
(A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g instead of 8.003 g. The calculated molar mass of the unknown acid will be ___________ than the true value,

A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g instead of 8.003 g. The calculated molar mass of the unknown acid will be ___________ than the true value,

A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300g instead of8.003g. The calculated molar mass of the unknown acid will be GREATER/LESS than true value b/c mass of

1) The color of bromocresol green indicator is??? when pH < 4, green when pH 4 5.3 and ???? in pH > 5.3. 2)(A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g

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


The procedure described in this experiment was used to determine the molar mass of unknown liquid (nonelectrolyte). 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.

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

Three students are asked to determine the mass of a coon. They each measure different values for the mass of the coin using a balance. Student A recorded a mass of 63.08g, student B recorded a mass of 63.022g and student C recorded a mass of 63.0328g. If

Experiment questions: Experiment 1 results mass of beaker:116.944 g mass of dodecanoic:11.629 g hot water: 175 C warm water: 10 C Average Fressing pt of Dodecanoic = 42.7 Experiment 2 results: Unknown C solution mass: 2.091g Hot water: 175C warm water: 10C

The freezingpoint depression for a given aqueous solution is 0.32 K. The freezingpoint depression constant for water is 1.86 K/m. Calculate the molality of solutes in the solution. The equation for freezing point depression is ΔTf = Kf · m, where ΔTf

An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% Carbon and 5.30% H. The molar mass is determined by measuring the freezingpoint depression of an aqueous solution. A freezing

1) For a freezing point depression experiment we had to create an ice bath and add salt to the ice. I have to answer the question, why was salting the ice necessary in order to complete the experiment and how does this apply to the principles/concepts

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

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

Freezingpoint 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


Freezingpoint 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

if the freezing point of the solution is recorded 0.2 degrees C lower than the actual freezing point, will the molar mass determination for the unknown solid be too high or too low?

Derive a formula for the molar mass of the solute in terms of the freezing point depression, deltaT, the freezingpoint constant, Kf, and the masses of solvent, msolvent, and solute, msolute, used in an experiment like this one. SHow your work and include

A student determines the freezing point of a solution of 1.96g of naphthalene in 25.64g of paradichlorobenzene(PDB). The following temperaturetime 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

A student determines the freezing point of a solution of 1.96g of naphthalene in 25.64g of paradichlorobenzene(PDB). The following temperaturetime 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

Find the molecular mass of a solute by freezing point depression. Solvent: paradichlorobenzene Freezing point of pure solvent: 53.02C Mass of unknown substance: 2.04g Freezingpointdepressin constant:7.1c/m Mass of paradichlo...: 24.80g Freexing point

When 0.500 g of an unknown compound was dissolved in 15.0 g benzene, the freezing point depression was determined to be 0320C. The molar mass of the unknown compound is ?? g/mol. (The freezing point depression constant for benzene is 5.12C kgmol. I really

When 0.500 g of an unknown compound was dissolved in 15.0 g benzene, the freezing point depression was determined to be 0320C . The molar mass of the unknown compound is ? g/mol. (The freezing point depression constant for benzene is 512C kgmol .

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).

When 0.500 g of an unknown compound was dissolved in 15.0 g benzene, the freezing point depression was determined to be 0.320 C. The molar mass of the unknown compound is ____ (The freezing point depression constant for benzene is 5.12 C kg/mol. )


a solution is prepared by mixing 2.17g of an unknown nonelectrolyte 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

The following errors occurred when the experiment was carried out. How would each affect the calculated molar mass of the solute(too high, too low, no effect)? Explain. a. The thermometer used actually read 1.4 centigrade too high. b. some of the solvent

a student determines the molar mass of methanol by the method used in this experiment. she found that the equilibrium temperature of a mixture of ice and pure water was .4 degrees Celsius on her thermometer. when she added 10g of her sample to the mixture,

a. Calculate the expected freezingpoint depression of a 0.200 m KNO3 solution. b. Will the value you calculated match the actual freezingpoint depression for this solution? Why or why not? a). 0.372 degrees Celsius b). Possibly because not all of the

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

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.

