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October 2, 2014

Search: chem(freezing point)

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chem - freezing point
When 18 g of ethylene glycol C2H6O2 is dissolved in 150 g of pure water, the freezing point of the solution is _____ C. (The freezing point depression constant for water is 186C kgmol.
October 4, 2010 by jerry

Chem 1200
Freezing-point depression can be used to determine the molecular mass of a compound. Suppose that 1.28 g of an unknown molecule were added to 19.9 g of water and the freezing point of the solution determined. If the new freezing point of water were found to be -1.50C, what ...
January 26, 2011 by Rukky

chem
When saccharin is added to pure water, the freezing point of the resulting solution drops to -5.0C, Calculate the freezing point depression of the aqueous saccharin solution. Note: freezing point of pure water is O.0C... Stuck thanks so much!
January 16, 2013 by Lala

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?
February 19, 2012 by Amy

Chem(again)
What is the relationship between the amount of solute and the amount of freezing point depression? delta T = kf m where delta T is the difference between the normal freezing point and the f.p. with a solute, kf is the freezing point constant, and m is the molality. Some ...
February 6, 2007 by Chrissy

intro to chem
disolving sucrose, NaCl< and calcium chloried affect the boiling point of frezing point of water. Assuming that you have 0.1m solution of all these 3 compounds: a)rank then in order of decreasing freezing point. b) rank in order of increasing boiling point c)why do the ...
October 27, 2010 by julia

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...
May 29, 2007 by Anonymous

CHEMISTRY
Assuming equal concentrations, rank these aqueous solutions by their freezing point: LiSO4, Li3PO4, SnCl4, NH4Br. (from highest freezing point to lowest freezing poinT) Thanks.
February 18, 2012 by Kylie

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...?
March 24, 2011 by hannah

chemistry
if the freezing point of the solution had been incorrectly determined to be lower than the true freezing point, how would that affect the calculated molar mass? Explain. The molecular weight would be higher if the true freezing point is bigger than the determined freezing ...
February 1, 2009 by Anonymous

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 ...
April 13, 2010 by anonymous

Gen Chem II
Vitamin K is involved in normal blood clotting. When 1.36 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 4.56 C. The freezing point and Kf constant for camphor can be found here. Calculate the molar mass of vitamin K.
February 10, 2013 by Nefret

Chemestry
Calculate the freezing point of a solution containing 12.2grams of benzoic acid, C6H5CO2H, dissolved in 250 grams of nitrobenzene, C6H5NO2. The freezing point of nitrobenzene is 7.7 C, and its freezing point depression constant is 7.0 C/m.
October 26, 2008 by Joshua help please

chemistry
Calculate the freezing point of 0.15 m calcium chloride aqueous solution. Assume that the molal freezing point depression constant of water is 1.86Ckg/mol and that the freezing point of water is 0.00C
April 19, 2012 by hereyago

Chem
An ethylene glycol solution contains 20.9 g of ethylene glycol (C2H6O2) in 85.0 mL of water. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.) freezing point C boiling point C How would I set this up? thanks
March 22, 2011 by Lilly

Chemistry
If the freezing point of pure toluene is -95.15 oC and its freezing point depression constant is -8.38 oC/molal, what is the freezing point of a solution made by dissolving 39.338g of anthracene (C14H10) in 150.0mL of toluene? (Density of toluene = 0.8669g/mL)
January 30, 2013 by Jaden

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 ...
April 30, 2007 by Kim

Chemistry
calculate the freezing and boiling points of each of the following solutions. (a) 0.37 m glucose in ethanol freezing point ______I got -1.2e2 but its wrong_______C boiling point _________I got 1.1e2 but its wrong:(____C (b) 15.0 g of decane, C10H22, in 37.9 g CHCl3 freezing ...
March 24, 2011 by Rebekah

chemistry
10.0 g sample of p-dichlorobenzene, a component of mothballs, is dissolved in 80.0 g of benzene, C6H6. The freezing-point of the solution is 1.20oC. The freezing point of benzene is 5.48oC. The molal freezing point constant, kf, for benzene is 5.12oC/m. Calculate the apparent...
August 6, 2009 by Jim_R

