A molal is a unit of concentration that represents the number of moles of solute per kilogram of solvent. It is calculated by dividing the number of moles of solute by the mass of the solvent in kilograms.
m = moles/kg = 3.00/1.50 = 2.00 molal
During the determination of the partial molal quantities the weight of the solution to which a substance is added is taken into consideration while in case of the partial molar quantity the volume is taken into consideration.
The answer is 15,015 g.
The answer is 15,039 g hydrogen chloride (HCl).
A one molal solution of urea contains one mole of urea dissolved in one kilogram of solvent (usually water), while a one molar solution contains one mole of urea dissolved in one liter of solution. Since the density of the solution can vary, a one molal solution typically has a lower concentration of urea in terms of volume compared to a one molar solution, making it more dilute. This is because the molarity takes into account the total volume of the solution, while molality focuses only on the mass of the solvent.
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This is a colligative property which does not depend on the nature of solute is the molal boiling point elevation constant or ebullioscopic constant of the solvent.
They are equivalent. Molal is now an obsolete, not recommended term.
To determine the molal concentration of a solution, you need to divide the moles of solute by the mass of the solvent in kilograms. This calculation gives you the molality of the solution, which is expressed in moles of solute per kilogram of solvent.
The boiling point is 101 oC.
In order to compare the molality of two solutions, you need to consider the number of particles the solute separates into in a solution. Urea (CH4N2O) separates into one particle in solution, while NaCl separates into two particles. Therefore, 1 molal urea solution is equal to 0.5 molal NaCl solution because NaCl produces twice as many particles in solution as urea.
m = moles/kg = 3.00/1.50 = 2.00 molal
Molal depression constant (Kf) is a colligative property constant that relates the lowering of the freezing point of a solvent to the molality of a solute in the solution. It is specific to each solvent and typically expressed in units of °C kg/mol.
Aprox. 830 g.
The freezing point depression of a solution is given by the equation ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the cryoscopic constant, and m is the molality of the solution. With the molality (m) of 3.23 molal and the cryoscopic constant for water (Kf) being approximately 1.86 ºC kg/mol, you can calculate the freezing point depression.
Approx. 830 g potassium iodide.
The freezing point depression constant for water is 1.86 degrees Celsius per molal.