Number of results: 59,871
Chemistry
1) Benzene freezes at 5.45 degrees celsius. The Kf for benzene is -5.07C/m. What would be the freezing point of a 0.210m solution of octane in benzene? I am not sure how to start this. I know the equation for freezing point is Kfp * m solute.
Sunday, February 12, 2012 at 5:38pm by Hannah
chemistry
An ethylene glycol solution is mad using 58.5g of (C2H6O2) and diluting to a total volume of 500.0 mL. Calculate the freezing and boiling point. Assume a density of 1.09 g/ml for the solution
Saturday, November 5, 2011 at 9:49am by Monique
Chemistry
A solution was made by dissolving 62.07 grams of a compound in 500g of water. The compound was not ionic. The freezing point of the solution was measured and found to be -1.86 degrees celsius. Using the Kf value in your textbook, the molar mass of this conpound can be ...
Sunday, February 12, 2012 at 8:17pm by Hannah
chemistry
A solution is made by dissolving 15.5 grams of glucose (C6H12O6) in 245 grams of water. What is the freezing-point depression of the solvent if the freezing point constant is -1.86 °C/m? Show all of the work needed to solve this problem.
Saturday, April 6, 2013 at 9:06am by MadiB PLEASE HELP :(
chemistry
A solution is made by dissolving 15.5 grams of glucose (C6H12O6) in 245 grams of water. What is the freezing-point depression of the solvent if the freezing point constant is -1.86 °C/m? Show all of the work needed to solve this problem.
Saturday, April 6, 2013 at 8:46am by MadiB PLEASE HELP :(
chemistry
A solution is made by dissolving 10.20 grams of glucose (C6H12O6) in 355 grams of water. What is the freezing-point depression of the solvent if the freezing point constant is -1.86 °C/m? Show all of the work needed to solve this problem.
Friday, March 29, 2013 at 7:27pm by kat
Chem II
A little reasoning is what you need. The freezing point is delta T = i*kf*m You know Kf is the same for all of them. You know, from the problem, that m is the same (0.075m) for all of them, so what's the difference? The only difference is i. A small i gives a smaller delta...
Thursday, August 2, 2012 at 8:34am by DrBob222
Chemistry
What is the freezing point of an aqueous 2.25 m potassium nitrate (KNO3) solution? The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC/m.
Thursday, August 26, 2010 at 10:15pm by Cecilia
Chemistry
What is the freezing point of an aqueous 2.25 m potassium nitrate (KNO3) solution? The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC/m.
Thursday, August 26, 2010 at 10:49am by Cecillia
Chemistry
What is the freezing point of an aqueous 2.65 m calcium chloride (CaCl2) solution? The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC/m.
Saturday, August 21, 2010 at 10:44pm by David
Chemistry
Calculate the freezing point depression of an aqueous solution prepared by mixing 22.0 g C6H12O6, with 600 ml of water
Monday, February 20, 2012 at 11:13pm by Kristen
Chemistry
Calculate the freezing point of each of the solution 75.0 of glucose,C6H12O6 , added to 9.30×10−2 of water.... Please help
Monday, December 6, 2010 at 2:04am by Garrett
Chemistry
You need to find the freezing point of a 1.50m aqueous NaCl solution. You calculate []Tf to be 1.86 degrees C/m x 3.00m or 5.86 degrees C. What is the temperature at which the solution freezes?
Tuesday, April 27, 2010 at 8:18pm by Kim
Chemistry
A solution made from .650g of an unknown compound in 27.8 g of diphenyl gave a freezing-point depression of 1.56 degrees C. Calculate the molality of the solution. (Kf for diphenyl is 8 degrees C/m)
Monday, October 18, 2010 at 5:47pm by Kolby
chemistry
Automotive antifreeze consists of ethylene glycol, C2H6O2, a nonvolatile electrolyte. Calculate the boiling point and freezing point of a 25.0 mass percent of ethylene glycol in solution.
Sunday, January 31, 2010 at 11:26pm by danielle
science
What is the freezing point of a solution of 12.0 g of CCl4 dissolved in 750.0 g of benzene? The freezing point of benzene is 5.48°C; Kf is 5.12°C/m.