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. any help would be ...
September 13, 2010 by lisa

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. any help would be ...
September 13, 2010 by lisa

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. any help would be ...
September 14, 2010 by lisa

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 acetic ...
February 18, 2013 by Ace

Chem 2
Assuming 100% dissociation, calculate the freezing point and boiling point of 2.44 m Na2SO4(aq)
February 6, 2014 by LLamaboy

chemistry
The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is ?0.072C. What would you expect the normal boiling point of this same solution to be? have no clue, thanks for the thelp Freezing point depression= N*kf* molality you have freezing point depression, ...
December 5, 2006 by tyler

Chem TWO
Assuming 100% dissociation, calculate the freezing point and boiling point of 2.91 m K3PO4(aq).
July 14, 2012 by Jenny

Chem
A solution is made by dissolving 0.584 mol of nonelectrolyte solute in 883 g of benzene. Calculate the freezing point and boiling point of the solution. Tf=? Tb=? I got Tf as 3.39 degrees Celsius I got Tb as 1.67 degrees Celsius It marked me wrong and said "You have given the ...
February 18, 2012 by Jen

CHEM- FP
camphor melts at 179.8 degrees, and it has a particularly high freezing point depression constant.(kf=40 degrees/m). when 0.186g of an organic substance of an unknown molar mass is dissolved in 22.01g of liquid camphor, the freezing point of the mixture is found to be 176.7 ...
October 8, 2010 by lucylu

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~!
April 17, 2011 by Hai

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 C. ...
September 7, 2007 by manny

chem
Calculate the freezing point and boiling point of a solution that contains 57.0 g NaCl and 53.4 g KBr dissolved in 750.3 mL H2O
March 3, 2011 by Anonymous

chemistry
a solution is prepared by mixing 2.17g of an unknown non-electrolyte with 225.0g of chloroform. The freezing point of the resulting solution is -64.2 C . The freezing point of pure chloroform is -63.5 C and its kf= 4.68C m^-1 . What is the molecular mass of the unknown? i know...
February 10, 2014 by hershi

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...
March 17, 2008 by Cameo

Chemistry
calculate the freezing point of a solution containing 12.2 grams of benzoic acid, dissolved in 250 grams of nitrobenzene. the freezing point of nitrobenzene is 5.7 celsius and its freezing point depression constant is 7.0 celsius/m. please help
October 27, 2008 by Joshua

chem
What is the freezing point (C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 C/m. whats wrong with my answer: molal: 0.069 moles Ca(NO3)2/0.115kg= 0.6 0....
September 26, 2010 by jessie

Chemistry
Calculate the boiling points of freezing points of the following solutions in water. a) boiling point of a 2.25m solution of propylene glycol (a non-electrolyte) b)freezing point of a 1.0m solution of potassium iodide c)freezing point of a 1.0m solution of nickel(II) nitrate d...
May 2, 2010 by Ralph

Chemistry
The boiling point of an aqueous solution is 102.48 C. What is the freezing point? I know that formula for freezing point is delta Tf = Kf*m but what do I plug in for each?
January 29, 2013 by Anon

Chemistry problem
What is the expected freezing point of a 3.50 m aqueous solution of BaCl2 (Kfp=1.86C/m)? What is the boiling point (Kbp=0.512C/m? & which is affected to the greater extent, the boiling point or the freezing point?
November 12, 2009 by Dan

Simple Chem Help
fill in the blank. The freezing point of a solution is_____ and the boiling point is ___________ than that of a pure solvent. lower...higher?
November 12, 2009 by Dan

