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August 29, 2014

Search: Chemistry: molality and freezing point?

Number of results: 60,471

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(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
Five (5.00) grams of glucose, C6H12)6, is dissolved in 500.0 grams of acetic acid. What is the new freezing point and boiling point for the solution? Kf acetic acid = 3.90, Kb acetic acid = 3.07 (normal freezing point for acetic acid = 16.60 dg C, boiling point = 118.5 dg C) f...
August 9, 2007 by lana

AP Chemistry
Why would .25 molality of CaCl2 have a larger effect on the freezing point of water than .25 molality of NaCl?
January 19, 2014 by Diamond

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
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

Chemistry
Colligative Properties The freezing point of distilled water was determined by recording a thermogram: -0.176. The freezing point of a 0.200 m (molality) solution containing an unknown, ionic compound was determined by recording a second thermogram. a. Determine the freezing ...
January 28, 2014 by Sam

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
which of the following would be expected to have the lowest freezing temperature? a. Ca(NO3)2 b. NaC2H3O2 c. CuSO4 d. HC2H3O2 e. C2H5OH per what? per gram? per mol? Any could have the lowest freezing point if I put a cup of any one and a scant amount of the others. For equal ...
April 21, 2007 by mary

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
Colligative Properties The freezing point of distilled water was determined by recording a thermogram: -0.176 degrees Celsius. The freezing point of a 0.200 m (molality) solution containing an unknown, ionic compound was determined by recording a second thermogram: -.904 ...
January 28, 2014 by Sam

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
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
which solution has highest freezing point if all are at the same molality calcium chloride sodium nitrate potassium sulfate iron(III) nitrate all have same freezing point please explain
March 16, 2012 by kim

Chemistry
What is the (a) molality, (b) freezing point, and (c) boiling point of a solution containing 2.29 g napthalene (C10H8) in 44.6 g of benzene (C6H6)?
April 19, 2013 by C

chemistry, freezing point depression
Hey guys I did a lab and I have to answer the questions relating to the lab. I did question 1 & 2, can someone check if they are correct, and question 3 I don't know how to do it. 1. Calculation to Determine the molecular weight of unknown substance Mass of unknown used: 2.0 g...
February 6, 2009 by Sev

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

Chem help!!
A rock salt (NaCl), ice, and water mixutre is used to make homemade ice cream. How many grams of rock salt must be added to lower the freezing point 10.0 degrees C? I have no idea what to do, please help! delta T = Kf*i*m delta T = 10. Kf is the molal freezing point constant, ...
May 3, 2007 by Lindsay

chemistry
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 1.86C kg) what i tried was 18/62 to find the moles. then i got .29/.150 to solve for the molality. then i ...
April 7, 2008 by david

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
lowest+freezing+point+of+Kbr+AlNO33+CH3COONa+NaNO2+MgCl2+of+same+molality
March 29, 2013 by deepak

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
Cyclohexane has a freezing point of 6.6 degree Celsius and a K(f) of 20.0 degree Celsius/m. 1.50g of an unknown solute is dissolved wth 18.0g of cyclohexane. The freezing point of the solution was 1.3 degree Celsius Using this iInformation assuming the solute doesn't ...
May 27, 2013 by Michael

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

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
Calculate the freezing point depression and osmotic pressure at 25 degrees C of an aqueous solution of 1.0 g/L of a protein (mol wt= 90,000) if the density of the solution is 1.0 g/mL. I know how to calculate freezing point depression and osmotic pressure, but I'm having ...
March 24, 2007 by Jessica

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
a solution of 0.2113 g of water dissolv ed in 25g of a solvent freezes at 11.5 degrees celcius below the freezing point of the solvent. what is the Kf for the solvent? A)0.735 B)1.36 c)5.39 D)24.5 Help!!! delta T = Kf*molality Calculate molality = #mols solute/kg solvent, plug...
April 27, 2007 by natali

Chemistry
I did an experiment to determine the freezing point depression and then find the molecular weight of the unknown solute added to the solvent, what would be the effect on calculating the molecular weight if some cyclohexane(my solvent) evaporated while the freezing point of the...
February 25, 2009 by Lauren

