Search: chem(freezing point)

Number of results: 36,318

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

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

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 -1.50°C, ...
Wednesday, January 26, 2011 at 2:42pm by Rukky

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 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

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!
Wednesday, January 16, 2013 at 1:09pm by Lala

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 ...
Wednesday, October 27, 2010 at 8:40pm by julia

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 ...
Tuesday, February 6, 2007 at 5:39pm by Chrissy

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

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...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
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

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
Calculate the freezing point of 0.15 m calcium chloride aqueous solution. Assume that the molal freezing point depression constant of water is 1.86°C·kg/mol and that the freezing point of water is 0.00°C
Thursday, April 19, 2012 at 2:39am by hereyago

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

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 II
Boiling point. delta T = i*Kb*m where i = number of particles Kb is boiling point constant m = molality. freezing point. delta T = i*Kf*m where Kf is freezing point constant. i and m have same meaning as above.
Thursday, February 14, 2008 at 3:56pm by Anonymous

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

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
Tuesday, March 22, 2011 at 6:53pm by Lilly

Chem
moles ethylene glycol = grams/molar mass. molality = moles/kg solvent. Solve for molality. delta T = Kf*m Find freezing point form delta T knowing that the normal freezing point of water is zero C. Same procedure for boiling point except delta T = Kb*m and add delta T to 100 C...
Sunday, March 13, 2011 at 5:53pm by DrBob222

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.
Sunday, February 10, 2013 at 2:44pm by Nefret

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
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

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
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

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

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 ...
Tuesday, September 14, 2010 at 4:08pm by lisa

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

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 5.5°C and Kf = 5.12 kg/mol. What is the freezing point of the solution?
Sunday, January 21, 2007 at 9:51pm by Anonymous

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
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
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

Chemisty
moles = grams/molar mass. Calculate moles. m = moles/kg solvent. Calculate m delta T = Kf*m Calculate delta T. The freezing point of the solvent, normally, is 0o C. The freezing poing depression constant for the solvent, H2O, is 1.86 o/m. You may have rewritten the problem, ...
Sunday, March 7, 2010 at 7:37pm by DrBob222

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 ...
Thursday, March 24, 2011 at 7:09pm by Rebekah

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?
Thursday, November 12, 2009 at 4:19pm by Dan

Simple Chem Help
yes. It is called freezing point depression, and boiling point elevation.
Thursday, November 12, 2009 at 4:15pm by bobpursley

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
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
The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is ?0.072°C. 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

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

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
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

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 ...
Friday, October 8, 2010 at 10:41pm by lucylu

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 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 -1.50°C, ...
Wednesday, January 26, 2011 at 9:47pm by Rukky

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

Chem-Molality
delta T = Kb*molality. Look up Kb for ethanol and solve for delta T. You know the normal boiling point of ethanol, simply add delta T to find the new boiling point. Same procedure for freezing point except you subtract delta T from 0 C to find the new freezing point. delta T...
Sunday, April 17, 2011 at 5:45pm by DrBob222

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?
Thursday, November 12, 2009 at 4:15pm by Dan

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

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

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
Thursday, March 3, 2011 at 5:45pm by Anonymous

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 ...
Sunday, February 19, 2012 at 6:44pm by JSJFJF

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

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 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
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
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

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

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

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?
Tuesday, November 6, 2007 at 3:01pm by palmer

science
That depends upon the temperature setting of your freezer. It is adjustable, you know. A recommended setting is 0 F (-18 C) I suggest you calculate the freezing point depression of a fully saturated solution of NaCl. That will tell you how high the temperature setting will ...
Tuesday, February 22, 2011 at 5:35am by drwls

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

Science
What is waters freezing point? What is Magnesium and Ammonias freezing point?
Monday, March 2, 2009 at 6:47pm by Logan

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
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 ...
Saturday, May 26, 2012 at 9:04pm by Carrie

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.
Tuesday, March 6, 2007 at 10:55pm by John

CHEMISTRY
No. Li2SO4; i = 3 Li2SO4 ==> 2LI^+ + SO4^2- Li3PO4; i = 4 Li3PO4 ==L> 3Li^+ + PO4^3- NH4B4; i = 2 NH4Br ==> NH4^+ + Br^- SnCl4; i = 5 SnCl4 ==>: Sn^4+ + 4Cl^- Since delta T = i*Kf*m and the only variable is i, then the lowest i will have the lowest ...
Saturday, February 18, 2012 at 11:03pm by DrBob222

chem - freezing point
moles ethylene glycol = grams/molar mass solve for moles ethylene glycol. molality = mols/kg solvent solve for molality delta T = Kf*m solve for delta T Subtract delta T from zero C to obtain the freezing point.
Monday, October 4, 2010 at 2:19pm by DrBob222

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.
Monday, February 27, 2012 at 8:01pm by science

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 # ...
Monday, March 26, 2007 at 10:28pm by Kat

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...
Sunday, September 26, 2010 at 5:39pm by jessie

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
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 ...
Friday, November 7, 2008 at 3:27pm by tomi

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

science
freezing. melting point and freezing point are the same.
Wednesday, December 17, 2008 at 6:21pm by bobpursley

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
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... 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

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

chem lab (webwork)
The answer is A. Let me legitimitize my answer; Since you can use the freezing point depression equation to find the molar mass of the solute, the molar mass obviously has an effect on the freezing point. I think its pretty clear that C is true. B is true by the definition of ...
Monday, April 5, 2010 at 1:04am by Santa Clause

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?
Sunday, March 7, 2010 at 7:37pm by Veronica

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
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

ap chem
Find the molecular mass of a solute by freezing point depression.
Tuesday, April 13, 2010 at 11:39pm by anonymous

Chemistry
a)How much would the freezing point change in a 2.5m solution of phenol in benzene? (freezing point of phenol is 7.40 degrees C, freezing point of benzene is 5.12 degrees C) b)How much would the boiling point change in a 1.0m solution of magnesium chloride in ethanol? (boiling...
Monday, May 3, 2010 at 11:20pm by Danny

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
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? ...
Sunday, April 7, 2013 at 9:29pm by Patricia

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

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

molal
freezing point depression=k*molesglycering/kg ethanol New freezing point= original-depression
Tuesday, September 14, 2010 at 4:08pm by bobpursley

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 −3.7°C. Calculate ...
Thursday, April 19, 2012 at 2:39am by hereyago

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
I'm not sure what brought these questions on but the freezing point of anything is not a function of it being stirred or not. When a solid is heated slowly (and best with stirring so the heating is uniform), the solid will begin to melt. At the point that both solid and ...
Saturday, July 10, 2010 at 2:46pm by DrBob222

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
The effect is known as the depression of the freezing point and it is a colligative property. When a solute (NaCl) is dissolved in a solvent (water), the freezing point is lowered, the boiling point is raised, and the vapor pressure of the solvent is lowered. Since the ...
Thursday, June 3, 2010 at 6:27pm by DrBob222

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