properties affect freezing point?
• What colligative property causes ice to melt?
• Why do colligative properties depend on the number of particles?
• How do ionic solutes affect the boiling point?
• Why do solutes lower vapor pressure?
• How does solubility affect boiling point?
• What are the colligative properties?
• What is the freezing point depression?
• What is the boiling point elevation?
• What is the vapor pressure of the pure solvent if the vapor pressure of a solution of 10.0 g of sucrose, #C_6H_12O_6#, in 100.0 g of ethanol is 55.0 mmHg?
• What is the molecular weight of sulfur if 35.5 grams of sulfur dissolve in 100.0 grams of CS2 to produce a solution that has a boiling point of 49.48°C?
• What is the molecular weight of acetic acid if a solution that contains 30.0 grams of acetic acid per kilogram of water freezes at -0.93°C. Do these results agree with the assumption that acetic acid has the formula CH3CO2H?
• What are common mistakes students make with Colligative Properties?
• Why does an 0.100 m solution of HCl dissolve in benzene have a freezing point depression of 0.512°C, while an 0.100 m solution of HCl in water has a freezing point depression of 0.372°C?
• Why do 0.60 grams of acetic acid dissolve in 200 grams of benzene to form a solution that lowers the freezing point of benzene to 5.40°C?
• What is the freezing point depression definition?
• What is the boiling point elevation formula?
• What determines osmotic pressure?
• How can I calculate freezing point depression of Water?
• Question #e2397
• Question #0e184
• Question #5c41e
• Question #4b054
• Question #7b124
• Question #e0398
• Question #8ad06
• In making candy, a certain recipe calls for heating an aqueous sucrose solution to the "softball" stage. Which has a boiling point of 235-240 F. Wat is the range of mass percentages of the solution of sugar (C12H22O12) that boils at those two temperature?
• How many grams of glucose (molar mass = 180.9g/mol) must be dissolved in 255g of water to raise the boiling point to 102.36Celsius?
• Why does adding 1 mole of salt, #NaCl#, lower the freezing point of a sample of water more than adding 1 mole of sucrose, #C_12H_22O_11#?
• Question #7d861
• If I pass dry air through solutions of 0.1 mol/L KCl and 6 mol/L HCl, which solution will lose mass?What will happen if I use moist air instead?
• What is the boiling point of a solution of 24.6 g of camphor in 98.5 g of benzene?
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• Question #accdb
• Question #38335
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• Question #c3228
• 20 g of fructose is being dissolved in 150g of H2O at 25°C.Calculate the boiling n freezing point of the solution.what is the osmotic pressure of the solution( density of water=100g/L)?
• Question #ec1e7
• Question #8be0e
• Question #5e092
• How is boiling point elevation applied to real life?
• Question #6b36c
• Question #006a2
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• Question #31f40
• Pure water freezes at 0°C and boils at 100°C. Would tap water likely freeze and boil at those exact temperatures? Why or why not?
• At 55.0 C, what is the vapor pressure of a solution prepared by dissolving 57.6 g of LiF in 259 g of water? The vapor pressure of water at 55.0 C is 118 mmHg. Assume complete dissociation of the solute.
• The vapor pressure of pure water at 25 degrees Celsius is 23.8 torr. What is the vapor pressure of a solution prepared by dissolving 18.0 g of glucose (molecular weight = 180.0g/mol) in 95.0 g of water?
• How would you determine the vapor pressure of a solution at 25C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water? The vapor pressure of pure water at 25C is 23.8 torr.
• How would you calculate the vapor pressure of a solution made by dissolving 88.2 g of urea (molar mass = 60.06 g/mol) in 303 mL of water at 35°C? Vapor pressure of water at 35 degrees is 42.18 mm Hg.
• A solution of sodium chloride in water has a vapor pressure of 19.6 torr at 25 degrees Celsius. What is the mole fraction of NaCl solute particles in this solution?
• Consider two solutions: one formed by adding 10 g of glucose, C6H12O6, to 1 L of water and another formed by adding 10 g of sucrose, C12H22O11, to 1 L of water. Are the vapor pressures the same?
• What is the vapor pressure in mmHg of a solution of 16.0 g of glucose (C6H12O6) in 80.0 g of methanol (CH3OH) at 27 degrees C? The vapor pressure of pure methanol at 27 degrees C is 140 mmHg.
• 150g of NaCl completely dissolve in 1.00 kg of water at 25.0 C. The vapor pressure of pure water at this temperature is 23.8 torr. How would you determine the vapor pressure of the solution?
• Question #e695c
• Question #38e70
• How should water impurities affect the melting point, and boiling point of water?
• What is the freezing point of an a nonionizing antifreeze solution containing 38.8g ethylene glycol, #C_2H_6O_2#, and 409 g of water?
