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4. In another experiment, 1.249 g of citric acid were added to the 16.27 g of...
How many grams of citric acid, C6H8O7 (Mm = 1925 g / mol), must be added...
How many grams of citric acid, C6H8O7 (Mm = 1925 g / mol), must be added to 50.0g of acetic acid (Tb = 118.5 C, Kb = 3.07 C / m) to prepare a solution with a boiling point of 120.3 C?
9. A solution of 1,035 g of benzoic acid in 8.525 g of lauric acid had...
9. A solution of 1,035 g of benzoic acid in 8.525 g of lauric acid had a freezing point of 39.6 C What is the molar mass of benzoic acid? The freezing point of lauric acid is 43.2 C and Kris 3.60 C.kg/mol.
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point...
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point of the solution. The molar mass of palmitic acid is 256.48 g/ mol. The molal freezing point constant , Kf for stearic acid is 4.5 degrees C/ m and pure stearic acid freezes at 69.3 degrees Celsius.
מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water...
מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water to give a solution whose freezing point is -3.8°C. The freezing point depression constant of water is 1.86 °C/m. The molar mass of glucose is 180.16 g/mol Give your answer in grams to 3 significant figures
Course Contents> ... Experiment 6 -- Colligative Properties -- Freezing Point De Due in 3 hours,...
Course Contents> ... Experiment 6 -- Colligative Properties -- Freezing Point De Due in 3 hours, 1 minute 5 homework point(s) Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent K=20.0. 0.144 g of an unknown solute is dissolved in 7.88 g of cyclohexane (C6H12). The freezing point of the solution was 3.36°C. Calculate the corresponding molar mass of the solute. 117.89 g/mol 1homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries To the...
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water...
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water to produce an antifreeze solution with a freezing point of-19.0°C? (The density of ethylene glycol is 1.11 g/cm°, and the density of water is 1.00 g/cm³. K, for water is 0.51°C•kg/mol and Kf is 1.86°C kg/mol.) Volume %3D What is the boiling point of this solution? Boiling point °C %3D 5 item attempts remaining Submit Answer Try Another Version [References] Consider an aqueous solution...
Hi, I need some help with Chemistry. Q1: Q2: Here is some background for the questions: Thank y...
Hi, I need some help with Chemistry.
Q1:
Q2:
Here is some background for the questions:
Thank you in advance.
You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...
A.) A protein solution containing 70.0 mg of the protein (dissolved in water) displays an osmotic...
A.) A protein solution containing 70.0 mg of the protein (dissolved in water) displays an osmotic pressure of 319.88 Pa at 310.15 K. If the volume of the protein solution is 22.0 mL, what is the molar mass of the protein? B.)What is the boiling point (in °C) of a solution of 8.16 g of I2 in 57.5 g of toluene, assuming the I2 is nonvolatile? (For toluene, Tb = 110.63°C and Kb = 3.40°C·kg/mol.) C.)What is the freezing point...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass of benzoic acid grams) Freezing temperature of pure lauric acid (°C) From Part 8.02 11.04 g. 4 2.95 4 227900 Freezing point of the benzoic acid and lauricucid ("C) Part III: Unknown solute and lauric Acid Mass of lauric acid (grams) 8.0 49 Mass of unknown solute (grams) P.98g Freezing temperature of pure lauric acid ("C) (From Part 45°C Freezing point of the unknown...
An Alka-Seltzer tablet consists of NaHCOs (sodium bicarbonate), citric acid (H3C&HsO; citric acid...
I Need the pre-lab
Questions, please
An Alka-Seltzer tablet consists of NaHCOs (sodium bicarbonate), citric acid (H3C&HsO; citric acid is triprotic), aspirin and other inert ingredients. When dissolved in water, citric acid and NaHCO3 components react as follows: In the first part of the experiment, we will determine the mass of NaHCO in a tablet of Alka Seltzer. To do this, we will use a known mass of a powdered sample of Alka-Seltzer and determine the mass of CO2 gas...
9. A solution of 1,035 g of benzoic acid in 8.525 g of lauric acid had a freezing point of 39.6 C What is the molar mass of benzoic acid? The freezing point of lauric acid is 43.2 C and Kris 3.60 C.kg/mol.
מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water to give a solution whose freezing point is -3.8°C. The freezing point depression constant of water is 1.86 °C/m. The molar mass of glucose is 180.16 g/mol Give your answer in grams to 3 significant figures
Course Contents> ... Experiment 6 -- Colligative Properties -- Freezing Point De Due in 3 hours, 1 minute 5 homework point(s) Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent K=20.0. 0.144 g of an unknown solute is dissolved in 7.88 g of cyclohexane (C6H12). The freezing point of the solution was 3.36°C. Calculate the corresponding molar mass of the solute. 117.89 g/mol 1homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries To the...
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water to produce an antifreeze solution with a freezing point of-19.0°C? (The density of ethylene glycol is 1.11 g/cm°, and the density of water is 1.00 g/cm³. K, for water is 0.51°C•kg/mol and Kf is 1.86°C kg/mol.) Volume %3D What is the boiling point of this solution? Boiling point °C %3D 5 item attempts remaining Submit Answer Try Another Version [References] Consider an aqueous solution...
Hi, I need some help with Chemistry.
Q1:
Q2:
Here is some background for the questions:
Thank you in advance.
You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass of benzoic acid grams) Freezing temperature of pure lauric acid (°C) From Part 8.02 11.04 g. 4 2.95 4 227900 Freezing point of the benzoic acid and lauricucid ("C) Part III: Unknown solute and lauric Acid Mass of lauric acid (grams) 8.0 49 Mass of unknown solute (grams) P.98g Freezing temperature of pure lauric acid ("C) (From Part 45°C Freezing point of the unknown...
I Need the pre-lab
Questions, please
An Alka-Seltzer tablet consists of NaHCOs (sodium bicarbonate), citric acid (H3C&HsO; citric acid is triprotic), aspirin and other inert ingredients. When dissolved in water, citric acid and NaHCO3 components react as follows: In the first part of the experiment, we will determine the mass of NaHCO in a tablet of Alka Seltzer. To do this, we will use a known mass of a powdered sample of Alka-Seltzer and determine the mass of CO2 gas...
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