Chemistry 1200
Freezing-point depression can be used to determine the molecular mass of a compound. Suppose that 1.28 g of an unknown molecule were added to 19.9 g of water and the freezing point of the solution determined. If the new freezing point of water were found to be -1.50C, what ...
January 26, 2011 by Rukky

chemistry
you are conducting a freezing-point determination in the laboratory by using an aqueous solution of KNO3. The observed freezing point of the solution is -1.15 C. Using a pure water sample, you recorded the freezing point of the pure solvent of the same thermometer as .25 C. ...
February 17, 2011 by Anonymous

chem
a compound containing only boron, nitrogen and hydrogen was found to be 40.3% B, 52.2%N, and 7.5% H by mass. If 3.301g of this compound is dissolved in 50.00g of benzene, the solution produced freezes at 1.30 degrees celsius. If Kf(freezing point depression constant) for ...
November 7, 2008 by tomi

Chemistry
Explain why the freezing point of a pure solvent is constant, whereas the freezing point of a solution decreases with steady cooling.
March 20, 2011 by Cassie

Chemistry
I am stuck in this problem I need to calculate the molality first so I could find T but I don't know which one is the solvent and which one is the solution the problem is to calculate the freezing point of a solution containing 12.2g of benzoic acid, dissolved in 250g of ...
October 27, 2008 by Maria

ap chem
Find the molecular mass of a solute by freezing point depression.
April 13, 2010 by anonymous

chem
How much energy is required to raise the temperature of 217 g of solid mercury at its freezing point to mercury vapor at its boiling point.
February 27, 2012 by science

chem
How much energy is required to raise the temperature of 217 g of solid mercury at its freezing point to mercury vapor at its boiling point.
February 27, 2012 by science

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?
October 14, 2010 by lulu

Chemistry
What Occurs as a salt dissolves in water? the number of ions in the solution increases and the freezing point decrease the number of the ions in the solution increase and the freezing point increase the # of ions in the solution decrease and the freezing point increase the # ...
March 26, 2007 by Kat

Chemistry
When 0.855 g of this solid was dissolved in 7.50 g of napthalene, the solution had a freezing point of 78.0 C. The pure solvent freezes at 80.0 C; its molal freezing point constant is 6.8 C/m. What is the molecular formula of the compound?
January 17, 2011 by Justyn

Physical Chemistry
When 1.33 g of a nonpolar solute was dissolved in 50.0 g of phenol, the latter's freezing point was lowered by 1.454C. Calculate the molar mass of the solute. The kf of phenol is 7.27 (Kkg)/mol. What is the normal boiling point of an aqueous solution that has a freezing ...
May 24, 2010 by Anonymous

chemistry
Could someone help me with these problems? 1. Why is it advantageous to choose a solvent with a large value for k(fp)? I don't really know 2. Why is it not necessary to wait for an entire sample of water to freeze in order to determine its freezing point? I think it has ...
March 4, 2009 by Karthik

Chemistry
Calculate the freezing point of a solution of 3.46 g of a compound,X,in 160 g of benzene. When separate sample of X was vaporised, its density was found 3.27 g/L at 116 c and 773 torr. The freezing point of pure benzen is 5.45 c, and kf is 5 .12 c/m.
October 30, 2011 by Ethio

9th grade chem
What is the freezing point depression of an aquous solution of 10.0 g of glucose in 50.0 g H2O?
December 14, 2010 by Gabrielle

Chemistry
Name and describe two colligative properties that are affected by solute concentration, then list whyone would be affected in that manner. So this is what i put for my answer Lowers freezing point: Each additional level of molal concentration lowers the freezing point. The ...
May 26, 2012 by Carrie

chemistry... please help!
Pure glacial acetic acid HC2H3O2 has a freezing point of 16.62 degrees C. Its freezing point depression constant is Kf=3.57 Cm^-1. A solution was made by taking 9.755 g of an unknown non-electrolyte and dissolving it in 90.50 g of glacial acetic acid. The measured freezing ...
February 13, 2009 by Anonymous

chemistry
Assuming equal concentrations, rank these aqueous solutions by their freezing point.? K2CO3, Li3PO4, Sn(ClO3)4, NH4I I tried to rank them according to the number of ions but i can't get it. highest freezing point --> lowest freezing point Sn(ClO3)4 -> Li3PO4 -> K2CO3...
February 19, 2012 by Eric

chemistry
If the freezing point of the solution had been incorrectly read 0.3degrees C lower than the true freezing point, would the calculated molar mass of the solute be too high or too low? Explain.
February 20, 2013 by mm