Wednesday, May 6, 2009 at 4:19pm by Stephanie
chemistry
4) An aqueous solution is 1.65 m glucose. What are the boiling point and freezing point of this solution?
Monday, October 15, 2012 at 7:38pm by Mike
Chemistry
An aqueous solution is 0.257 m NaOH. What are the boiling point and freezing point of this solution?
Thursday, March 29, 2012 at 5:51pm by MJ
Chemistry
Calculate the freezing point depression and osmotic pressure at 25 degrees C of an aqueous solution of 1.0 g/L of a protein (mol wt= 90,000) if the density of the solution is 1.0 g/mL. I know how to calculate freezing point depression and osmotic pressure, but I'm having ...
Saturday, March 24, 2007 at 4:37pm by Jessica
chem
calculate the freezing and boiling points of each of the following solutions. (a) 0.50 m glucose in ethanol for the freezing point i got 58 but it said i have the wrong sign...?
Thursday, March 24, 2011 at 9:22pm by hannah
chem(freezing point)
please help! I am lost! Question: Find the expected freezing point of a water solution that contains 286g of aluminum nitrate (Al(NO3)3) in 8.5 kg of water. answer in celcius Note the correct spelling of Celsius. delta T = i*Kf*m Determine the molality of 286 g Al(NO3)3 in 8.5...
Tuesday, May 29, 2007 at 9:53pm by Anonymous
Chemistry
What is the freezing point of a solution made by dissolving 450 g of ethylene glycol (C2H6O2) in 550 g of water? The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC/m.
Saturday, August 21, 2010 at 10:00pm by Cecilia
Chemistry
The normal freezing point is zero C. Therefore, the new freezing point will be -5.86 degrees C. However, when I multiply 3 x 1.86 I obtain 5.58 and the freezing point would be -5.58.
Tuesday, April 27, 2010 at 8:18pm by DrBob222
chem132
When 15.0 g of ethyl alcohol, C2H5OH, is dissolved in 750 g of formic acid, the freezing point of the solution is 7.20 C. The freezing point of the pure formic acid is 8.40 C. Evaluate Kf for fomic acid.
Friday, July 16, 2010 at 12:42am by bree
Chemistry
1. Which of the following is not true? a. The freezing point of sea water is lower than the freezing point of pure water. b. The boiling point of a water sample from the Salt Lake is lower than the boiling point of pure water. c. The freezing point of 0.1 M NaCl is lower than...
Monday, March 17, 2008 at 12:48pm by Cameo
chemistry
A solution that contains 0.500 g phenol in 12.0 g cyclohexane freezes at ¨C2.44¡ãC and boils at 81.94¡ãC. Calculate the freezing©\point depression and boiling©\point elevation constants for cyclohexane.
Wednesday, February 16, 2011 at 12:16am by Anonymous
Chemistry
The freezing point of ethanol is -114.6 deg Celsius and its Kf value is 2.00degC/m. What is the freezing point for a solution prepared by dissolving 50.0g of glycerin in 200g ethanol? I thought it may have been using the formula deltaT=Kf*m, but I'm not sure.
Wednesday, February 13, 2013 at 11:51am by Jonah
Chemistry
Two moles of a nonelectrolyte solute are dissolved in 1 kg of an unknown solvent. The solution freezes at 7.8 degrees Celsius below its normal freezing point. What is the molal freezing point constant of the unknown solvent? What is your prediction for the identity of the ...
Monday, May 17, 2010 at 11:14pm by Alyssa
Chemistry
A 1.00% by mass MgSO4(aq) solution has a freezing point of -0.192°C. (a) Estimate the van't Hoff i factor from the data. (b) Determine the total molality of all solute species. (c) Calculate the percentage dissociation of MgSO4 in this solution. Can anyone help me with...
