The initial freezing temperature of 0.13 kg of a pure solvent is 6°C. 15.0 grams of a solute with molar mass of 147.63 g/mol is added to the pure solvent. The solute is known to dissociate into 2 ionic particles when dissolved in the pure solvent. The freezing temperature of the solution after the addition of the solute is -3°C. What is the Kf of the solvent?

Determine the freezing point of the solution. (Use Kf = 1.86 °C/m.)

2 Zn*2 (aq) +Fe*2 (ag) + 6 CN (ag) = Zn2Fe(CN)6 (5) [znz Fe (CN),] A certain equilibrium reaction has K = 2.8 x 10-13 at 25 °C. What is the change in Gibbs Free Energy (kJ/mole) under these conditions?

Using the Kf value for water from your book, you prepare a solution at 25.0 °C from 9.17 mol of some solid and 7.31 L of water (d = 0.997 g/mL), but you forgot the identity of the solid. You know it was either glucose, sodium acetate, sodium phosphate, or sodium sulfate. You decide to determine the mass indirectly by measuring the freezing point depression of the solution, and find that the solution has a freezing point of −7.02 °C. Which substance is it and how do you know this?

The solubility of the hypothetical salt A3 B2 is 6.2 × 10–º mol/L at a certain temperature. What is Ksp for the salt? A3 B2 dissolves according to the equation Aз В2(8) — ЗА?t (ag) + 2B% (аq)

Be sure to answer all parts. The solubility of an ionic compound M2X3 (molar mass = 287 g) is 6.60 × 10 17 What is Kp for the compound? ds. X 10 (Enter your answer in scientific notation.)

Camphor is a white solid that melts at 179.50°C. It has been used to determine the molecular weights of organic compounds because of its unusually large freezing-point-depression constant (39.7°C/m), which allows ordinary thermometers to be used. The organic compound is dissolved in camphor, and then the melting point of the solution is determined. If 1.08 g of an unknown compound is dissolved in 73.6 g camphor, the freezing point is found to be 177.09°C. What is the molecular weight of the unknown compound?

Calculate the molality of a solution composed of 4.5g of AgNO3 in 250mL of aqueous solution.

Drug B has a solubility of 2.5 g B 100−1 g−1 water at 80oC and at 4oC the solubility of B is only 0.36 g B 100−1 g−1 of water. If a saturated drug solution at 80oC has 1000 g of drug in it, determine how much water (W) is also present with the drug. The solution is then cooled to 4oC and the drug precipitate is separated from the saturated drug solution. How much of the drug will be precipitated (P) from the initial solution?

Consider a body of water in equilibrium with solid calcium sulfate, CaSo4, for which Ksp= 3.0 x 10^-5 at 25 degrees C. Calculate the solubility, in g/L, of calcium sulfate in water assuming that other reactions are negligible.  *