(V) (8 points) What is the freezing point temperature for a solution of 1.221 g of...
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.
6) A solution made by dissolving 1.083 g of benzoic acid (CyH6O2) in 8.242 g of lauric acid. (benzoic acid MM =122.13 g/mol; lauric acid FP = 43.2°C: K= 3.87°C kg/mol a) What is the mass percent of benzoic acid? b) What is the molality of the solution? c) What is the freezing point of the solution?
DATA AND CALCULATIONS Mass of lauric acid Mass of benzoic acid Freezing temperature of pure lauric acid Freezing point of the benzoic acid-lauric acid mixture Freezing temperature depression, At 38-1c Molality, m molkg Moles of benzoic acid mol Molecular weight of benzoic acid (experimental) g/mo Molecular weight of benzoic acid (accepted) g/mol Percent error
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
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...
A 2.00 g samples of benzoic acid (mw = 122.2 amu) is dissolved in 50.0 g of lauric acid acid, which has a normal melting point of 45.0 oC. If the new solution has a depressed freezing point of 43.7 oC, what is the freezing point depression constant for lauric acid? A.0.251 oC/m B.3.97 oC/m * C.3.25 oC/m D.0.307 oC/m E.None of the above
CHM 112 Determination of Molar Mass by Freezing Point Depression Report Sheet and Data Analysis DATA TABLE Mass of lauric acid (g) 8.003 Mass of benzoic acid (g) 1.005 Freezing temperature of pure lauric acid (°C) 42.4 Freezing point of the benzoic acid-lauric acid mixture (°C) 38.7 Discuss possible sources of error in this experiment and how those errors would affect the final calculated molar mass. This is an open ended question and a thorough answer is expected. You should...
What is the freezing point of a solution containing 22.78 g juglone (C10H6O3), a nonelectrolyte, and 207.0 g acetic acid (CH3COOH)? The normal freezing point of acetic acid is 16.60 °C and Kfp for acetic acid is 3.90 °C/m
What is the freezing point of a solution containing 45.39 g 5-bromo-2-naphthoic acid (C11H7BrO2), a nonelectrolyte, and 160.7 g acetic acid (CH3COOH)? The normal freezing point of acetic acid is 16.60 °C and Kfp for acetic acid is 3.90 °C/m.
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...