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November 21, 2014

Search: Chemistry:Freezing Points

Number of results: 54,684

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: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.
November 11, 2012 by Anonymous

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

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

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

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

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

Chemistry
Determine the freezing points of each 0.20m aqueous solution. a)K2SO4 b)CsNO3 c)Al(NO3)3
April 29, 2010 by Jack

chemistry
Assuming equal concentration rank these by freezing points, Na3PO4, Li2Co3,NH4Cl, and Sn(NO3)4
January 27, 2013 by chelsea

chemistry
What would be the freezing and boiling points of a solution of 5.00g of sodium chloride dissolved in 25.0g of water?
May 9, 2014 by Jaques

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 ...
February 2, 2012 by Larry

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

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

Chem II
How do you figure freezing points and boiling points?
February 14, 2008 by Ken

Chemistry
What would be the freezing and boiling points of a solution prepared by dissolving 1.00g of benzoic acid (C6H5CO2H) in 10.0g of benzene?
May 9, 2014 by Jaques

Chemistry
3) The chemical formula for ethylene glycol (antifreeze) is C2H6O2 and Isopropyle alcohol is C3H7OH. Calculate the new boining and freezing oints for 1000.0 g of aqueous solution (total volume), that is 30.0% solute (the antifreeze and the alcohol are the solutes). You will ...
May 19, 2011 by Adam

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

Chemistry
Assuming equal concentrations and complete dissociation, rank these aqueous solutions by their freezing points: Li2SO4 K3PO4 LiNO3
November 5, 2014 by Dustin

science
using a fahrenheit thermometer, what temp is 22 degrees below freezing. Freezing on F is what? Freezing - 22 = ??
November 6, 2006 by jataya

chemistry
Arrange the following aqueous solutions in order of increasing freezing points (lowest to highest temperature): 0.10 m glucose, 0.10 m BaCl2, 0.20 m NaCl, and 0.20 m Na2SO4.
March 8, 2011 by Bianca

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

Chemistry - Van't Hoff Factor
How does the van't hoff factor relate to freezing points? If one van't hoff factor is bigger than another, is its freezing point lower or greater? delta Tf = iKfm. So increasing i will increase delta Tf Van't Hoff factor is the concentration of particles in a solute, so, if it...
January 5, 2007 by Belinda

Chemisty-Freezing Points
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)? delta T = Kf m m = mols/kg solvent. Change 8.5 g naphthalene to mols and 425 g benzene to kg. That will get delta T...
January 21, 2007 by Swim4eva

chem
what are the normal freezing points and boiling points of the following solutions: a. 21.1g NaCl in 135mL of water b. 15.4g urea in 66.7 mL water?
January 12, 2011 by paul

chem
what are the normal freezing points and boiling points of the following solutions: a. 21.1g NaCl in 135mL of water b. 15.4g urea in 66.7 mL water?
January 12, 2011 by paul

Chemistry
Calculate the freezing of solution of 3.46 g of compound,X, in 160 g of benzen.when separated sample of X was vaporised, it density 3.27 g/L at 116 c and 773 torr. The freezing point of pure benzene is 5.45 c and Kf is 5.12 c/m.
November 8, 2011 by Ethio

chemistry
What is the osmotic pressure in torr of a 0.0155 M glucose solution at body temperature ( 35.7 C)? What are the boiling and freezing points for the same solution?
April 22, 2013 by Ali

science
When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these solutions, however, are higher...
May 12, 2010 by kayci

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
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

chemistry
Is melting endothermic or exothermic? Things that are melting are taking on heat, endothermic Would freezing be the same? No, of course not. If melting is endothermic, then freezing must be exothermic. Believe it or not, and I know it sounds goofy, freezing water to ice is an ...
November 5, 2006 by Gemma

Chemistry
In calibrating a thermometer by setting only the freezing and boiling points, what assumptions are you making regarding the internal diameter of the thermometer and the expansion of alcohol?
November 2, 2010 by Chris

chemistry
In calibrating a thermometer by setting only the freezing and boiling points, what assumptions are you making regarding the internal diameter of the thermometer and the expansion of alcohol?
April 6, 2011 by Tina

chemistry
In calibrating a thermometer by setting only the freezing and boiling points, what assumptions are you making regarding the internal diameter of the thermometer and the expansion of alcohol?
April 6, 2011 by Tina

science
When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these solutions, however, are higher...
May 12, 2010 by kayci

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

science
Boiling points and freezing points are examples of? a. physical properties b. matter c. chemical properties d. energy i am pretty sure it is a but i just need to have someone assure to me i am right
February 15, 2008 by josh

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...
January 23, 2013 by Hannah

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
Why would it not be useful to just use pure ethanol or pure ethylene glycol as an antifreeze since their normal freezing points are -114.1 C abd -12C respectively.
February 14, 2011 by redgy

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

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

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

Chemistry
Why is heating required for this formation: 6NaOH (aq) + Al2(SO4)3 (aq) 2Al(OH)3 (s) + 3Na2SO4 (aq)? Wouldn't freezing favour the formation of Al(OH)3 since freezing lower the KSP and more Al(OH)3 would precipitate?
March 22, 2010 by Alan