Friday, December 10, 2010 at 4:21am by Daiyo
chemistry
which solution has highest freezing point if all are at the same molality calcium chloride sodium nitrate potassium sulfate iron(III) nitrate all have same freezing point please explain
Friday, March 16, 2012 at 2:51pm by kim
chemistry
When 18 g of ethylene glycol C2H6O2 is dissolved in 150 g of pure water, the freezing point of the solution is ___ (degrees)C. ( The freezing point depression constant for water is 1.86(dgrees)C kg/mol. I know the formulas I just need to see it done step by step please.
Monday, August 4, 2008 at 10:23pm by Jared
Chemistry
The freezing point depression of a 0.100 molality solution of NaCl(aq) solution is 0.34 deg C. Calculate the % dissociation of NaCl(aq) (Kf for water = 1.86 deg Cm^-1)
Sunday, August 30, 2009 at 5:10pm by AJ
chemistry
A 115 mL sample of a 10.0 M ethylene glycol (C2H6O2) solution is diluted to 1.30 L. What is the freezing point of the final solution? (Assume a density of 1.06 g/mL for the final solution.) What is the boiling point of the final solution? How would I go about setting this up? ...
Sunday, April 29, 2012 at 1:09am by Jen
chemistry
Calculate the freezing point of a solution contaning 5.0 grams of KCl and 550.0 grams of water. answer is -0.45 C but i don't know how to get here
Thursday, October 4, 2012 at 8:55am by Paloa
chemistry
A glucose solution contains 55.8g of glucose (C6H12O6) in 455g of water. Calculate the freezing poing and boiling point of the solution. (Assume a density of 1.00 g/ml for water. This what I did, I got moles of C6H12O6, 0.89 moles C6H12O6 then I got the mass of the solution ...
Friday, November 4, 2011 at 2:41pm by Monique
chemistry
what is the freezing point of a solution of 12.0 g of CCl4 dissolved in 750.0g of benzene? the freezing point of benzene is 5.48 degrees C ; Kf is 5.12 degrees c/m.
Wednesday, April 28, 2010 at 10:08pm by Kim
ap chem
Find the molecular mass of a solute by freezing point depression. Solvent: para-dichlorobenzene Freezing point of pure solvent: 53.02C Mass of unknown substance: 2.04g Freezingpointdepressin constant:7.1c/m Mass of para-dichlo...: 24.80g Freexing point solution: 50.78 C Can ...
Tuesday, April 13, 2010 at 11:44pm by anonymous
Chemistry hw
Assuming 100% dissociation, calculate the freezing point and boiling point of 3.13 m SnCl4(aq). Tf=? Tb=? My work: SnCl4 with 100% dissociation gives a van't hoff factor of 5, 1Sn 4+ ion and 4 Cl- ions deltaT = i x Kf x m for freezing point = 5 x 0.51C/m x 3.13m = deltaTf ...
Sunday, February 19, 2012 at 1:41am by Akle
Chemistry 130
No, it could not be used. You have to have molecules of solute dispersed uniformly over the surface of the solution to achieve freezing point depression. If the material does not dissolve, you would have a colloidal mixture. Patches of ice would form at the normal freezing point.
Wednesday, October 7, 2009 at 12:07pm by drwls
Chemistry
a) Solution A has a higher osmotic pressure than Solution B pi = MRT. Effective molarity A is 0.2, effective molarity B is 0.3 so A will give a smaller osmotic pressure than B. b) Solution A has a lower vapor pressure than Solution B Psolution = Xsolvent*Pnormal solvent. Since...
Sunday, March 7, 2010 at 10:23pm by DrBob222
Chemistry
A solution is prepared by placing 72.8 g of calcium chloride in 120 g of water at 22C. The vapor pressure of water at 22C is 2.6 kPa. a)What is the boiling point of the solution? b)What is the freezing point of the solution?
Wednesday, September 16, 2009 at 2:52am by haley
Chemistry
Cyclohexane has a freezing point of 6.6 degree Celsius and a K(f) of 20.0 degree Celsius/m. 1.50g of an unknown solute is dissolved wth 18.0g of cyclohexane. The freezing point of the solution was 1.3 degree Celsius Using this iInformation assuming the solute doesn't ...
