How could i determine the apparent molal concentration of BaNO3 when the freezing point of the aqueous solution is -2.65 degrees Celcius
divide by the freezing point depression constant of water.
freezing point=molality*freezing point depression constant
To determine the apparent molal concentration of Ba(NO3)2 in an aqueous solution using freezing point depression, you'll need a few key pieces of information:
1. Freezing point constant (Kf) of the solvent: The Kf value is specific to the solvent you're using. For water (the common solvent in aqueous solutions), the Kf value is 1.86 °C kg/mol.
2. Freezing point depression (∆Tf): This is the difference between the freezing point of the pure solvent and the freezing point of the solution. In this case, ∆Tf is given as -2.65 °C.
Now, you can use the formula to calculate the apparent molal concentration:
∆Tf = Kf x molality
To rearrange the formula and solve for the molality (molal concentration), divide both sides of the equation by Kf:
molality = ∆Tf / Kf
Insert the values for ∆Tf (-2.65 °C) and the Kf value for water (1.86 °C kg/mol):
molality = -2.65 °C / 1.86 °C kg/mol
After calculating the division, you will get the molality of the solution. This represents the number of moles of solute (Ba(NO3)2) per kilogram of solvent (water).