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April 21, 2014

Search: Chemistry:Freezing Points

Number of results: 113,094

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...
Sunday, May 2, 2010 at 11:31pm 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.
Sunday, November 11, 2012 at 9:19pm by Anonymous

chemistry
50C is halfway between the freezing and boiling points of water (0C and 100C) 50F is is slightly above the freezing point (32F) and well below the boiling point (212F)
Wednesday, September 26, 2012 at 5:22pm by Scott

Chemisty-Freezing Points
A 1.60 g sample of napthalene (a non-electrolyte with a formula of C10H8) is dissolved in 20.0 g of benzene (C6H6). The freezing point of benzene is 5.5C and Kf = 5.12 kg/mol. What is the freezing point of the solution?
Sunday, January 21, 2007 at 9:51pm by Anonymous

Chemistry:Freezing Points
I'm not sure as to whether or not spreading salt on sidewalks would be beneficial, considering the outside temperature. The freezing point of pure H2O is 0 C or 32 F. But Im not sure what that would infer?
Sunday, November 11, 2012 at 9:19pm 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 ...
Thursday, March 24, 2011 at 7:09pm by Rebekah

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

Chemistry
Follow the problems you've already done above on freezing points.
Monday, February 25, 2013 at 2:19am by DrBob222

chemistry
If you are talking about the freezing point method there will be no effect. WHY? Because the reading of the normal freezing point is 1 degree too high and the reading for the freezing point of the solution containing the solute is alo 1 degree too high; however, the DIFFERENCE...
Sunday, February 10, 2013 at 10:08pm by DrBob222

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 ...
Saturday, February 18, 2012 at 10:34pm by Jen

Chemistry
Delta tf is the CHANGE in freezing point. The initial freezing point was not 9C. Water freezes at 0C, and then when you add a solute, the freezing point is depressed some.
Wednesday, February 3, 2010 at 10:25am by bobpursley

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.
Saturday, February 18, 2012 at 11:03pm by Kylie

Science
What might be the differences between liquids in a mixture? They might have different... what? Boiling points? Freezing points? Density, which in liquids we often measure as specific gravity. If it's a mixture, the two liquids will very probably have different boiling points, ...
Saturday, September 19, 2009 at 2:37pm by jim

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 ...
Monday, May 24, 2010 at 2:50pm by Anonymous

chemistry
molality is used for colligative properties: vapor pressure, boiling, freezing points
Tuesday, May 25, 2010 at 8:40pm by bobpursley

Chem II
How do you figure freezing points and boiling points?
Thursday, February 14, 2008 at 3:56pm by Ken

Chem
The comment made by the teacher explains what to do. Look up the freezing and boiling points of pure benzene and apply the appropriate corrections. You did not calculate the freezing and boiling points. You calculated the changes from the pure compound (benzene), and you did ...
Saturday, February 18, 2012 at 10:34pm by drwls

Chemistry
Determine the freezing points of each 0.20m aqueous solution. a)K2SO4 b)CsNO3 c)Al(NO3)3
Thursday, April 29, 2010 at 5:31pm by Jack

Chemistry:Freezing Points
What's your main problem with this? Is it not obvious that if NaCl will lower the f.p. by 17 C and the T is -8 then ....... What is the f.p. of pure H2O?
Sunday, November 11, 2012 at 9:19pm by DrBob222

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...DRBobb i have a questionnnn
Delta T is the difference between the normal freezing point and the freezing point of the solution. I wondered how you obtained a freezing point of 23 BUT I figured you had somehow managed it so 23 + 0.1 was the difference. If the freezing point of the solution before the ...
Sunday, February 8, 2009 at 8:13pm by DrBob222

chemistry
Assuming equal concentration rank these by freezing points, Na3PO4, Li2Co3,NH4Cl, and Sn(NO3)4
Sunday, January 27, 2013 at 7:50pm by chelsea

Math
In the celsius scale, the difference between the freezing and boiling points of water, at 0 and 100 degrees, is 100 degrees. In the farenheit scale, the freezing point of water is 32 degrees, while the boiling point is 212 degrees, placing the boiling and freezing points of ...
Wednesday, November 12, 2008 at 7:29am by Victor

