In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15oC. Barium nitrate dissociates via the process: Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q) Ksp = [Ba2+][NO3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPa
In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was
filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine
Ksp. It was observed in their experiments that the solution boils at 100.15oC. Barium nitrate dissociates via the process:
Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q)
Ksp = [Ba2+][NO3−]2
Calculate the following if Kb,water = 0.51 K-kg/mol:
a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol
b) Solubility product, Ksp
c) Vapor pressure of the solution in kPa
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