Monday, May 27, 2013 at 9:08pm by Michael
chemistry
Data: freezing point of pure cyclohexane: 6.0 degrees celcius Freezing point of unknown soluton: 1.6 degrees celcius weight of cyclohexane: 40.0231g=0.0400231 kg weight of unknown solute: 0.4872 g K_f_ of cyclohexane: -20.00 degrees Celciusx kg/mole questions: 1. what is the ...
Monday, May 2, 2011 at 12:56am by Tina
CHEM- solution/freezing piont
a solution of sulfur (2.560g) in naphthalene (100g) freezes 0.68K lower the freezing point of pure naphthalene (353.10K). for naphthalene, Kf= 6.8K kg mol. calculatem the molecular formula of the sulfur dissolved in the naphthalene?
Thursday, October 14, 2010 at 1:05am by lulu
Chemistry
Which of the following solutes, dissolved in 1000g of water, would provide a solution would the lowest freezing point? .030 mol of BaCl2, CO(NH2)2, CaSO4, CH3COOH, or .030 mol of NH4NO3 Again, the steps needed to determine for the freezing point.
Tuesday, February 19, 2013 at 5:50am by Marcus
Chemistry
I am confused about why this is the answer to a practice problem I was given. (answer is c). Could someone explain why/why not for each answer? 2) Solution A is made from 1 L of water and 0.1 moles of Na(CH3COO), and Solution B is made from 1 L of water and 0.1 moles of Na2(...
Sunday, March 7, 2010 at 10:23pm by Trixie
Chemistry:Freezing Points
The freezing point lowering of a saturated aqueous solution of NaCl is 17 Celsius. Would spreading salt on the icy sidewalks be beneficial when the temperature outside is -8 Fahrenheit? Explain.
Sunday, November 11, 2012 at 9:19pm by Anonymous
chem
How would i found out the freezing point of a solution which has 0.05mol of acetic acid dissolved into 125g of benzene? Benzene melts at 5.5C and has a constant of 5.1C/m. The acid forms a dimer (what is this and how does it affect the calculations?) A dimer is a molecule from...
Tuesday, August 7, 2007 at 5:10am by Chris
Chemistry
What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 in 115 g of water? The molal freezing point depression constant for water is 1.86°C/m. (Note that when Ca(NO3)2 dissolves in water Ca2+ and NO32- ions are produced).
Friday, May 25, 2012 at 12:10am by Henry
Chem
a chemist is asked to identify 2 solutions whose labels have peeled off. One is known to contain 1.0 mol of NaCl, the other is 1 mol of Na2CO3. Both solutes are dissolved in 1 kg of water. If the chemist measures the freezing point of each solution, can it identify which is ...
Monday, April 30, 2007 at 8:03pm by Kim
chemistry
1. If a gaseous sample contains 73% N2 by volume, what is the solubility of N2 in water at 25°C and 1.0 atm (kH in H2O at 25°C = 7.0 10-4 mol/Latm)? 2. Calculate the vapor pressure of a solution of 0.60 mol of cholesterol in 4.5 mol of toluene at 32°C. Pure toluene...
Monday, January 31, 2011 at 3:49pm by Ashley
chemistry
delta T = Kb*m m = 18/62 = 0.29 mols molality = 0.29/0.15 = 1.93 m delta T = 1.86 x 1.93 = 3.6 degrees. The normal freezing point is zero, so the new freezing point must be 0.0 - 3.6 = -3.6. I suspect that's your problem. You are stopping at delta T which IS 3.6 but the ...
Monday, April 7, 2008 at 12:24pm by DrBob222
Chemisty-Freezing Points
The freezing point of benzene is 5.5°C. What is the freezing point of a solution of 8.50 g of naphthalene (C10H8) in 425 g of benzene (Kf of benzene = 4.90°C/m)? delta T = Kf m m = mols/kg solvent. Change 8.5 g naphthalene to mols and 425 g benzene to kg. That will get...
Sunday, January 21, 2007 at 9:51pm by Swim4eva
molal
the freezing point of ethanol (C2H5OH) is -114.6C. the molal freezing point depression constant for ethanol is 2.00C/m. what is the freezing point (C) of a solution prepared by dissolving 50.0 g of glycerin (C3H8O3, A nonelectrolyte) in 200 g of ethanol. i tried to solve it on...