• What is the boiling point of an ionic solution containing 29.7 g #Na_2SO_4# and 84.4 g water, assuming 100% ionization?
• What is the boiling point of a solution made by dissolving 31 g of NaCl in 559 g of water?
• Can someone clarify freezing point depression and boiling point elevation for me?
• If a solvent contains a few impurities, how does its boiling point compare to the pure solvent?
• What is the van't Hoff factor of #Na_3PO_4# in a 0.40 m solution whose freezing point is -2.6°C ?
• Both #NaCl# and #CaCl_2# are used to melt ice on roads and sidewalks in winter. What advantages do these substances have over sucrose or urea in lowering the freezing point of water?
• Question #75a08
• A solution is made by dissolving 25.0 g of magnesium chloride crystals in 1000 g of water. What will be the freezing point of the new solution assuming complete dissociation of the #MgCl_2# salt?
• Methanol, #CH_3OH# is used as an antifreeze. How many grams of methanol would you need per 1000.0 g of water for an aqueous solution to stay liquid at -20.0° C?
• What is the tendency of a solute to change the melting point of a solid called?
• What is the freezing point of a 0.05500 m aqueous solution of #NaNO_3#, if the molal freezing-point-depression constant of water is 1.86°C /m?
• George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to a boil. Before adding the pasta, he adds 58 g of table salt to the water and again brings it to a boil. What is the temperature of the salty boiling water?
• Glycerin, #C_3H_8O_3#, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding 164 g glycerin to 338 mL #H_2O# at 39.8°C?
• Question #c1499
• Question #53001
• Question #eb24b
• Question #d75c8
• Question #fb71b
• Question #d7617
• Question #d3727
• What will be the freezing point of a 20.0% solution of glucose, #C_6H_12O_6# in water?
• Question #e1c07
• How many grams of #NH_4OH# must be dissolved in 75 g of water to lower the freezing point -3.0°C?
• Question #83c33
• What is the boiling point of a solution containing 2.33 g of caffeine, #C_8H_10N_4O_2#, dissolved in 15.0 g of benzene? The boiling point of pure benzene is 80.1 °C and the boiling point elevation constant, Kbp, is 2.53 °C/m.
• Question #9c1c3
• What is the difference between vapour pressure of a solvent and vapour pressure of pure solvent in Raoult's law?
• A solution consists of 200. g of a nonelectrolytic solute dissolved in 500. g of water. It freezes at -9.30°C. What is the molecular weight of the solute?
• What is the molality of a solution of phosphoric acid, #H_3PO_4# that contains 24.5 g of phosphoric acid (molar mass 98.0 g) in 100 g of #H_2O#?
• If 39 grams of benzene are dissolved in 100.0 grams of water, what is is boiling point?
• Juan is making spaghetti and he adds 29 grams of #NaCl# to 250 grams of water. What is the boiling point of this solution?
• The freezing point of an aqueous solution is -2.79°C. What is the boiling point of this solution?
• Assuming 100% dissociation, what is the freezing point and boiling point of 3.39 m #K_3PO_4(aq)#?
• For equimolar solutions of #"sugar"#, #"potassium sulfate"#, and #"potassium hexaferricyanide"#, which will exert the LEAST vapour pressure?
• Salt, NaCl, has a solubility of 35.7g per 100g of water at 0 degrees C. What is the lowest possible melting point for ice that could be obtained considering the solubility of NaCl in water? The Kf for H2O is 1.86 C/m
• What is the freezing point of a solution that contains 0.5 moles of Nal in 500g of water? (Kf = 1.86C/m; molar mass of water = 18g)
• One mole of two different compounds happens to weight the same, but one compound ionizes in water and the other does not. Which will give the lowest freezing point depression?
• How do you do freezing point depression problems?
• What is the molecular mass of a substance if 22.5 g dissolved in 250 g of water produces a solution whose freezing point is -0.930°C?
• What is the freezing point of a nonionizing antifreeze solution containing 388g ethylene glycol #C_2H_6O_2# and 409 g of water?
• Question #93cfe
• Question #cb01d
• The freezing point of an aqueous sodium chloride solution is -0.20°C. What is the molality of the solution?
• What is the expected boiling-point elevation of water for a solution that contains 150 g of sodium chloride dissolved in 1.0 kg of water?
• Consider 1.60 g of naphthalene (C10H8) is dissolved in 20.0 g of benzene. The freezing point of benzene is 5.5oC, and the freezing point of the mixture is 2.8oC. What is the molal freezing point constant for benzene?
• When 3 grams of #"NaCl"# are added to 75.25 grams of water, what is the change in the water's freezing point?
• Equimolal solutions of #"KCl"# and compound #"X"# in #"H"_2"O"# show depressions of freezing pts. in a #4:1# ratio . Assuming #"KCl"# to be ionized completely , the compound #"X"# must ?