Chemistry
How does dissolving a solute affect the boiling point or freezing point of the solution? What about the solution's vapor pressure? Read about Raoult's Law, freezing point depression and boiling point elevation.
March 6, 2007 by John

physical science
Dissolving sodium chloride in water will 1: raise the freezing point of the solution, 2. raise the freezing point of the sodium chloride, 3. lower the freezing point of the solution, or 4. lower the freezing point of the sodium chloride?
November 6, 2007 by palmer

chem
How many moles of ethylene glycol must be dissolved in 500 g of water (Kf = 1.86) to lower the freezing point to -5.00 0C?
February 5, 2008 by Mark

9th grade chem
estimate the freezing point of an aqueous of 10.0 g of glucose dissolved in 500.0 g of water
December 14, 2010 by Gabrielle

Science
What is waters freezing point? What is Magnesium and Ammonias freezing point?
March 2, 2009 by Logan

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 ...
February 19, 2012 by Akle

chemistry
Ok, in my lab, I measured the freezing point of NaNO3 and it was 0.79 C and I have to answer the question: Why might your measured value of the freezing point of water not equal 0oC?
January 31, 2009 by Anonymous

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?
January 14, 2011 by Maria

chemistry
A solution is made by dissolving 21.5 grams of glucose (C6H12O6) in 255 grams of water. What is the freezing-point depression of the solvent if the freezing point constant is -1.86 C/m?
September 25, 2011 by ryan

chemistry
the addition of 50 g of salt to a sample of pure water causes its freezing point to be reduced from 0.0 C to -3. 15 C. Determine how by how many degrees the freezing point dropped for every 10 g of salt added?
January 29, 2013 by Ya Girl

Chemistry
What is the freezing point of a solution prepared by adding 264g of copper(ii) sulfate to 4 liters of water? The freezing point constant of water is 1.86C/m.
March 9, 2014 by Bruce Wayne

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...
September 16, 2010 by lisa

chemistry
The procedure described in this experiment was used to determine the molar mass of unknown liquid (non-electrolyte). The solution was made by mixing 0.961 g of the unknown with 100.0 g of water. The freezing point depression of the solution was −3.7C. Calculate the ...
April 19, 2012 by hereyago

Chemistry II
If the freezing point depression (DTf) is 5.62 and the freezing point depression constant (Kf) is 3.90, what is the molality of the solution? Assume that the solute is a nonelectrolyte (i = 1).
September 8, 2009 by Lindsay

Chemisty
A solution contains 20g of C^6H^12O^6 in 250g of water. What is the freezing-point depression of the solvent? What is the Freezing point of the solvent?
March 7, 2010 by Veronica

Chem
What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 216.2 g water to give a solution with a freezing point of -1.62 C?
March 31, 2010 by Stephany

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 ...
September 15, 2010 by lisa

chemistry
What is the expected freezing point of a 3.50 m (m standing for molality)aqueous solution of BaCl2(Kfp= 1.86 degrees Celsius/m)? What is the expected boiling point(Kbp= 0.512 degrees Celsius/m)? which is effected to the greater extent, the boiling point or freezing point? ...
April 7, 2013 by Patricia

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.
March 29, 2013 by kat

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.
April 6, 2013 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.
April 6, 2013 by MadiB PLEASE HELP :(

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.
February 13, 2013 by Jonah

11th Grade Chemistry
The freezing point of an aqueous solution that contains a non-electrolyte is -9.0 degrees celcious. A. What is the freezing-point depression of the solution? B. What is the molal concentration of the solution?
April 27, 2010 by Taylor

general chemisty
Calculate the freezing point of a solution of 20.0 g methyl salicylate, C7H6O2, dissolved in 800 g of benzene, C6H6. Kf for benzene is 5.10C /m and the freezing point is 5.50C for benzene. A) -1.05C B) 1.05C C) 4.45C D) 6.54C
September 26, 2010 by Amy

