# Calculate the freezing point of a solution of 2.50 g of Al(NO3)3 in 13.40 g of water. (ans in oC and assume no ion pairing occurs.)

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Chemistry
Calculate the molarity of Fe(NO3)3 in Solution A. Solution A: Mass of Fe(NO3)3 solid: 1.21g & Vol of Solution: 100mL In a previous ? Using the mass I weighed 404.0g/mol to calculate moles of Fe(NO3)3 in solid hydrate----I got 0.00300 mol Fe(NO3)3)

Chemistry

chemistry
Calculate the freezing point of 1molar aqueous solution (density =1.04g) of kcl (kf for water =1.86)K=39,cl=35.5

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
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?

chem
an aq. solution(NaCl) made by using 133g diluted to a total solution volume of 1 L.Calculate the molarity, molality & mass % of the solution(density of solution = 1.08g/mL) [ans: M=1.92M, m=2.0m, 10.4 %] i need the calculation work bcus my ans is contradict from the real ans...

college chemistry
A solid consists of mixture of NaNO3 and Mg(NO3)2. When 6.50 g of this solid is dissolved in 50.0 g of water, the freezing point is lowered by 5.40⁰C. What is the composition of the solid (in mass percent)? Assume ideal behavior but watch out for the van’t Hoff factor.

chemistry
Consider a 0.70 M solution of Al(NO3)3 in water. What is the nitrate ion concentration in this solution, in units of moles/L?

Chemistry
Consider a 0.70 M solution of Al(NO3)3 in water. What is the nitrate ion concentration in this solution, in units of moles/L?

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
which property of a distilled water solution will not be affected by adding 50 mL of CH3OH to 100.mL of the water solution at 25? conductivity mass freezing point boiling point please help

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?

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?

Chemistry
Solid Na2SO4 is added to a solution which is 0.020 M in Pb(NO3)2 and 0.045 M in AgNO3. Assume the volume remains constant. Ksp = 2.0 10-8 for PbSO4 and Ksp = 1.2 10-5 for Ag2SO4. What is the concentration of the first ion precipitated when the second ion starts to precipitate?

chem
(a) When a 4.75-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (see figure), the temperature drops from 23.0‹C to 16.6‹C. Calculate ƒ¢H (in kJ/mol NH4NO3) for the solution process NH4NO3(s) ¨ NH4+(aq) + NO3−(aq). ...

Chemistry
A solution is prepared by placing 72.8 g of calcium chloride in 120 g of water at 22C. The vapor pressure of water at 22C is 2.6 kPa. a)What is the boiling point of the solution? b)What is the freezing point of the solution?

Chemistry
Calculate the freezing point depression of an aqueous solution prepared by mixing 22.0 g C6H12O6, with 600 ml of water

Physics
The freezing point depression of a .100 m solution of NaCl solution is .34C. Calculate the percent dissociation of NaCl.( Kf for water=1.86) Please help

chemistry
calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of water (MgBr2=184 g, Kf for water =1.80 K kg mol-1)

Chemistry
A solution was made by dissolving 62.07 grams of a compound in 500g of water. The compound was not ionic. The freezing point of the solution was measured and found to be -1.86 degrees celsius. Using the Kf value in your textbook, the molar mass of this conpound can be ...

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
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
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
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.

Chemistry
Calculate the new freezing point and the new boiling point of an aqueous solution that contains 40.5 g of Calcium Nitrate dissolved in 225 grams of water.

Chemistry
Pb(NO3)2(aq) 2 x 10-3 M Na2SO4(aq) 2 x 10-3 M Pb(NO3)2(aq) + NaSO4(aq) → PbSO4(s)+ 2NaNO3(aq) a) What are the concentrations of each ion within this solution? b) If 1L of each solution is mixed; will a precipitate form? why?

Chemistry II
A solution is prepared by placing 72.8 g of magnesium chloride in 120 g of water at 22oC. a)What is the boiling point of the solution? b)What is the freezing point of the solution?

Chemistry
Calculate the volume of 2.45 M NaI that would be needed to precipitate all of the Hg+2 ion from 185 mL of a 2.44 M Hg(NO3)2. AND Calculate the molarity of an acetic acid solution if 47.81 mL of the solution is needed to neutralize 147 mL of 1.32 M sodium hydroxide.

general chemisty
Calculate the freezing point of a solution of 20.0 g methyl salicylate, C7H6O2, dissolved in 800 g of benzene, C6H6. Kf for benzene is 5.10°C /m and the freezing point is 5.50°C for benzene. A) -1.05°C B) 1.05°C C) 4.45°C D) 6.54°C

chemistry
A 115 mL sample of a 10.0 M ethylene glycol (C2H6O2) solution is diluted to 1.30 L. What is the freezing point of the final solution? (Assume a density of 1.06 g/mL for the final solution.) What is the boiling point of the final solution? How would I go about setting this up? ...

