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Chemistry: molality and freezing point?

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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, ...

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...

chem
Assuming complete dissociation, what is the molality of an aqueous solution of KBr whose freezing point is -2.95 ∘C? The molal freezing-point-depression constant of water is 1.86 (∘C⋅kg)/mol. Molality = m

Chemistry
The equation for lowering the freezing point of a solvent is given in your manual. Given that the freezing point for the pure solvent is 79.4 °C , the molality is 0.1 m , and the freezing point depression constant is 6.9 °C/m , determine the freezing temperature for the ...

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...

AP Chemistry
Why would .25 molality of CaCl2 have a larger effect on the freezing point of water than .25 molality of NaCl?

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...

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...

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 ...

chemistry
1. Find the molality of the solution prepared by dissolving 0.238g toluene, C7H8, in 15.8g cyclohexane 2. A pure sample of the solvent phenol has a freezing point of 40.85 degrees C. A 0.414 molal solution of isopropyl alcohol was observed to have a freezing point of 38.02 ...

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 # ...

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 ...

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).

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 ...

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 ...

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? ...

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

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)?

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...

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 ...

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, ...

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 ...

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

chemistry
lowest+freezing+point+of+Kbr+AlNO33+CH3COONa+NaNO2+MgCl2+of+same+molality

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.

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 ...

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...

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 ...

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...

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...

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 ...

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...

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) ...

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 ...

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

Chemistry
Benzene (C6H6) has a normal freezing point of 5.50oC and a density of 0.88 g/mL. When 1.28 g of naphthalene (C10H8) is dissolved in 125 mL of benzene, the freezing point of the solution is 5.03oC. Determine the molal freezing point constant for this solvent.

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!

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~!

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)

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)

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?

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?

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 ...

chemistry
A freezing point depression experiment was conducted using cyclohexane as the solvent. The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point of a solution containing 0.135 g of an unknown nonelectrolyte ...

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 ...

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 - ...

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 ...

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 ...

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.

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 (...

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?

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 # ...

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

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?

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

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...

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 ...

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 ...

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...

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 ...

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

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, what ...

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

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 ...

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?

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. ...

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.

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.

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 ...

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?

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.

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)

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.

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)

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?

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...

Chemistry
A student determines the freezing point of a solution of 1.96g of naphthalene in 25.64g of paradichlorobenzene(PDB). The following temperature-time reading are recorded. PDB/Napthalene Time(Min) 0 0.5 1.5 2 2.5 3 3.5 4 4.5 Temp(°C) 59.7 58.0 54.8 53.4 52.1 50.9 49.5 49.6 49.5...

Chemistry
A student determines the freezing point of a solution of 1.96g of naphthalene in 25.64g of paradichlorobenzene(PDB). The following temperature-time reading are recorded. PDB/Napthalene Time(Min) 0 0.5 1.5 2 2.5 3 3.5 4 4.5 Temp(°C) 59.7 58.0 54.8 53.4 52.1 50.9 49.5 49.6 49.5...

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 1.454°C. Calculate the molar mass of the solute. The kf of phenol is 7.27 (K·kg)/mol. What is the normal boiling point of an aqueous solution that has a freezing ...

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 ...

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.

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 ...

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 (...

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?

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?

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?

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 ...

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 ...

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?

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 1.86°C/m.

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...

Chemistry
A 1.00% by mass MgSO4(aq) solution has a freezing point of -0.192°C. (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 ...

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 ...

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 ...

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 ...

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 ...

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 ...

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.

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.

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.

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