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
Thursday, April 19, 2012 at 2:39am 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 ...
Sunday, February 1, 2009 at 1:34am by Anonymous

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 ...
Thursday, May 19, 2011 at 10:25am by Adam

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...
Friday, January 5, 2007 at 7:15pm by Belinda

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...
Wednesday, May 12, 2010 at 8:29pm by kayci

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

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?
Wednesday, January 12, 2011 at 7:30am 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?
Wednesday, January 12, 2011 at 7:38am by paul

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...
Wednesday, May 12, 2010 at 6:56pm by kayci

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...
Sunday, January 21, 2007 at 9:51pm by Swim4eva

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?
Monday, April 22, 2013 at 1:01pm by Ali

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...
Thursday, August 6, 2009 at 12:24pm by Jim_R

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
Friday, February 15, 2008 at 4:14am by josh

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)
Wednesday, January 30, 2013 at 9:34pm by Jaden

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?
Tuesday, November 2, 2010 at 6:20pm 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?
Wednesday, April 6, 2011 at 12:36am 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?
Wednesday, April 6, 2011 at 12:36am by Tina

chemistry
You will need to read in your text and look on the web for most of your information. First off, HCl is a gas and NaCl is a solid. HCl is a polar covalent bond while NaCl is an ionic bond. You can look up the boiling points, freezing points, delta H and that information. That ...
Tuesday, September 22, 2009 at 12:43pm by DrBob222

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
Monday, October 27, 2008 at 8:50am by Joshua

Chemistry:Freezing Points
The freezing point is zero C normally. Spreading (or spraying) saturated NaCl solution CAN lower it by 17 degrees C according to the problem. The temperature is only -8 C, therefore, the ice would melt. In fact it would melt with an outside temperature of -16 C but it would ...
Sunday, November 11, 2012 at 9:19pm by DrBob222

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 ...
Sunday, November 5, 2006 at 5:39pm by Gemma

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...
Monday, February 10, 2014 at 11:16pm by hershi

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

Chemistry
delta T = Kf*m, then solve for freezing point knowing that 0C is the normal freezing point of an aqueous solution.
Tuesday, January 18, 2011 at 12:39am 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

Chemistry
Explain why the freezing point of a pure solvent is constant, whereas the freezing point of a solution decreases with steady cooling.
Sunday, March 20, 2011 at 11:39pm by Cassie

chemistry freezing point
What is freezing point depression when 125g of br2 is added to 755g of Benzene? Kf(benzen e = 5.12C\m.
Sunday, January 21, 2007 at 9:51pm by janee

Chemisty-Freezing Points
.553
Sunday, January 21, 2007 at 9:51pm by Anonymous

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.
Monday, February 14, 2011 at 2:10pm by redgy

science
using a fahrenheit thermometer, what temp is 22 degrees below freezing. Freezing on F is what? Freezing - 22 = ??
Monday, November 6, 2006 at 6:00pm by jataya

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

chemistry
(a) x = 273.15 Kelvin (b) p = freezing (c) heat of freezing (d) Q = melting (e) heat of fusion
Saturday, June 11, 2011 at 3:12am by Jai

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?
Sunday, February 26, 2012 at 10:41am by pat

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 ...
Wednesday, January 26, 2011 at 9:47pm by Rukky

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? ...
Tuesday, February 21, 2012 at 1:06pm by Hannah

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.
Tuesday, November 8, 2011 at 9:09am by Ethio

Chemistry
As the mixture reaches the freezing point, the solvent (in this case water?) freezes which makes the solution more concd in alcohol. A more concd solution means the freezing point is decreased. This continues which makes the freezing point a broad range instead of a sharp point.
Wednesday, February 23, 2011 at 5:02pm by DrBob222

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. ...
Thursday, February 17, 2011 at 7:10pm by Anonymous

Chemistry
Your problem is that you are not substituting delta T. Instead, you are substituting the freezing point of the solution. delta T = (difference between freezing point of the pure solvent and freezing point of the solution). In this case that is 5.50-5.19 = ?? I took a quick ...
Sunday, March 20, 2011 at 11:23pm by DrBob222

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

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 will ...
Monday, November 7, 2011 at 3:20pm by DrBob222