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

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
Hey guys I did a lab and I have to answer the questions relating to the lab. I did question can someone please check if these are accurate 1. Calculation to Determine the molecular weight of unknown substance Mass of unknown used: 2.0232 g Mass of water used: 50.0 g (0.05kg) ...
February 3, 2010 by Saira

chemistry
The freezing-point depression is -0.930 Celsius degree. Determine the molality of the solution of an unknown nonelectrolyte in water. Please help!! I do not understand this problem!
February 7, 2012 by vivian

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

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
When a certain amount of MgF2 is added to water, the freezing point lowers by 3.5 oC. What was the molality of the magnesium fluoride? (Kf for water = 1.86 oC/m)
February 10, 2012 by lw

chemistry
A 0.0230 g sample of an unknown was dissolved in 2.260 g of benzene. The molality of this solution, determined by freezing point depression, was 0.0408 m. What is the molecular weight of the unknow substance?
October 4, 2012 by Crystal

Chemistry
An aqueous solution of an unknown compound boils at 101.00 degrees Celsius (760 torr). What is the molality, and freezing point of this solution?
April 21, 2011 by John

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 8, 2008 by tomi

science
hi guys I really need some help with my homework its so confusing here it is. 5.00g of glucose,C6H12O6, is dissolved in 500g of acetic acid. What is the new freezing point and boiling point for the solution? Kf,acetic acid = 3.90 Kb,acetic acid = 3.07 (normal freezing point ...
March 24, 2007 by stacy

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

chemistry is this answer right
115 grams of KCl is dissolved in 750 ml of water. what are the molality, molarity, mole percent, % mass, ppm by mass. what would the freezing point and boiling point of that solution assuming Kf of water is 1.86 degree celsius/m and Kb is .0512 degree celsius/m chemisty - ...
February 8, 2011 by shaknocka lewis

Chemistry
A dilute electrolyte solution is prepared by dissoving iron (III) chloride in water. It is found to have a freezing point of -2.10 degrees C. Calculate the molality of the solution.
October 18, 2010 by Gracyn

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
The normal freezing point of cyclohexane is 6.55 C. When 0.458 g of benzophenone is dissolved in 15.0 g of cyclohexane, the freezing point is found to be 3.19 C. What is the experimental molar mass of benzophenone? (Kf cyclohexane = 20.0 C m^-1). A) 182 B) 866 C) 397 D) 191 (...
November 9, 2012 by Ania

chemistry
I'm starting to learn about colligative properties and i want to know if there are different equations for boiling point elevation and freezing point depression? In the book they give me the equation: (delta)Tb= Kb times molality. But my teacher gave us: delta Tb = Kb times # ...
June 1, 2010 by jenny

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
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
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
A water solution containing an unknown quantity of an unknown nonelectrolyte solute has a freezing point of -0.21 Celsius. What is the molality of the solution? Kf=-1.86C/m
May 12, 2011 by Anonymous

Chemistry
I'm not sure if i did this problem right or not. I keep reading through my book, and i think i followed the equations right, but i'm not confident with my answers. The problem: 5.0 g of glucose,C6H12O6, is disolved in 500.0 g of acetic acid. What is the new freezing point and ...
October 22, 2010 by Angelina

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
Hey guys I did a lab and I have to answer the questions relating to the lab. I did question can someone please check if these are accurate 1. Calculation to Determine the molecular weight of unknown substance Mass of unknown used: 2.0 g Mass of water used: 50.0 g (0.05kg) Kf...
May 27, 2009 by Saira

chemistry
A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have a freezing point of -3.260C. The density of ...
April 25, 2013 by lucy

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
What is the molality of an aqueous solution of sucrose that freezes at -3.00 C? The freezing point lowering constant for water is -1.86 C/molal. 0.62 molal 1.62 molal 2.37 molal 5.58 molal
June 11, 2010 by amanda

