Solute Mass(g) Observed Freezing Point (Celcius) m i Theoretical Freezing Point (Celcius) NaCl 2.94g -1 CaCl2...
| Solute | Mass(g) | Observed Freezing Point (Celcius) | m | i | Theoretical Freezing Point (Celcius) |
| NaCl | 2.94g | -1 | |||
| CaCl2 * 2H20 | 7.37g | 0 | |||
| C12H22O11 | 17.14g | 0.5 |
100.0g of pure ice water freezing point 0.5 C
Final Freezing Point -3
- Your solvent mass should be the mass of the water and the mass of the ice
- You should use your observed freezing point of pure water to adjust the values for the observed freezing point of the solution, that will make comparing your observed and theoretical freezing points much easier
- Make sure you account for the water of hydration in your calculations for moles of calcium chloride; include the water in the molar mass calculation, and use the resulting molar mass to calculate the number of moles of hydrated calcium chloride
PLEASE COMPLETE THE CHART SHOWING WORK. THANK YOU!!!
Homework Answers
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Solute
Mass(g)
Observed Freezing Point (Celcius)
m
i
Theoretical Freezing Point (Celcius)
NaCl
2.94g
-1
CaCl2...
Lab 3: Determination of Molar Mass by Freezing Point Depression 1 During winter, several different "salts"...
Lab 3: Determination of Molar Mass by Freezing Point Depression 1 During winter, several different "salts" are used to melt ice sodium chloride (NaCI), a mix of sodium chloride and magnesium chloride (NaCl and MgCla calcium magnesium acetate (CaMg(CHO)). Assume you have 1 mole of each of these in 1 kg of water. Compare the freezing point depressions of these three "salts." a. b. What is the ratio of moles of "salt" to freezing point depression for each? What is...
Naci КСІ CaCl2 °C g Part B. Initial Freezing Point of Water Mass of water Mass...
Naci КСІ CaCl2 °C g Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) g/mole mole kg| m g g g/mole mole kg m g/mole mole kg m -37°C -3.7°C -55 °C °C "C/ml cl "C/m 'cl "Clm
Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of...
Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) NaCl 0°C 10.0 g 0.58 9 g/mole mole kg KCI oºch 10.0 g 0.75 g g/mole mole kg CaCl2 0°C 10.09 1.11 g g/mole mole kg m -5.6°C °c C/m -3.7°C...
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...
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....
Solute X (molecular substance) was added to a pure solvent and the freezing point depression was...
Solute X (molecular substance) was added to a pure solvent and the freezing point depression was measured to be 7.0°C. Separately, the same amount of solute Y (molecular substance) was added to the same amount of pure solvent and the freezing point depression was measured to be 10.5°C. Which solute (X or Y) has the higher molar mass. Explain your rationale. thank you
A. Freezing Point of Cyclohexane (Solvent 1. Mass of beaker, test tube (g) 2. Freezing point,...
A. Freezing Point of Cyclohexane (Solvent 1. Mass of beaker, test tube (g) 2. Freezing point, from cooling curve 3. Instructor's approval of graph 33010 B. Freezing Point of Cyclohexane plus Unknown Solute Trial 1 Parts B.1, B.3) Unknown solute no. Trial 2 (Part B.4 Trial 3 Part B.5 1. Mass of beaker, test tube, cyclohexane (g) 2. Mass of cyclohexane (g) 3. Tared mass of added solute (g) 4. Freezing point, from cooling curve CC) 5. Instructor's approval of...
i need help with the calculations from the first part of the lab Freezing Point Depression...
i need help with the calculations from the first part of the
lab
Freezing Point Depression Name Part A. Initial Freezing Point of Water 0°C 0°C 0°C Mass of water 10. 09 0.0 g 10.09 Mass of Ethylene Glycol 0.5 g 1.0 9 1 .5 9 Molecular weight of Ethylene Glycol 62.1 g/mol moles of Ethylene Glycol molem ole mole kg of water in solution kgkgl molality of solution Final Freezing Point of solution Change in Freezing Point ke value...
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g...
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
Chemistry: Molar mass determination and freezing point depression. If your unknown solute sample weighed 0.634 grams,...
Chemistry:
Molar mass determination and freezing point depression.
If your unknown solute sample weighed 0.634 grams, but some of it stuck to the test tube wall when you were pouring it in and did not dissolve in the t-butyl alcohol, what sort of error will this cause in the calculated molar mass of your unknown solute? Explain. What would be the freezing point of an aqueous solution that contains 10.3 grams of ethylene glycol [(C_2H_4(OH)_2] in 100 mL of water?
Lab 3: Determination of Molar Mass by Freezing Point Depression 1 During winter, several different "salts" are used to melt ice sodium chloride (NaCI), a mix of sodium chloride and magnesium chloride (NaCl and MgCla calcium magnesium acetate (CaMg(CHO)). Assume you have 1 mole of each of these in 1 kg of water. Compare the freezing point depressions of these three "salts." a. b. What is the ratio of moles of "salt" to freezing point depression for each? What is...
Naci КСІ CaCl2 °C g Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) g/mole mole kg| m g g g/mole mole kg m g/mole mole kg m -37°C -3.7°C -55 °C °C "C/ml cl "C/m 'cl "Clm
Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) NaCl 0°C 10.0 g 0.58 9 g/mole mole kg KCI oºch 10.0 g 0.75 g g/mole mole kg CaCl2 0°C 10.09 1.11 g g/mole mole kg m -5.6°C °c C/m -3.7°C...
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...
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....
A. Freezing Point of Cyclohexane (Solvent 1. Mass of beaker, test tube (g) 2. Freezing point, from cooling curve 3. Instructor's approval of graph 33010 B. Freezing Point of Cyclohexane plus Unknown Solute Trial 1 Parts B.1, B.3) Unknown solute no. Trial 2 (Part B.4 Trial 3 Part B.5 1. Mass of beaker, test tube, cyclohexane (g) 2. Mass of cyclohexane (g) 3. Tared mass of added solute (g) 4. Freezing point, from cooling curve CC) 5. Instructor's approval of...
i need help with the calculations from the first part of the
lab
Freezing Point Depression Name Part A. Initial Freezing Point of Water 0°C 0°C 0°C Mass of water 10. 09 0.0 g 10.09 Mass of Ethylene Glycol 0.5 g 1.0 9 1 .5 9 Molecular weight of Ethylene Glycol 62.1 g/mol moles of Ethylene Glycol molem ole mole kg of water in solution kgkgl molality of solution Final Freezing Point of solution Change in Freezing Point ke value...
Chemistry:
Molar mass determination and freezing point depression.
If your unknown solute sample weighed 0.634 grams, but some of it stuck to the test tube wall when you were pouring it in and did not dissolve in the t-butyl alcohol, what sort of error will this cause in the calculated molar mass of your unknown solute? Explain. What would be the freezing point of an aqueous solution that contains 10.3 grams of ethylene glycol [(C_2H_4(OH)_2] in 100 mL of water?
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