• Does salt lower boiling point?
• Question #9d5e0
• How does adding a solute to a solvent affect the boiling point of the solvent?
• How many grams of salt must be added to 300g of water to increase its boiling point by 5°C?
• A solution is prepared by dissolving 40.0 g of sucrose, in 250 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?
• What is the boiling point of a 0.743 m aqueous solution of #KCl#?
• Question #635ea
• What is the boiling point (in °C) of a 1.56 m aqueous solution of #CaCl_2#?
• Question #0c4c5
• A 2% by weight aqueous solution of NaCl (MW= 58.45) has a boiling point of 100.31 °C. What is the van't Hoff factor for NaCl?
• What effect does increasing the concentration of a dissolved solute have on each on boiling point, freezing point, and vapor pressure?
• Question #f5ef6
• The freezing point of an aqueous solution that contains a nonelectrolyte is #-4.0^@"C"#. What is the molal concentration of the solution? #Kf = 1.86^@"C/m"#
• Question #09c15
• What is the equation for freezing point?
• Question #da7b4
• Give the thermodynamic derivation of van't Hoff reaction isotherm, and explain its significance?
• What is the freezing point of an aqueous solution containing #"40.0 g"# of ethylene glycol in #"60.0 g"# of water? #K_f = 1.86^@"C/m"# and #K_b = 0.512^@ "C/m"# for water.
• Question #7be8c
• What do colligative properties depend on?
• What is the boiling point of Deep Eutectic Solvent(DES) of the mixure of Choline Chloride and Urea??????
• Does the water that comes from taps in our homes meet safety regulations?
• Find the freezing point (in #""^@ "C"#) for a solution consisting of #"60.0 g"# water and #"40.0 g"# ethylene glycol?
• Is sodium lauryl sulfate harmful to skin?
• Question #0f0c8
• We dissolve #25*g# mass of the following solutes in equivalent volumes of water. Which solutions will display the GREATEST freezing point depression?
• Question #d9acc
• How do you write position and momentum in terms of the raising and lowering operators?
• Why do we not collect water by evaporation?
• What is the molality for an aqueous solution whose freezing point dropped by #15^@ "C"# due to addition of #"CaCl"_2(s)#? #K_f = 1.86^@ "C/m"# for water.
• Question #a0ccf
• Question #59807
• Question #9cbbd
• Raoult's Law and vapor pressure?
• Question #0c0c9
• What is the mol fraction of ethylene glycol in the solution phase for an aqueous solution with a vapor pressure of #"760 torr"# if the pure vapor pressure was #"1077 torr"#?
• Question #a903a
• What are three colligative properties of solutions?
• When 8.05 g of an unknown compound X was dissolved in 100. g of benzene (C6H6), the vapor pressure of the benzene decreased from 100.0 torr to 94.8 torr at 26 degrees C. What is the mole fraction and molar mass of X?
• For an arbitrary nonelectrolyte, calculate the freezing point when #"0.0192 mols"# of it is dissolved in #"5.00 g"# of water? #K_f = 1.86^@ "C/m"# for water.
• Question #f0370
• Which of the given solutions should display the GREATEST departure from the freezing point, and the boiling point of the water solvent?
• Question #ea97e
• What is the concentration of #500*g# of #H_2C=CH_2# in #1*L# of water?
• What is the van't Hoff factor?
• Question #b576d
• Question #4f3c7
• Question #4b1a8
• Calculate the molality of a solution made by dissolving a compound in camphor if the freezing point of the solution is 162.33 degrees C: the melting point of pure camphor was measured to be 178.43 degrees C. K sub f for camphor is 37.7 degrees C/m sub c?
• What is the molar mass of the solute if #"4.18 g"# of it dissolved in #"36.30 g"# of benzene (#K_f = 5.12^@ "C"cdot"kg/mol"#) generates a solution with a freezing point of #2.70^@ "C"#? The freezing point of benzene is #5.53^@ "C"#.
• What are the molarity, molality, and mole fraction of ethylene glycol (#"C"_2"H"_6"O"_2#) in an aqueous solution that contains 40 % by mass of the solute? The density of the solution is #"1.06 g/mL"#.
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• Question #3b3c3
• Why is salt used to melt ice on the roads? What would happen to many roadside plants as a result?
• Question #03020
• How many isomers will #C_6H_12# make, when a given isomer is dissolved in a suitable solvent?
• What is the molar mass of a non-electrolyte compound if 4.28 grams is dissolved in 25.0 grams of chloroform solvent to form a solution which has a boiling point elevation of 2.30 degrees celsius?
• What is the freezing point of a 1molal and 0.432molal #Zn(H2O)_6 ^(+2)#?
