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Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of...
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
molecular weight moles of solute kg owater insolution molality of solution change in freezing point Naci...
molecular weight
moles of solute
kg owater insolution
molality of solution
change in freezing point
Naci KCI CaCl, 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) 9 9 9 g/mole g/ mole mole mole kal kg m m -31°C 3 °C...
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...
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...
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a...
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a 0.850 M solution of CaCl2 contains 1.28 g of solute? 9. The volume of a 27.0% (by mass) solution is 162.9 mL. The density of the solution is 1.128 g/mL. What is the mass of solute in this solution? 10. Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL. What is the...
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...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute in solution1 1.5 volume of unknown solute in solution 2 1.5 freezing point of pure acetic acid 16.3 freezing point of solution 1 14.5 freezing point of solution 2 11.3 average molar mass of unknown solute Calculations for Part 1 The density of acetic acid is 1.049 g/mL and Kf(acetic acid) =3.90 °C·kg/mol The density of the unknown is 0.791 g/mL. 1.Calculate the masses...
Freezing points are lowered as a function of the number of moles of solute particles per...
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
Enter your answer in the provided box. The formula that governs the depression of freezing point...
Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: AT = i x kb x m where: AT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a nonionic solute that does not...
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 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
molecular weight
moles of solute
kg owater insolution
molality of solution
change in freezing point
Naci KCI CaCl, 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) 9 9 9 g/mole g/ mole mole mole kal kg m m -31°C 3 °C...
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...
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a 0.850 M solution of CaCl2 contains 1.28 g of solute? 9. The volume of a 27.0% (by mass) solution is 162.9 mL. The density of the solution is 1.128 g/mL. What is the mass of solute in this solution? 10. Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL. What is the...
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...
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
Enter your answer in the provided box. The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: AT = i x kb x m where: AT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a nonionic solute that does not...
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...
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