Based on the following data, compare the effect of crystal size on solubility in water at 25oC for (1) KCl, a soluble inorganic salt, with that for (2) BaSO4, an almost insoluble inorganic salt, and (3) sucrose, a very soluble organic compound. σs,L for barium sulfate=0.13 J/m2 and σs,L for sucrose =0.01 J/m2 What conclusions can you draw from the results?

1. a. Calculate the molar solubility of AgBr in pure water. Kp for AgBr is 5.0 x 10-13. b. Calculate the molar solubility of AgBr in 5.00 M NH3. The overall formation constant for Ag(NH3)2* is 1.7 x 10".

1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…

Why is it easy to measure the amount of adsorption of a pure gas, but difficult to measure adsorption of a pure liquid?