A biomedical engineer is working in a lab that is isolating gene fragments. She dissolves a 10.0mg sample in enough water to make 30.0mL of solution. The osmotic pressure of the solution is 0.340torr at 25C. What is the molar mass of the gene fragment? If the solution density is 0.997g/mL, what is the freezing point for this aqueous solution?
Osmotic pressure of a solution is calculated as follows:
Where C is the molar concentration
R is gas constant =
Hence, we can write
Hence, the concentration of gene fragment is .
It is given that the solution volume is 30.0 mL = 0.030 L.
Hence, the number of moles of gene fragment in the 30.0 mL volume is
Hence, 10.0 mg sample of the gene fragment equals . Hence, the molar mass can be calculated as
hence, the molar mass of the gene fragment is (rounded to three significant figures).
Now, given that the density of the solution is 0.997 g/mL
The mass of the solution of volume 30.0 mL can be calculated as
Now, the presence of the gene fragment lowers the freezing point of the aqueous solution compared to that of pure water.
The change in freezing point is calculated as
Where i is the van't Hoff factor ( For a non-electrolyte like a gene fragment , i=1)
Kf is the molal freezing point depression constant of water =
m is the molality of solvent given in moles of solute per kg of solvent.
Now, we can calculate the molality of our solution as follows:
Moles of gene fragment = (already calculated above)
Mass of solvent = Mass of solution - Mass of gene fragment = 29.91 g - 0.01 g = 29.90 g = 0.0299 kg
Hence,
Hence, we can calculate the depression in freezing point as follows
We know that the freezing point of pure water = 0 oC
Hence, the freezing point of the solution can be calculated as
Note that practically the freezing point of the solution is almost close to zero as the moality of the solution is so low owing to the high molar mass of gene fragment.
A biomedical engineer is working in a lab that is isolating gene fragments. She dissolves a...
Hy 1.008 664,427 0 15.964 18. A biochemical engineer isolates a bacterial gene fragment and dissolves a 20.6. mg sample of the material in enough water to make 41.5 mL of solution. The osmotic pressure of the solution is 0.340 torr at 25.0°C. (a) What is the molar mass of the gene fragment (5 pts)? 2mci we6 .0206 s .0415 C= .0206 ms.
2 attempts left Check my work Be sure to answer all parts. A biochemical engineer isolates a bacterial gene fragment and dissolves a 16.0-mg sample in enough water to make 30.0 mL of solution. The osmotic pressure of the solution is 0.340 torr at 25°C. (a) What is the molar mass of the gene fragment? g/mol (b) If the solution density is 0.997 g/mL, how large is the freezing point depression for this solution (K of water = 1.86°C/m)?
In a study designed to prepare new gasoline-resistant coatings, a polymer chemist dissolves 6.117 g poly(vinyl alcohol) in enough water to make 100.0 of mL solution. At 25°C, the osmotic pressure of this solution is 0.266 atm. What is the molar mass of the polymer sample?
5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 mL of solution. The osmotic pressure at 25C is 278.0 torr. What is the molar mass of the solid? 6a. Calculate the van't Hoff factor of a 0.085M potassium sulfate solution that has an osmotic pressure of 5.4atm at 25C 5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 ml. of solution. The osmotic pressure at 25...
A 36.5% by mass of C6H12O6, aqueous solution is prepared in the lab. the density of the solution is 2.97 g/ml. what is the osmotic pressure of the solution at 42 OC ( R=0.08206 L*atm/mol*K)
[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...
how much is a working solution will she need to neutralize 10.5 ML of 0.250MH3 PO four Please answer C and show steps. Thank you! C. How much of the working solution will she need to neutralize 10.5 mL of 0.250 M H3PO4? 2. A student prepared a stock solution by dissolving 15.0 g of NaOH in enough water to make 150 mL of a stock solution. She then took 22.5 mL of the stock solution and diluted it with...
Conceptual Questions L You are working as a technician in a lab, and your supervisor has asked you to isolate the gene for super sweet corn (ssc/) from-the sample of corn genomic DNA. She gives you the following map, and she also gives you a radioactively labeled probe that is specific for the scl gene. Devise an experimental protocol to isolate the gene from-the genomic DNA, what enzymes would you use to digest the DNA? How would you isolate the...
3a. How many grams of sucrose must be added to 430g of water to lower the vapor pressure 1.4mmHg at 25C? The vapor pressure of water at 25C is 233.8 mmHg and molar mass is 342.3 g/mol 3. Vapor pressure lowering a) How many grams of sucrose must be added to 430 R of water to lower the vapor pressure 1.4 mm Hg at 25 °C? The vapor pressure of water at 25°C is 23.8 mm Hg and the molar...
1. 1200 mL aqueous solution of 45 g of ethylene glycol and 80 g of sucrose were prepared with a density of 1.37 g/mL. Assume that the solution behaves ideally. Notes: The vapor pressures of water and ethylene glycol at 20 °C are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water are 0.51 K/m and 1.86 K/m, at 25 °C respectively. a. What is the freezing point of this solution? b. What is the vapor pressure,...