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

chemistry 111
in calibrating your thermometer by setting only the freezing and boiling points, what assumptions are you making regarding the internal diameter of the thermometer and the expansion of the thermometer fluid?
February 26, 2012 by pat

Chemistry
I had to perform an experiment for the freezing point depression in which we had to determine the frezzing points of water as a pure solvent, sodium chloride, sucrose, and ethylene glycol. We had to work with a partner so I completed the experiment for water, NaCl, and the ...
February 20, 2012 by Hannah

Chemistry
1) For a freezing point depression experiment we had to create an ice bath and add salt to the ice. I have to answer the question, why was salting the ice necessary in order to complete the experiment and how does this apply to the principles/concepts behind this experiment? ...
February 21, 2012 by Hannah

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
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

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
How many grams of Urea would you have to dissolve in 500ml of H2O in order for the mass percent of H2O to be 88.8%? What is the mole fraction of Urea? What are the new boiling and freezing points?
December 5, 2010 by regina

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

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

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

physics
What is the boiling and freezing points of celsius scale and kelvin
July 17, 2011 by Gift

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... 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

science
When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these solutions, however, are higher...
May 12, 2010 by kayci

physics
What are the temperatures for freezing water and boiling water on the Kelvin temperature scale? a)273K for freezing water; 373K for boiling water b)0K for freezing water; 100K for boiling water c)32K for freezing water; 212K for boiling water
March 29, 2012 by Kristie

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

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

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 :(

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

math
When converting Farrenheit to Celcius, why is there only 32degrees difference between the freezing points of 32 and 0, but 110 degrees difference between the boiling points of 210 and 75 degrees?
April 1, 2009 by michelle

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

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

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
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
why would it not be useful to just use pure ethanil or pure ethylene glycol as aN ANTIFREEZE SINCE THEIR NORMAL FREEZING POINTS are -114.1 degrees celsius and -12 degrees celsius respectively
February 8, 2011 by shaknocka lewis

chemistry
why would it not be useful to just use pure ethanil or pure ethylene glycol as aN ANTIFREEZE SINCE THEIR NORMAL FREEZING POINTS are -114.1 degrees celsius and -12 degrees celsius respectively
February 8, 2011 by shaknocka lewis

8th grade science
How does altitude affect the freezing, melting and boiling points of water?
September 29, 2013 by A

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 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

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

chemistry lab
why would it not be useful to just use pure ethanil or pure ethylene glycol as aN ANTIFREEZE SINCE THEIR NORMAL FREEZING POINTS are -114.1 degrees celsius and -12 degrees celsius respectively
February 7, 2011 by shaknocka

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

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

chemistry
what do coefficents represent in a balanced equation? What would removing air from a sealed container do to the container? What does it mean that "like dissolves like"? Dissolving a solute in a solvent does what to the solven'ts freezing and boiling points? What must be true ...
June 10, 2008 by Miley

chemistry
Which of the following pairs are both exothermic processes? Question options: a. Evaporation/melting b. Evaporation/freezing c. Condensation/melting d. Condensation/freezing
March 8, 2014 by peterson

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

physics
Figure 18-23 shows three linear temperature scales, with the freezing and boiling points of water indicated.
September 28, 2012 by Anonymous

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

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 1.86C/m. (Note that when Ca(NO3)2 dissolves in water Ca2+ and NO32- ions are produced).
May 25, 2012 by Henry

Chemistry
Vitamin K is involved in normal blood clotting. When 2.40 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 8.05 C. The freezing point and Kf constant for camphor can be found here. Calculate the molar mass of vitamin K.
October 16, 2013 by Shardai

Chemistry
Vitamin K is involved in normal blood clotting. When 2.40 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 8.05 C. Calculate the molar mass of vitamin K. Kf value is 37.8 and the normal freezing point is 176 degrees C
October 17, 2013 by Shardai

CHEMISTRY- PLEASE HELP:)!
Pure lauric acid is melted and the freezing point is determined to be 43 degrees celsius. A solution is made by dissolving .50 grams of paradicholrobenzene into 3.00 grams of lauric acid. Determine the molality of this solution. I got 1.1m. which is right. But then it says the...
April 16, 2008 by Miley

Chemistry
What is the freezing point of an aqueous 2.65 m calcium chloride (CaCl2) solution? The freezing point of pure water is 0.0C and Kf of pure water is -1.86C/m.
August 21, 2010 by David

Chemistry
What is the freezing point of an aqueous 2.25 m potassium nitrate (KNO3) solution? The freezing point of pure water is 0.0C and Kf of pure water is -1.86C/m.
August 26, 2010 by Cecillia

Chemistry
What is the freezing point of an aqueous 2.25 m potassium nitrate (KNO3) solution? The freezing point of pure water is 0.0C and Kf of pure water is -1.86C/m.
August 26, 2010 by Cecilia

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