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

What is the freezingpoint depression of water in a solution of 100g of sucrose, C12 H22 O11, and 500g of water? (Molar freezing point depression constant for water is 1.86°C/m.)

3.92g of a nondissociating compound are dissolved in 400.g of liquid benzene. The freezing point of the solution is 5.19 degrees celsius. Calculate the molar mass of the compound. (The freezing point of the pure benzene is 5.50 degrees celsius and its

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 0.161 g of an unknown nonelectrolyte solute and 5.818 g of cyclohexane was 3.98°C. What is the molar


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 0.161 g of an unknown nonelectrolyte solute and 5.818 g of cyclohexane was 3.98°C. What is the molar

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 =

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.

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.

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.

Molecular Mass by Freezing point Depression (Preliminary Lab) The following errors occurred when the above experiment was carried out. How would each affect the calculated molecular mass of the solute (too high,too low, no effect)? Explain your answer. (a)

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

you are conducting a freezingpoint 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

I had to perform an experiment for the freezing point depression in which we had to determine the freezing points of water as a pure solvent, sodium chloride, sucrose, and ethylene glycol. We had to work with a partner so I completed the experiment for

Find the molecular mass of a solute by freezing point depression.


Thyroxine, an important hormone that controls the rate of metabolism in the body can be isolated from the thyroid gland. If 0.455 g of thyroxine is dissolved in 10.0 g of benzene, the freezing point of the solution could be measured as 5.144°C. Pure

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

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

After performing a freezing point depression experiment I had to find the molecular weight of glycol. Now I have to answer the question what value did I assume "i" to equal and why did I make this assumption. My teacher told us the value of i to use for

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,

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.

The freezing point of a salt and water mixture is 0.58 C. The freezing point of an unknown ionic solution (0.100 m) is 1.04 C. 1. Determine the freezing point depression for the ionic solution. 2. How do you determine the van't Hoff factor for the ionic

The molar mass of a nondissociated, nonvolatile 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

So I did a titration experiment using 0.01 M potassium permanganate. In an erlenmeyer flask I placed a mass sample of FeSO4 with enough DI water to have a total volume of 2025ml. I recorded the volume of MnO4 it took for the solution to change color

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


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

A solution is made by dissolving 21.5 grams of glucose (C6H12O6) in 255 grams of water. What is the freezingpoint depression of the solvent if the freezing point constant is 1.86 °C/m?

A solution is made by dissolving 10.20 grams of glucose (C6H12O6) in 355 grams of water. What is the freezingpoint depression of the solvent if the freezing point constant is 1.86 °C/m?

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?

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

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.

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

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!

A solution is made by dissolving 10.20 grams of glucose (C6H12O6) in 355 grams of water. What is the freezingpoint depression of the solvent if the freezing point constant is 1.86 °C/m? Show all of the work needed to solve this problem.

A solution is made by dissolving 15.5 grams of glucose (C6H12O6) in 245 grams of water. What is the freezingpoint depression of the solvent if the freezing point constant is 1.86 °C/m? Show all of the work needed to solve this problem.


A solution is made by dissolving 15.5 grams of glucose (C6H12O6) in 245 grams of water. What is the freezingpoint depression of the solvent if the freezing point constant is 1.86 °C/m? Show all of the work needed to solve this problem.

A solution contains 20g of C^6H^12O^6 in 250g of water. What is the freezingpoint depression of the solvent? What is the Freezing point of the solvent?

Camphor, C16H16O which has a freezing point of 174°C, has a freezing point depression constant of 40.0°C/m. Explain the usefulness and the limitation of camphor as a solvent for determination of molecular weights. For whose kind(s) of solute would

had to perform an experiment for the freezing point depression in which we had to determine the frezzing points of water as a pure solvent, sodium chloride, sucrose, and ethylene glycol. We had to work with a partner so I completed the experiment for

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 nonelectrolyte and dissolving it in 90.50 g of glacial acetic acid. The

I had to perform an experiment for the freezing point depression in which we had to determine the frezzing points of water as a pure solvent, sodium chloride, sucrose, and ethylene glycol. We had to work with a partner so I completed the experiment for

