Exposing a 250 mL sample of water at 20.∘C to an atmosphere containing a gaseous solute at 27.59 kPa resulted in the dissolution of 4.51×10−3 g of the solute. Use Henry's law to determine the solubility of this gaseous solute when its pressure is 79.39 kPa.

When 14.3 g of a certain molecular compound X are dissolved in  85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X.   molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07   If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to  2  significant digits.

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?

The solubility of an ionic solid in water is quantified by this expression:   Ksp   Kc   Keq   Ka or Kb

(a) Calcium fluoride, CaF2, has Ksp= 4.0 x 10–11; what is the solubility of CaF2 in water? (b) What is the solubility of CaF2 in 0.050 M NaF solution? (c) What is the solubility of CaF2 in 0.010 M CaCl2solution? (Express all solubility in mol/L)

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.  *

At 25 °C the solubility of lead(Il) bromide is 2.70 x 10 mol/L. Calculate the value of Kgp at this temperature. Enter your answer in exponential format using a capital "E (example 1.23E-4) and no units (value 2%).

7. Camphor (C10oH160) freezes at 179.8°C, and it has a particularly large freezing point depression constant, Kf = 40.0 °C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 176.7°C. What is the molar mass of the solute?

A chemistry student weighs out 0.011 kg of an unknown solid compound X and adds it to 100 ml of distilled water at 17. C. After 10 minute stirring, all of the X has dissolved. Just to be sure, the student adds a further 25. mg of X to the solution, and it, too, dissolves. Using only the information above, can you calculate the solubility of Xin water at 17.° C7 If you said yes, calculate it. Be sure your answer has a unit symbol and 21 O yes 0 no 0.0 X H DID G 4.

For the calculation of the solubility c of a gas in a solvent, it is often convenient to use the expression c = Kp, where K is the Henry’s law constant. Breathing air at high pressures, such as in scuba diving, results in an increased concentration of dissolved nitrogen. The Henry’s law constant for the solubility of nitrogen is 0.18 μg/(g H2O atm). What mass of nitrogen is dissolved in 100 g of water saturated with air at 4.0 atm and 20 °C? Compare your answer to that for 100 g of water saturated with air at 1.0 atm. (Air is 78.08 mol per cent N2.) If nitrogen is four times as soluble in fatty tissues as in water, what is the increase in nitrogen concentration in fatty tissue in going from 1 atm to 4 atm?