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
If you dissolve 29.25 g of sodium chloride in 250 g of H2O. What would be the freezing point? Kfp- -1.86 degrees C/molal I know the formula is K times molality. I am taking -1.86(2.00) and getting -3.72 degrees Celsius, when the answer is -7.44 degrees. What am I doing wrong?
September 19, 2011 by Hannah

AP Chemistry
1. The heat of solution of salta may either be endothermic or exothermic. What factors determine this? 2. As a solution freezes, why does the freezing temperature continue to decrease? 3. When the concentration of very dilute aqueous solutions are calculated, why are the ...
February 4, 2007 by anonymous

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 - 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

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
If a solution has a lot of particles, is it going to have a low or high boiling point? For instance, would NaCl have a higher or lower boiling point than C12H22O11, based on the amount of particles it has (NaCl has more than C12H22O11)? Are you thinking of solutions with ...
April 19, 2007 by Grace

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
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
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
A solution made from .650g of an unknown compound in 27.8 g of diphenyl gave a freezing-point depression of 1.56 degrees C. Calculate the molality of the solution. (Kf for diphenyl is 8 degrees C/m)
October 18, 2010 by Kolby

Chemistry
The freezing point depression of a 0.100 molality solution of NaCl(aq) solution is 0.34 deg C. Calculate the % dissociation of NaCl(aq) (Kf for water = 1.86 deg Cm^-1)
August 30, 2009 by AJ

Chemistry: molality and freezing point?
What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23.3C? Assume the density for water is exactly 1g/mL. m = moles solute / kg solvent Help please?
January 27, 2009 by Agatha

Chemistry
The molar mass of a non-dissociated, non-volatile compound is to be determined by dissolving 5.00 g of the compound into 50.0 g of benzene. The freezing point of benzene was lowered by 2.5 degrees C. The freezing point depression constant (Kf) for benzene is 5.0 degree C/molal...
January 31, 2007 by Jason

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
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

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... 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
How would I go about doing this question, can someone explain it step by step please, my answer I keep getting is 1.17m CaCl2, but the answer is 1.35m CaCl2? A 1.30M solution of CaCl2 in water has a density of 1.1g/mL/ What is the MOLALITY? Also, when for questions with ...
June 16, 2009 by DrFunk

Chemistry
An aqueous salt solution has a freezing point of -.5 degrees Celsius and causes neither swelling or shriveling of cells. The kf of water is 1.86 K kg/mol. What is the osmotic pressure that is exerted on cells when placed in pure water? (ignore differences between molarity and ...
February 15, 2014 by Anonymous

chemistry
Something that will lower the freezing point of water to -3.7 degrees Celsius if one mole were placed in 1000 grams of water? To solve this I know I have to use the equation Tf= IKfm, Tf= 3.7, but how I go about the problem there if I don't know Kf or the the mole of solute (...
May 27, 2014 by A

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
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
A 1.00% by mass MgSO4(aq) solution has a freezing point of -0.192C. (a) Estimate the van't Hoff i factor from the data. (b) Determine the total molality of all solute species. (c) Calculate the percentage dissociation of MgSO4 in this solution. Can anyone help me with this at...
December 10, 2010 by Daiyo

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

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

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
Which solution has the lower freezing point? 90.0 g CH3OH in 100. g H2O 180.0 g CH3CH2OH in 200. g H2O I have worked this problem for someone within the last 3-4 days. delta T = kf m kf is not needed for this problem. change 90 g CH3OH and 180 g CH3CH2OH to mols. Change 100 ...
January 24, 2007 by Kelly

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
this is a really long question. i don't understand how to answer it. help please. A 10.0% aquueous solution of sulfuric acid has a density of 1.0661 g/mL at 20 degrees celsius. A. how many grams of H2SO4 are found in 50.0 g of this solution? B. how many grams of water are ...
April 7, 2013 by Nicole

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
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 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
A) We have an experiment , using the solution of KNO3 , measured freezing point of solution is -1.15 degree , and using a sample of pure water the thermometer read o.25 degree as freezing point of the sample , calculate the molal concentration of KNO3 assume that the ...
July 4, 2014 by MAD

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