• Question #8933a
• The freezing point depression of potassium ethanoate is greater than that of the other two solutes (camphor and urea) when an equal number of moles of each is used. Can somebody explain this?
• How does the boiling point of a solution evolve with INCREASED number of particles in solution? How would the boiling point increase given #0.1*mol*L^1# concentrations of #NaCl#, and #BaCl_2# in a water solvent?
• What is the boiling point of an aqueous solution of #"CaCl"_2# with a molal concentration of 1.56 mol/kg?
• Which of the following solutes is most effective in lowering the freezing point of water?
• What are the colligative Properties? How many Types are they? Explain?
• What mass of cholesterol should be dissolved in #"295 g"# of benzene to lower the freezing point by #"0.450 K"#? (#M = "386.6 g/mol"# for cholesterol and #"78.11 g/mol"# for benzene.)
• If #k_f=1.86*""^(@)C*mol^-1*kg# for water, what is the freezing point of a solution composed of #255*kg# #CaCl_2#, and #33.8*L# of water?
• If I cool a solution containing 62 g of ethylene glycol in 250 g water to -9.3 °C, what mass of ice will separate out?
• Question #9f5d4
• Question #a8fdb
• Does vapor pressure vary with the number of particles in solution? What if you have #"1 M"# of #"NaCl"#, vs. #"1 M"# #"KCl"#, vs. #"1 M"# #"CaCl"_2#?
• What effects, if any, do impurities have on the boiling point of water?
• What is the change in freezing point when #"54 g"# of glucose (use #"FW" = "180 g/mol"#) is dissolved in #"0.250 kg"# of water? #K_f = 1.86^@ "C/m"# for water.
• Question #7517e
• Question #66b16
• Why is salt sprinkled on icy roads and sidewalk?
• Question #a0387
• Question #e3ea3
• Which solution will exhibit the GREATEST freezing point depression for #1*mol*L^-1# aqueous solutions of: #"(i) propanol; (ii) potassium bromide; (iii) calcium bromide?"#
• Question #5a076
• If #"14 g"# of calcium nitrate is dissolved in #"200 g"# of water, and it experiences a #70%# dissociation, what is the solution's vapor pressure if the solvent began at the normal boiling point of water? Hint: the normal boiling point occurs at 760 torr.
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• Question #a4a55
• An organic solute was dissolved in napthalene such that the freezing point dropped by 7.9 degrees. What is the molality of the solution?
• What is the effect of the van't Hoff factor on the boiling point elevation or freezing point depression for a given electrolytic solution?
• Question #cc2fd
• What is the boiling point for a 3 molal #"CaCl"_2# aqueous solution? #K_b = 0.512^@ "C/m"#.
• What is the freezing point for an aqueous solution with #"0.195 molal"# #"K"_2"S"# dissolved in it? Assume #100%# dissociation. #K_f = 1.86^@ "C/m"#.
• What is the new boiling point for an aqueous #"0.743 molal"# solution of #"KCl"#? #K_b = 0.512^@ "C/m"#
• What is the boiling point of an aqueous solution of #LiBr# that is #0.527*mol*kg^-1# with respect to the salt?
• A solution that contains #"13.2 g"# of solute in #"250 g"# of #"CCl"_4# freezes at #-33^@ "C"#. What is the FW of the solute? #T_f^"*"# of #"CCl"_4# is #-22.8^@ "C"# and its #K_f = -29.8^@ "C/m"#.
• The boiling point of a solution containing 10.44g og an unknown nonelectrolyte in 50g of acetic acid is 159.2 degree celsius. What is the molar mass of the solute?
• Can you help me out please? Thanks!
• Can you help me please? I have a chemistry class tomorrow but I need to bring with me the answer for these two questions. So, please help. Thanks!
• Question #e16a6
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• What is the vapor pressure of a #"1.00-molal"# sugar solution at #25^@"C"#? Sugar is nonvolatile, nonelectrolyte solute. The vapor pressure of water at #25^@"C"# is #"23.8 torr"#. The molar mass of water is #"18 g/mol"#
• Urea, #("NH"_2)_2"CO"#, is dissolved in #"100 g"# of water. The solution freezes at #-0.085^@"C"#. How many grams of urea were dissolved to make this solution?
• What is the molality of benzene in a solution that contains #"6.502 g"# of benzene in #"162.7 g"# of chloroform/#"CHCl"_3# (#K_f# for #"CHCl"_3# is #4.68^@ "C"cdot"kg/mol"# and #T_f^"*"# of #"CHCl"_3# is #63.5^@ "C"#)?
• Sucrose is a nonvolatile, nonionizing solute in water. Determine the vapor pressure at #25^@"C"# of the #"1.5-m"# sucrose solution. Assume that the solution behaves ideally. The vapor pressure of pure water at #25^"C"# is #"23.8 torr"# ?