Thursday, September 16, 2010 at 4:33am by lisa
Chemistry
Pure benzene has a normal freezing point of 5.50 degrees Celsius. A solution containing 11.4 grams of a molecular substance dissolved in 150.0 grams of benzene (Kf=5.12C/m) has a freezing point of 1.20 degrees Celsius. What is the molar mass of the solute?
Monday, March 22, 2010 at 7:31pm by Katelynn
chemistry
Compute the freezing point of this Solution: 25.5g C7H11NO7S (4-nitro-2-toluenesulfonoic acid dihydrate) in 1.00*10^2g H2O (nonionizing solute) The freezing point of H2O is lowered 1.86 Celsius per mole of solute. The boiling point of H2O is raised 0.512 Celsius per mole of ...
Monday, November 22, 2010 at 2:03pm by Jose Reyes
chemistry
1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute is present in 1200g of water, what are the ...
Thursday, February 2, 2012 at 3:25am by Larry
Chemistry
I need this answered really fast. 4. Ethylene glycol (C2H6O2) is used as an antifreeze in cars. If 400 g of ethylene glycol is added to 4.00 kg of water, what is the molality? Calculate how much the freezing point of water will be lowered. The freezing-point depression ...
Friday, May 17, 2013 at 4:45pm by Lauren
molal (again)
i tried to solve it on my own but im confused about the last part, this i what i have so far.. moles of glycerin= 50.0/92.10=0.54 molality=0.54/0.200=2.7 is that right? im a little confused about the numbers im supposed to use for step 3... this was the question: the freezing ...
Wednesday, September 15, 2010 at 7:55pm by lisa
Chemistry
divide by the freezing point depression constant of water. freezing point=molality*freezing point depression constant
Monday, May 3, 2010 at 12:47pm by bobpursley
chem- molar weight
I worked this problem, I would like to know if I did it correctly, I think I missed something, I'm not sure..... When a 20.0 gram sample of an unknown compound is dissolved in 500 grams of benzene, the freezing pointof the resulting solution was observed to be 3.77 degrees...
Friday, September 7, 2007 at 7:48pm by manny
Chemistry
Thyroxine, an important hormone that controls the rate of metabolism in the body can be isolated from the thyroid gland. If 0.455 g of thyroxine is dissolved in 10.0 g of benzene, the freezing point of the solution could be measured as 5.144°C. Pure benzene freezes at 5....
Monday, January 21, 2013 at 7:27pm by Emma
Chemistry
A 1.065-g sample of an unknown substance is dissolved in 30.00 g of benzene; the freezing point of the solution is 4.25 degrees C. The compound is 50.69% C, 4.23% H, and 45.08% O by mass. Info you might need on benzene: Normal Freezing point,degrees C: 5.53 Kf, degrees m^1: 5....
Monday, February 25, 2013 at 2:19am by JJ
science
Using data from this table of molal boiling-point-elevation and freezing-point-depression constants, calculate the freezing and boiling points of each of the following solutions. a)0.39 m glucose in ethanol (b) 22.8 g of decane, C10H22, in 53.9 g CHCl3 (c) 3.90 g NaOH in 109 g...
Wednesday, January 23, 2013 at 4:02pm by Hannah
chem
A solution prepared by dissolving 3.00 grams of ascorbic acid (vitamin C, C6H8O6), in 50.0 grams of acetic acid has a freezing point that is depressed by T = 1.33 oC below that of pure acetic acid. What is the value of the molar freezing point-depression constant for ...
Monday, February 18, 2013 at 10:57pm by Ace
chemistry
what are the boiling point and freezing point of a 3.17 m solution of naphthalene in benzene
Friday, December 7, 2012 at 9:37pm by Anonymous
Chemistry
The boiling point of an aq solution 102.11 C. What is the freezing point?
Tuesday, July 12, 2011 at 5:38pm by Josh
Chemistry
The boiling point of an aq solution 102.11 C. What is the freezing point?