In a certain experiment, the rate constant, k, was measured as a function of the temperature, T. Two data points were as follows: (A) 25°C, 1.1 x 10–5 min–1, and (B) 225°C, 2.4 x 102 min–1. The student who performed the experiment then plotted

When 0.5mol of a certain ionic substance is dissolved in 1.0kg of water, the freezing point of the resulting solution is 3.72 ∘ C .(Freezing point depression of water is 1.86 kgwater molsoluteparticles ). How many ions does the substance give when it

The freezing point of an aqueous solution that contains a nonelectrolyte is 9.0 degrees celcious. A. What is the freezingpoint depression of the solution? B. What is the molal concentration of the solution?

When 18 g of ethylene glycol C2H6O2 is dissolved in 150 g of pure water, the freezing point of the solution is ___ (degrees)C. ( The freezing point depression constant for water is 1.86(dgrees)C kg/mol. I know the formulas I just need to see it done step


A student wants to run an experiment to determine how the distribution of mass (location of mass) affects an object`s rotational velocity. For this experiment the student picks 3 rings. One is a wood ring (like a hulahoop) with all of its mass at the

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

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

A compound containing only boron, nitrogen, and hydrogen was found to be 40.3% B, 5202% N, 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 degree celsius. if the freezing point depression

What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 in 115 g of water? The molal freezing point depression constant for water is 1.86°C/m. (Note that when Ca(NO3)2 dissolves in water Ca2+ and NO32 ions are produced).

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

10.0 g sample of pdichlorobenzene, a component of mothballs, is dissolved in 80.0 g of benzene, C6H6. The freezingpoint 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.

A student mistakenly used an ethanol solution containing an unknown ionic compound in part C of the experiment. How would this affect the Van't Hoff factor determined experimentally? Justify your answer with an explanation.

What are the differences in measuring the molar mass using freezing point depression between studying ionic solids and molecular solids?

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,


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,

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

Using data from this table of molal boilingpointelevation and freezingpointdepression constants, calculate the freezing and boiling points of each of the following solutions. a)0.39 m glucose in ethanol (b) 22.8 g of decane, C10H22, in 53.9 g CHCl3 (c)

When 3.78 g of nonvolatile solute is dissolved in 300.0 g of water, the freezing point depression is 0.646 o C. Calculate the molar mass of the solute. The cryoscopic constant of water is 1.86 K kg mol 1. When 3.78 g of nonvolatile solute is dissolved in

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

1) The molecular mass of a substance was determined by the freezing point depression technique. The minimum data required for the determination are a. ƒ´Tf and Kf only. b. ƒ´Tf , Kf and mass of solute. c. ƒ´Tf , Kf , mass of solute and mass of

How would the calculation percent of oxalate of the unknown affected when weighting out the unknown solid the actual mass is .758 grams however the mass is mistakenly recorded as .785 grams

Question: Two substances, A and B, have the same melting point. how can you determine if they are the same without using any form of spectroscopy? Explain in detail. My answer: Perform a mixture melting point. In this procedure, pulverize and mix A and B

I had to perform an experiment for the freezing point depression in which we had to determine the frezzing points of water as a pure solvent, sodium chloride, sucrose, and ethylene glycol. We had to work with a partner so I completed the experiment for

A Biology student wants to know if Mountain Dew will make plants grow faster than water. As a Chemistry student, you have agreed to assist in the planning of the experiment to make sure the student designs a valid experiment. 1) What is the experimental


if calculating molecular weight of unknown by freezing point depression...All of the unknowns in the activity were nonpolar organic molecules with molecular weight= 100250 g/mol and using around 1g of the unknown. Provide an example of a solvent that

A researcher conducted an experiment on the effects of a new “drug” on depression. The researcher had a control group that received nothing, a placebo group and an experimental group that received the “drug”. A depression inventory that provided a

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.

Assuming equal concentrations, rank these aqueous solutions by their freezing point: LiSO4, Li3PO4, SnCl4, NH4Br. (from highest freezing point to lowest freezing poinT) Thanks.

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