a solution is prepared by dissolving 4.9 g of sucrose (C12H22O11) in 175 g of water. calculate the boiling point and osmotic pressure of this solution at 25°c. assume that molarity and molality of this solution are equal. E(h2O) = 0.52.

delta T = i*Kb*molality

i = 1 for sucrose
Kb. You need to look up that constant. For water it is approximately 0.51 C/m but don't assume I am correct. Confirm that.
molality = moles sucrose/kg solvent. mols = g/molar mass and solvent is 0.175 kg.
Substitute and solve for delta T, then add that increment to the normal boiling point of water.
For osmotic pressure use
p = MRT. The problem tells you to use as M the same you calculated for m. You know R and T. Solve for osmotic pressure in atm if you use R = 0.08205. Post your work if you get stuck.

To determine the boiling point and osmotic pressure of a solution, you will need to use the formulas regarding colligative properties. There are three main colligative properties: boiling point elevation, freezing point depression, and osmotic pressure. In this case, we are concerned with the boiling point elevation.

1. Calculate the molality of the solution:
Molality (m) = moles of solute / mass of the solvent (in kg)

To find the moles of sucrose, use the molar mass of sucrose (342.3 g/mol):
Moles of sucrose = mass of sucrose (in g) / molar mass of sucrose

Moles of sucrose = 4.9 g / 342.3 g/mol

Now, calculate the mass of the water in kg:
Mass of water = 175 g / 1000 (to convert grams to kg)

Now, you can calculate the molality:
Molality = moles of sucrose / mass of water (in kg)

2. Calculate the boiling point elevation (∆Tb):
∆Tb = Kb * i * m

In this case, we are assuming that the molarity and molality of the solution are equal, so the van't Hoff factor (i) is 1.
Kb is the molal boiling point elevation constant for water, which equals 0.52 °C/molal.

∆Tb = 0.52 °C/molal * 1 * molality

3. Calculate the boiling point of the solution:
Boiling point = normal boiling point of the solvent + ∆Tb

The normal boiling point of water is 100 °C.

4. Calculate the osmotic pressure of the solution (∏):
∏ = i * M * R * T

In this case, we are assuming that the molarity and molality of the solution are equal, so the van't Hoff factor (i) is 1.
M is the molarity of the solution, which is equal to the molality.
R is the ideal gas constant, approximately 0.0821 L·atm/(mol·K).
T is the temperature in Kelvin, which is 25 °C + 273.15.

Now, you can substitute the values into the formula to calculate the osmotic pressure (∏).

These steps will allow you to calculate both the boiling point and osmotic pressure of the solution at 25 °C.