Tuesday, July 12, 2011 at 4:06pm by Josh
Chem
a) An ethylene glycol solution contains 21.1 g of ethylene glycol in 86.0 ml of water. compute the freezing point of the solution. b) Compute the boiling point of the solution.
Sunday, March 13, 2011 at 5:53pm by Emilene
Chemistry
It would have helped to give the data below. Here is how you do the problem. I assume there is a density. Use the density to calculate the mass. mass -= volume x density. Then for heat used there are two formula to use. Within a phase you use mass x specific heat x (Tfinal-...
Thursday, March 8, 2012 at 6:40pm by DrBob222
Chemistry
Calculate the molecular mass of the nonionic solutes. 8.02 grams of solute in 861 grams of water lower the freezing point to -0.430 celsius. the freezing point of H2O is lowered 1.86 celsius per mole of solute. the boiling point of H2O is raised 0.512 celsius per mole of solute.
Monday, November 22, 2010 at 2:13pm by Jose Reyes
science
What is the boiling point of a solution of 0.150g of glycerol in 20g of water? What is the freezing point?
Monday, January 28, 2013 at 3:05pm by Absa
Chemistry
What is the freezing point of a solution of 1.17g of 1-naphthol, C10H8O, dissolved in 2.00ml of benzene at 20 degrees C? The density of benzene at 20 degrees C is 876g/ml. Kf for benzene is 5.12 degrees C/m, and benzene's normal freezing point is 5.53 degrees C.
Monday, April 4, 2011 at 3:36pm by Jake
chemistry
How do I calculate the freezing point of 11.3g FeCl3 in 155g water? I know how to calculate i and m but how do you find Kf?
Tuesday, December 4, 2012 at 9:19pm by Farah Massardi
Chemistry
Does anyone know how to do this problem, i can't seem to solve it. If 39.25 g of a substance is dissolved in 155.5 g of benzene solvent, the freezing point of the solution is 0.08 oC. Calculate the apparent molar mass (g/mol) of substance.
Tuesday, February 2, 2010 at 12:52am by SuSu
Chemistry
40.0 g of magnesium chloride (MgCl2) in 250.0 g of water at 22 °C.Calculate a) the vapor pressure of this solution, b) the freezing point, c) the boiling point. I know it is something like this, but I continue to get the incorrect answer. A) 40.og Mgcl2*(1mol mgcl2/ 95.2 ...
Thursday, May 23, 2013 at 1:03pm by Jasmine
Chemistry (science)
I dont know how to answer this. An aqueous solution of glucose has a freezing point of -0.37. What is the concentration of the solution?
Sunday, August 26, 2012 at 8:36am by Camela
Chemistry
what would the freezing point be for a solution of 0.87M aqueous ammonia? The density of this solution is 0.992g/cm3
Monday, May 3, 2010 at 9:45am by Chem
Chemistry
What would the freezing point be for a solution of 0.87 M aqueous ammonia? the density of this solution is 0.922 g/cm3.
Saturday, May 1, 2010 at 4:42pm by Anonymous
chemistry
If Pdcb replaces naphthalene as an active ingredient in mothballs , what is the value of kf for camphor if a 0.260 m solution of PDCB in camphor decreases the freezing point of camphor by 9.8 degrees C. I am sure that you will use the formula ^T=-kfm. Since you are given the 0...
Monday, January 26, 2009 at 9:17pm by betsy
Chemistry
delta T = i*Kf*m i = 1 for glucose i = 3 for CoCl2 i = 4 for FeCl3 i = 2 for NaI (i = van't Hoff factor which is the number of particles in soln). But you really don't need any of that stuff above to answer the question. Note that pure water freezes at 0 C. ALL solutes...
Monday, November 7, 2011 at 3:20pm by DrBob222
Chemistry
ok so my freezing point for NaCl was -2.0 so I can do -2.0-(0.5)= -2.5 degrees celsius. My freezing point for DI water was positive 0.5. So delta T would be -2.5?
Monday, February 20, 2012 at 4:23pm by Hannah
chem - freezing point
b. What is the freezing point depression when 153 g of bromine is added to 100 g of benzene?
