The high melting points of ionic solids indicate that a lot of energy must be supplied to separate the ions from one another. How is it possible that the ions can separate from one another when soluble ionic compounds are dissolved in water, often with essentially no temperature change?
Answer to relevant Questionsa. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. b. Based on your answers to part a, which ion, Cl2 or I2, is more strongly attracted to water? Which solvent, water or carbon tetrachloride, would you choose to dissolve each of the following? a. KrF2 b. SF2 c. SO2 d. CO2 e. MgF2 f. CH2O g. CH2PCH2 Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate. Consider the following: What would happen to the level of liquid in the two arms if the semipermeable membrane separating the two liquids were permeable to a. H2O (the solvent) only? b. H2O and solute? You add an excess of solid MX in 250 g of water. You measure the freezing point and find it to be 20.028oC. What is the Ksp of the solid?
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