Homework Answers
(Kf) The cryoscopic constant, which is dependent on the properties of the solvent, not the solute. (Note: When conducting experiments, a higher Kf value makes it easier to observe larger drops in the freezing point. For water, (Kf= 1.853 K·kg/mol.),, therefore correct true statement is - "Kf should be large so that the temperature change will be large enough to measure"
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QUESTION 25 The molar mass of a compound can be determined by the freezing point depression...
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a...
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
Post-Lab Material Experiment 19 Data and Calculations: Molar Mass Determination by Depression of the Freezing Point...
Post-Lab Material Experiment 19 Data and Calculations: Molar Mass Determination by Depression of the Freezing Point 0.3 Name Section A. Measured Freezing Point of Pure Water B. Finding the Freezing Point of a Solution of Liquid Unknown Target mass of solute (Calculated based on the parameters in the instructions) Unknown # Liquid 3.5 Actual mass of solute used Trial Freezing point of solution (observed) -3.0 Mass of solution 116.6 Trial II Freezing point of solution -3.3 Mass of solution 101.3....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf...
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute? 1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the...
A Molar Mass from freezing-point Depression. 1. Provide definitions for the following terms: a. Solution-cv b....
A Molar Mass from freezing-point Depression. 1. Provide definitions for the following terms: a. Solution-cv b. Solute c. Solvent d. Colligative property e. Freezing-point depression a. What is the objective of this experiment? b. How will that objective be achieved? 3. A 0.2436-g sample of an unknown substances was dissolved in 20.0 mL of cyclohexane. The density of cyclohexane is 0.779 g/mL. The freezing-point depression was 2.5*C. Calculate the molar mass of the unknown substance. 4. What safety rules must...
Determination of Molar Mass by freezing Point depression Not sure how to answer these two questions...
Determination of Molar Mass by freezing Point depression
Not sure how to answer these two questions
Calcium chloride, CaCI_2 is commonly used as road salt. If one mole of CaCI_2 is dissolved in 1 kg v of water, would the freezing point of the solution be greater than, less than, or the same as a solution prepared by dissolving one mole of table sugar (sucrose, C_12H_22O_11) in 1 kg of water? Explain your answer. A student followed our lab procedure...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
t-Butanol has a freezing point of 25.82 oC and a freezing point depression constant of 8.37...
t-Butanol has a freezing point of 25.82 oC and a freezing point depression constant of 8.37 oC/m. What will be the freezing point (in oC) of a solution that is 1.64 molal solute dissolved in t-butanol?
Molar mass determination by depression of freezing point lab I'm stuck on calculating the moles of...
Molar mass determination by depression of freezing point lab I'm
stuck on calculating the moles of solute.. How do I calculate it?
Also can u please check if I've done everything else correctly..
The data I collected: Measured freezing point of pure water: 0.0
degrees Celsius Actual mass of solute used: 10.12g Freezing point
of solution (observed): -3.4 Celsius Mass of solution: 84.7g
Freezing point of a Solution of liqud unknown Freezing point depression: Trial #1. 0.0℃ (-3.4°C)= 3.4℃ Molality...
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
Post-Lab Material Experiment 19 Data and Calculations: Molar Mass Determination by Depression of the Freezing Point 0.3 Name Section A. Measured Freezing Point of Pure Water B. Finding the Freezing Point of a Solution of Liquid Unknown Target mass of solute (Calculated based on the parameters in the instructions) Unknown # Liquid 3.5 Actual mass of solute used Trial Freezing point of solution (observed) -3.0 Mass of solution 116.6 Trial II Freezing point of solution -3.3 Mass of solution 101.3....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
A Molar Mass from freezing-point Depression. 1. Provide definitions for the following terms: a. Solution-cv b. Solute c. Solvent d. Colligative property e. Freezing-point depression a. What is the objective of this experiment? b. How will that objective be achieved? 3. A 0.2436-g sample of an unknown substances was dissolved in 20.0 mL of cyclohexane. The density of cyclohexane is 0.779 g/mL. The freezing-point depression was 2.5*C. Calculate the molar mass of the unknown substance. 4. What safety rules must...
Determination of Molar Mass by freezing Point depression
Not sure how to answer these two questions
Calcium chloride, CaCI_2 is commonly used as road salt. If one mole of CaCI_2 is dissolved in 1 kg v of water, would the freezing point of the solution be greater than, less than, or the same as a solution prepared by dissolving one mole of table sugar (sucrose, C_12H_22O_11) in 1 kg of water? Explain your answer. A student followed our lab procedure...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
Molar mass determination by depression of freezing point lab I'm
stuck on calculating the moles of solute.. How do I calculate it?
Also can u please check if I've done everything else correctly..
The data I collected: Measured freezing point of pure water: 0.0
degrees Celsius Actual mass of solute used: 10.12g Freezing point
of solution (observed): -3.4 Celsius Mass of solution: 84.7g
Freezing point of a Solution of liqud unknown Freezing point depression: Trial #1. 0.0℃ (-3.4°C)= 3.4℃ Molality...
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