Assuming the van't Hoff factors in the table, calculate the mass of each solute required to produce each of the following aqueous solutions.
Solute | i Measured |
NaCl | 1.9 |
MgSO4 | 1.3 |
FeCl3 | 3.4 |
PART B
258 mL of a magnesium sulfate solution that has an osmotic pressure of 4.07 atm at 301 K .
Express your answer using two significant figures.
PART C
An iron(III) chloride solution containing 297 g of water that has a boiling point of 103 ∘C.
Express your answer using one significant figure.
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Assuming the van't Hoff factors in the table, calculate the mass of each solute required to...
Calculate the mass of solute required to make 2.70 x 10^2 ml of magnesium sulfate solution that has an osmotic pressure of 3.83 atm at 312 K. MgSO4: expected- 2, measured- 1.3
1. Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol-1 that is dissolved in enough water to create 20.0 mL of solution. A) 288 K B) 314 K C) 278 K D) 293 K E) 299 K 39) 2. Identify the solute with the highest van't Hoff factor. A) MgCl2 B) Naci C) MgSO4 D) nonelectrolyte E) FeCl3
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