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
Can someone check my answer and let me know me if the are right or wrong. If I wrong can you give me the right answer plz. 1. What is the maximum amount of KCl that can dissolve in 600 g of water? (The solubility of KCl is 34 g/100 g H₂O at 20°C.) * 34 g 204 g 56 g******* ...

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.

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
Please show work. 2Al(s) + 2NaOH(aq) + 6H2O(l) ---> 2NaAl(OH)4(aq) + 3H2(g) What mass of hydrogen gas would be formed from a reaction of 2.48 g Al and 4.76 g NaOH in water? Pb(NO3)2(s) + 2NaI(aq) ----> 2PbI2(s) +2NaNo3(aq) (a) If the solution contains 7.00 g NaI, what ...

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
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
In comparing the phase diagram for water with that of a solution of sugar in water, all of the following decrease except a) the vapor pressure b) the boiling point c) the freezing point d) the triple point

chemistry
A 0.750 g sample of an unknown substance is dissolved in 20.0 g of benzene, C6H6. The freezing point of the solution is 4.53 oC. Calculate the molar mass of the substance. The normal freezing point for benzene is 5.53 oC and Kf is 5.12 oC/m.

chemistry
A 0.750 g sample of an unknown substance is dissolved in 20.0 g of benzene, C6H6. The freezing point of the solution is 4.53 oC. Calculate the molar mass of the substance. The normal freezing point for benzene is 5.53 oC and Kf is 5.12 oC/m.

Chemistry
Solid Na2SO4 is added to a solution which is 0.012 M in Pb(NO3)2 and 0.048 M in AgNO3. Assume the volume remains constant. Ksp = 2.0 10-8 for PbSO4 and Ksp = 1.2 10-5 for Ag2SO4. (a) Which compound precipitates first? (b) What is the concentration of the first ion precipitated...

Chemisrty
the freezing point of water is -1.86 degree Cm, if 5.00 g Na2SO4 is desolve at 45.0g H2o the freezing point is changed by -3.82 degree C. Calculate the Van't Hoff Factor for Na2SO4

chemistry
the freezing point of water is -1.86 degree Cm, if 5.00 g Na2SO4 is desolve at 45.0g H2o the freezing point is changed by -3.82 degree C. Calculate the Van't Hoff Factor for Na2SO4

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 ...

Chemistry
I am confused about why this is the answer to a practice problem I was given. (answer is c). Could someone explain why/why not for each answer? 2) Solution A is made from 1 L of water and 0.1 moles of Na(CH3COO), and Solution B is made from 1 L of water and 0.1 moles of Na2(...

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
A solution was prepared by dissolving 0.817g of sulfur S8, in 100.0g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution

Chemistry
A solution is made by dissolving 0.698 mol of nonelectrolyte solute in 777 g of benzene. Calculate the freezing point and boiling point of the solution

chemistry
The formate ion, (CHO2-), is related to the acetate ion and forms ionic salts with many metal ions. Assume that 9.7416 g of M(CHO2)2 (where M represents the atomic symbol for a particular metal) are dissolved in water. When a solution of 0.200 M sodium sulfate is added, a ...

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
An antifreeze solution is prepared containing 40.0 g of ethylene glycol (molar mass = 62.0 g/mol) in 60.0 g of water. Calculate the freezing point of this solutions A.-20.1°C B.0.518°C C.20.1°C D.120.1°C

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 ...

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

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

Chemistry
Vitamin K is involved in normal blood clotting. When 2.32 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 7.78 °C. The freezing point and Kf constant for camphor can be found here. Calculate the molar mass of vitamin K.

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 ...

1) In comparing the phase diagram for water with that of a solution of sugar in water, all of the following decrease except a) the vapor pressure b) the boiling point c) the freezing point d) the triple point I chose the boiling point as the answer. Is this correct? Thank you.

chemistry
calculate the freezing point of an aqueous solution of 15.5 grams of glucose dissolved in 150 grams of water

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.

Chemistry II
An unknown solute (a nonelectrolyte) was obtained and 5.37 g was weighed out. After dissolving the solute in water, the mass of the solution was 26.58 g. From the experimental results, the freezing point depression was found to be 3.6oC. If the freezing point depression ...

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...

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 ...

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 ...

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
Calculate the freezing point of a solution contaning 5.0 grams of KCl and 550.0 grams of water. answer is -0.45 C but i don't know how to get here

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
5.00kg glycol, C2H4(OH)2, [this is anti-freeze!] is added to your radiator. If your radiator contains 12.0kg of water, what would be the freezing point of the water-antifreeze mixture? The molal freezing point depression constant for water is 1.86 degrees celsius x kg/mole.

