1. Calculate the molality of benzoic acid / TBOH solution and use the measured ΔTf (the change in freezing points) to calculate the value of Kf for TBOH.
Change in freezing points is 9.1 c
TBOH used is 3.2071g and Benzoic Acid used is 0.4083g
2. Obtain the freezing point of the unknown compound/ TBOH solution from the plateau of the curves. Use your calculated Kf value above for TBOH and the measured ΔTf of the unknown compound (the change in freezing points) to calculate the molality of the unknown compound/ TBOH solution. Finally calculate the molecular weight of the unknown compound (MW = grams / moles).
Change in freezing points is 12 c
TBOH used is 3.1579g and Unknown used is 0.5092g
Homework Answers
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1. Calculate the molality of benzoic acid / TBOH solution and
use the measured ΔTf (the...
Calculate the molality of benzoic acid / TBOH solution and use the measured ΔTf (the change...
Calculate the molality of benzoic acid / TBOH solution and use the measured ΔTf (the change in freezing points) to calculate the value of Kf for TBOH. Change in freezing points is 9.1 c TBOH used is 3.2071g and Benzoic Acid used is 0.4083g
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DATA TABLE Mass of lauric acid (9) 8.25 1.09 42.22 C Mass of benzoic acid (g)...
DATA TABLE Mass of lauric acid (9) 8.25 1.09 42.22 C Mass of benzoic acid (g) Freezing temperature of pure lauric acid ('C) Freezing point of the benzoic acid-lauric acid mixture (C)39,11°c Going Further Questions: 1. Calculate molality (m), in molkg, using the formula AT- Kx m. The K value for lauric acid is 3.9°c-kg/mol. 2. Calculate moles of benzoic acid solute, using the molality and the mass (in kg) of lauric acid solvent. 3. Calculate the experimental molecular weight...
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Calculate the molality (m) for the following data: A student knows or gathered the following information: Kf = 5.12 °C/m Tf (pure) = 35.7 °C Tf (solution) = 44.4 °C mass of solvent = 5.007 g mass of unknown acid = 1.006 g ΔTf = m * Kf Answer:________
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...
What is the relationship between the moles of solute and the mass of solute? Rewrite the molality expression in terms o...
What is the relationship between the moles of solute and the
mass of solute?
Rewrite the molality expression in terms of grams and molecular
weight.
Background:
Properties that depend on the concentration of particles in solution are called colligative properties. The number of particles in a solvent can affect the freezing or boiling point of solvent. To express the effect of concentration on freezing point or boiling point, molality is used in place of molarity. Molality (m) is the number...
Same Question and data but different parts. Please solve for all three. Last attempt left QUESTION...
Same Question and data but different parts. Please solve for all
three. Last attempt left
QUESTION 1 The data given in question-1 is used in the remainder of the postlab assignment questions. A 2.0 g of unknown material was dissolved in 9.00 mL of water (density of water = 1.0 g/mL) The freezing point of pure water is 0.00 °C and Kf of water is 1.86 °C/m. If the solution made above shows a new freezing point at -2.76 °C,...
The freezing point of pure lauric acid was measured. Then the freezing point of a solution...
The freezing point of pure lauric acid was measured. Then the freezing point of a solution of 4.003 g of lauric acid with 0.399g of unknown was measured. Determine the molar mass of the unknown. Kf for lauric acid = 4.4 °C/m. Freezing point of Lauric acid =44°C Freezing point of Unknown= 39°C
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...
Drop at freezing point: A student performed the colligative properties experiment for which he measured 50.00mL...
Drop at freezing point: A student performed the colligative properties experiment for which he measured 50.00mL of a solvent and weighed it giving a mass of 75.25g. I determined that the freezing point of the pure solvent was 1.00C. Then he added 0.30g of an unknown solid and determined that the freezing point of solution was -1.00C. The Kf of the pure solvent is 20.2C / m. Use the information presented above to answer the following questions: 1. What is...
DATA TABLE Mass of lauric acid (9) 8.25 1.09 42.22 C Mass of benzoic acid (g) Freezing temperature of pure lauric acid ('C) Freezing point of the benzoic acid-lauric acid mixture (C)39,11°c Going Further Questions: 1. Calculate molality (m), in molkg, using the formula AT- Kx m. The K value for lauric acid is 3.9°c-kg/mol. 2. Calculate moles of benzoic acid solute, using the molality and the mass (in kg) of lauric acid solvent. 3. Calculate the experimental molecular weight...
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...
What is the relationship between the moles of solute and the
mass of solute?
Rewrite the molality expression in terms of grams and molecular
weight.
Background:
Properties that depend on the concentration of particles in solution are called colligative properties. The number of particles in a solvent can affect the freezing or boiling point of solvent. To express the effect of concentration on freezing point or boiling point, molality is used in place of molarity. Molality (m) is the number...
Same Question and data but different parts. Please solve for all
three. Last attempt left
QUESTION 1 The data given in question-1 is used in the remainder of the postlab assignment questions. A 2.0 g of unknown material was dissolved in 9.00 mL of water (density of water = 1.0 g/mL) The freezing point of pure water is 0.00 °C and Kf of water is 1.86 °C/m. If the solution made above shows a new freezing point at -2.76 °C,...
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...
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