Monday, October 4, 2010 at 2:19pm by martin
Chemistry
The boiling point of an aqueous solution is 102.35 °C. What is the freezing point? Constants can be found here.
Tuesday, February 21, 2012 at 1:59am by Heather
Chem TWO
Assuming 100% dissociation, calculate the freezing point and boiling point of 2.91 m K3PO4(aq).
Saturday, July 14, 2012 at 6:40pm by Jenny
Chemistry
A glucose solution contains 55.0g of glucose C6H12O6 in 475g of water. Compute the freezing point and boiling point of the solution. Assume a density of 1.00g/mL for water.
Tuesday, September 18, 2012 at 11:56pm by Monica
chemistry freezing point
What is freezing point depression when 125g of br2 is added to 755g of Benzene? Kf(benzen e = 5.12°C\m.
Sunday, January 21, 2007 at 9:51pm by janee
Chemistry
The freezing point of benzene is 5.5°C. What is the freezing point of a solution of 8.50 g of naphthalene (C10H8) in 425 g of benzene (Kf of benzene = 4.90°C/m)? I worked this problem for someone just a couple of days ago. delta T = kf m kf = 4.90 m = molality = mols/...
Wednesday, January 24, 2007 at 2:47pm by Kelly
chemistry
calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of water (MgBr2=184 g, Kf for water =1.80 K kg mol-1)
Wednesday, June 12, 2013 at 6:41am by rahul
chemistry
A 0.100 m K2SO4 solution has a freezing point of -0.43°C. What is the van't Hoff factor for this solution? Kf = 1.86°C/m
Sunday, February 5, 2012 at 2:13pm by Anonymous
Chemistry
which property of a distilled water solution will not be affected by adding 50 mL of CH3OH to 100.mL of the water solution at 25? conductivity mass freezing point boiling point please help
Wednesday, February 23, 2011 at 10:55pm by Penny
chem hw
Assuming equal concentrations, rank these aqueous solutions by their freezing point: Li2SO4, Li3PO4, SnCl4, NH4Br. (from highest freezing point to lowest freezing poinT) Is the order Li3PO4, Li2SO4, SnCl4, and NH4Br???????? If not what is the correct order?
Sunday, February 19, 2012 at 1:46am by Amy
Chemistry
What is the (a) molality, (b) freezing point, and (c) boiling point of a solution containing 2.29 g napthalene (C10H8) in 44.6 g of benzene (C6H6)?
Friday, April 19, 2013 at 2:07pm by C
chemistry
What are the freezing point and boiling point of an aqueous solution of 15.5 g glucose(C6H12O6) dissolved in 150 g of water?
Sunday, April 7, 2013 at 9:56pm by Daniel
Chem-Molality
What are the boiling point and freezing point of a 0.22 m solution of sucrose in ethanol? Can someone help me with this quickly? I'm SO confused~!
Sunday, April 17, 2011 at 5:45pm by Hai
Chemistry
I'm not sure if i did this problem right or not. I keep reading through my book, and i think i followed the equations right, but i'm not confident with my answers. The problem: 5.0 g of glucose,C6H12O6, is disolved in 500.0 g of acetic acid. What is the new freezing ...
Friday, October 22, 2010 at 2:48am by Angelina
Chemistry
You need to proof this problem. I don't think the numbers are right. Freezing point of water is -1.86; I don't know how you can add a solvent to it to RAISE the freezing point.
Wednesday, February 22, 2012 at 4:47pm by DrBob222
CHM
freezing point of cyclohexane...yes I am using the depression of freezing point method
Wednesday, October 10, 2012 at 1:58pm by Adam
Chemistry
Suppose you had a 1.00 m solution of AlCl3. Assuming complete dissociation, what is the theoretical change in the freezing point of this solution?
Sunday, May 9, 2010 at 6:47pm by Celeste
chemistry
In comparing the phase diagram for water with that of a solution of sugar in water, all of the following decrease except a) the vapor pressure b) the boiling point c) the freezing point d) the triple point
Friday, February 3, 2012 at 4:28pm by jimmy
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