Chem
An antifreeze solution is prepared containing 40.0 g of ethylene glycol (molar mass = 62.0 g/mol) in 60.0 g of water. Calculate the freezing point of this solution. Which calculation is it? A. 120.1⁰C B. -20.1⁰C C. 0.518 ⁰C D. 20.1⁰C

Is anyone here a chemistry genuis?
The formate ion, (CHO2-), is related to the acetate ion and forms ionic salts with many metal ions. Assume that 9.7416 g of M(CHO2)2 (where M represents the atomic symbol for a particular metal) are dissolved in water. When a solution of 0.200 M sodium sulfate is added, a ...

Chemistry
A solution is made by dissolving 0.526 mol of nonelectrolyte solute in 831 g of benzene. Calculate the freezing point and boiling point of the solution. Constants may be found here.

ecc
A solution was prepared by dissolving 0.834 g of sulfur, S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (Use the table from the textbook.)

chemistry
A solution was prepared by dissolving 0.834 g of sulfur, S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (Use the table from the textbook.)

chemistry
A solution was prepared by dissolving 0.834 g of sulfur, S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (Use the table from the textbook.)

chemistry
A solution was prepared by dissolving 0.834 g of sulfur, S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (Use the table from the textbook.)

Chemistry
Please please help me on this equation I'm stuck and your steps are confusing. Calculate the concentrations of each ion remaining in solution after precipitation is complete. (Enter a 0 if none of the ion remains.) Cl ‾ Ca2+ I have Ag+=0 and NO3^-3= 0.13 but I can't seem...

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
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
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
1. What is the vapor pressure at 25°C of a solution of 1.20g of nephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23°C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of the solution. 2. A ...

chemistry
Analysis of a compound gave 39.50% C, 2.20% H, and 58.30% Cl. 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 ...

Chemistry
1) What is the vapor pressure at 25°C of a solution of 1.20g ofnephtalene C10H8 in 25.6g of benzone C6H6? The vapor pressure of pure benzene at 23°C is 86.0mmHg the vapor pressure of naphthalene can be neglected. Calculate the vapor pressure lowering of the solution. 2)A ...

physics

chemistry
A solution. Of glucose was prepared by dissolving certain amount in 100 grams of water ,the depression in freezing point is. 0.041kelvin if depression of water is 1.86 kelvin*kg/mol.calculate the weight of glucose dissolved .

Chemistry
Calculate the freezing point and boiling point of each of the following solutions A. 2.75m NaOH in water B. 0.586m of water in ethanol c. 1.26m of naphthalene (C10H8) in benzene

chemistry
Which of these ions may be precipitated as sulfides? Assume neutral aqueous solution, pH=7. Silver (I) ion Sodium ion Calcium ion Lead (II) ion Manganese (II) ion Ammonium ion I think the silver I ion, lead II ion, and manganese ion may be precipitated as sulfides, but I'm not...

Chem
Which of these ions may be precipitated as sulfides? Assume neutral aqueous solution, pH=7. Silver (I) ion Sodium ion Calcium ion Lead (II) ion Manganese (II) ion Ammonium ion I think the silver I ion, lead II ion, and manganese ion may be precipitated as sulfides, but I'm not...

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 ...

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
An aqueous salt solution is formed by adding 11.67 g sodium sulfate (solute) to water (solvent). What mass (in g) of water is used if the freezing point of the solution is -12.9 Farenheit. Kf H2O = 1.86 Celsius/m

chemistry
Solid Na2SO4 is added to a solution which is 0.014 M in Pb(NO3)2 and 0.041 M in AgNO3. Assume the volume remains constant. Ksp = 2.0 10-8 for PbSO4 and Ksp = 1.2 10-5 for Ag2SO4. (a) Which compound precipitates first? 1 PbSO4 (b) What is the concentration of the first ion ...

Chemistry
From your Dilution Data in the procedure 3 and 4, calculate the initial concentration of Fe3+ (aq) ion for tubes 2-5. 1. Add 5.00ml of 1.00 x10^-3 M KSCN to all tubes. 2. To test tube 1 add 5 ml of 0.200M Fe(NO3)3. 3. Measure 8.00ml of 0.200M Fe(NO3)3 into 25.0ml cylinder. ...

Chemistry
1) Which ion(s) below would undergo hydrolysis in water? A) Cl- B) K+ C) NH4+ D) NO3- E) Two of the above My guess is C, but I'm not too sure about this one. 2) Calculate the [OH-] present in solution labeled 1.73 M methylamine. CH3NH3 + H2O --> CH3NH3+ + OH-. I get 2.76 x ...

CHEMISTRY
Wondering If I did this correctly so far 50.0 ml of a 0.0500 M solution of lead (II) nitrate is mixed with 40.0 ml of a 0.200 M solution of sodium iodate at 25°C. Calculate the Pb2+ and IO3- concentrations when the mixture comes to equilibrium. At this temperature the Ksp for...

chemistry
Calculate the freezing point of water at a depth of 10.0 cm below the surface of the water. The density of the water is 0.9998 g/cm3.

physics
Calculate the freezing point of water at a depth of 10.0 cm below the surface of the water. The density of the water is 0.9998 g/cm3.

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