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.
February 12, 2012 by Hannah

Chemistry
What will be the freezing point of a solution made by dissolving 5.25 g of naphthalene (C10H8) in 100.0 g benzene (C6H6?). The normal freezing point of benzene is 5.5C and K f (benzene) is 5.12C / m.
September 4, 2014 by Emily

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 5.48C; Kf is 5.12C/m.
May 6, 2009 by Stephanie

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 ...
May 2, 2011 by Tina

chemistry
Camphor, C16H16O which has a freezing point of 174C, has a freezing point depression constant of 40.0C/m. Explain the usefulness and the limitation of camphor as a solvent for determination of molecular weights. For whose kind(s) of solute would camphor be especially useful?
March 7, 2010 by iain

chemistry
A 0.750 g sample of an unknown substance is dissolved in 20.0 g of benzene, C6H6. The freezing point of the solution is 4.53 oC. Calculate the molar mass of the substance. The normal freezing point for benzene is 5.53 oC and Kf is 5.12 oC/m.
February 9, 2010 by CC

chemistry
A 0.750 g sample of an unknown substance is dissolved in 20.0 g of benzene, C6H6. The freezing point of the solution is 4.53 oC. Calculate the molar mass of the substance. The normal freezing point for benzene is 5.53 oC and Kf is 5.12 oC/m.
February 9, 2010 by CC

Chemistry
The molal freezing point constant(Kf) for acetic acid is 3.90 C/m. When 31.5 grams of unknown solute is dissolved in 650 grams of acid the freezing point is lowered by 0.79 what is the molar mass
March 7, 2013 by Chris

college chemistry
the normal freezing point of the element mercury, Hg(l), is a -38.9C and its molar enthalpy of fusion, ΔHfusion=2.29 KJ/mol. What is the entropy change (J/K) of the system when 50 g of Hg(l) freezes at the normal freezing point. Hg= 200.59 g/mol
December 6, 2010 by Jamaal

Chemisrty
the freezing point of water is -1.86 degree Cm, if 5.00 g Na2SO4 is desolve at 45.0g H2o the freezing point is changed by -3.82 degree C. Calculate the Van't Hoff Factor for Na2SO4
April 26, 2014 by saemreza

chemistry
the freezing point of water is -1.86 degree Cm, if 5.00 g Na2SO4 is desolve at 45.0g H2o the freezing point is changed by -3.82 degree C. Calculate the Van't Hoff Factor for Na2SO4
April 26, 2014 by saemreza

Bio Chem
What would the freezing point of water be if one prepared a 10 m solution of urea in water? (Tfp = 1.86C/m x m)?
November 29, 2010 by Anonymous

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....
February 25, 2013 by JJ

Chemistry
A crystalline white solid is a mixture of glucose (C6H12O6) and sucrose (C12H22O11). Is it possible that a 10.00 g sample of the solid dissolved in 100.0 g H2O might have a freezing point of -1.25 degrees C? Explain. Answer: No. The freezing point would be -1.03 degrees C
February 25, 2013 by JJ

chemistry
i need to know if I am in the right tract please let me know...I am calulating the molality of the following exercise so I could be able to apply the formula T=Kf * molality calculate the freezing point of a solution containin 12.2 grams of benzoic acid, dissolved in 250 grams...
October 27, 2008 by Joshua

Chem
1.10g of an unknown compound reduces the freezing point of 75.22g benzene from 5.53C to 4.92C. What is the molar mass of the compound?
February 4, 2011 by emerald

Chemistry
The freezing point of benzene is 5.5C. What is the freezing point of a solution of 8.50 g of naphthalene (C10H8) in 425 g of benzene (Kf of benzene = 4.90C/m)? I worked this problem for someone just a couple of days ago. delta T = kf m kf = 4.90 m = molality = mols/kg. ...
January 24, 2007 by Kelly

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.
August 4, 2008 by Jared

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