Chemistry
As the solution is cooled, at some point lower than the normal freezing point of the solvent, a few crystals of pure solvent freeze. That makes the remaining solution more concd in the solute which lowers the freezing point more and the solution must be cooled more to freeze ...
Sunday, March 20, 2011 at 11:39pm by DrBob222

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.
Wednesday, February 20, 2013 at 5:14pm by mm

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?
Tuesday, January 29, 2013 at 9:22pm by Anon

physics
What is the boiling and freezing points of celsius scale and kelvin
Sunday, July 17, 2011 at 3:06pm by Gift

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 ...
Monday, October 27, 2008 at 12:02am by Maria

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?
Monday, January 17, 2011 at 11:32pm by Justyn

chemistry
so water would have the highest freezing point? it wouldn't be aqueous NaI at 0.010 m ? i thought that lower concentration means higher freezing point, or is that only if they are all the same compound ?
Monday, November 5, 2012 at 10:49pm by Ania

Chemistry
Google freezing point, ethane freezing point, methane
Wednesday, May 18, 2011 at 2:11pm by bobpursley

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

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?
Sunday, December 5, 2010 at 5:04pm by regina

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.
Tuesday, March 8, 2011 at 8:39pm by Bianca

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...
Wednesday, May 12, 2010 at 7:02pm by kayci

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?
Wednesday, April 1, 2009 at 1:30pm by michelle

Chemistry
Two points here. 1. You told me how you did the freezing point data but I'll summarize it here. dT = Kf*m 0.0894 = 1.86*m m = about 0.048 m = mols/kg solvent so mol = m x kg solvent = 0.048*0.025 = about 0.0012 (you can do these more accurately). Then molar mass = g/mols = 0....
Tuesday, August 6, 2013 at 9:26pm by DrBob222

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

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
Thursday, March 29, 2012 at 7:57pm by Kristie

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, ...
Tuesday, December 5, 2006 at 2:59pm by tyler

Chemistry
Is 0.172 mol ethanol really 0.003734 g? Isn't it 0.172mol x 46 g/mol = 7.912 g? If you still have a problem, post the boiling point and freezing points of ethanol. I wouldn't want you to become homeless. ;-)
Saturday, April 7, 2012 at 6:01pm by DrBob222

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.
Sunday, March 9, 2014 at 12:01am by Bruce Wayne

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?
Saturday, January 31, 2009 at 8:28pm by Anonymous

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).
Tuesday, September 8, 2009 at 8:42pm by Lindsay

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?
Sunday, September 25, 2011 at 6:17pm by ryan

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.
Sunday, October 30, 2011 at 5:11pm by Ethio

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?
Friday, January 14, 2011 at 4:24pm by Maria

Chemistry
delta T = 101-100 = ?? delta T = Kb*molality Solve for molality. Now use the molality in the freezing point equation. delta T = Kf*m You have Kf and m, solve for delta T and convert to freezing point knowing the normal freezing point is zero C.
Thursday, April 21, 2011 at 10:40pm by DrBob222

chemistry
The solution with the greatest freezing-point depression, ΔTf, will have the lowest freezing point. Freezing-point depression is directly proportional to the total particle concentration. You need to compare the ions per formula unit. From highest to lowest the order is...
Sunday, February 19, 2012 at 6:44pm by JSJFJF

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?
Tuesday, January 29, 2013 at 11:45am by Ya Girl

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 ...
Wednesday, March 4, 2009 at 2:00am by Karthik

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.
Monday, October 4, 2010 at 2:19pm by jerry

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.
Sunday, October 26, 2008 at 5:38pm by Joshua help please

8th grade science
How does altitude affect the freezing, melting and boiling points of water?
Sunday, September 29, 2013 at 4:41pm by A

chemistry FP depression
What are the freezing point constants for the two solvents? Wouldn't the larger freezing point constant provide more temperature change and make reading the delta T more accurate (relatively)?
Tuesday, April 23, 2013 at 12:21am by DrBob222

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?
Tuesday, April 27, 2010 at 3:52pm by Taylor

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
Tuesday, February 8, 2011 at 9:37am 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
Tuesday, February 8, 2011 at 9:37am by shaknocka lewis

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 ...
Friday, February 13, 2009 at 1:54pm by Anonymous

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