Answer Happy

3. Using the data and the diagram provided below, determine the enthalpies of solytion of magnesium sulphate Enthalpy of lattice formation Ba(OH), = -2350 kJmol Enthalpy of hydration of Ba Enthalpy of hydration of OH = -460 kJmol = -1364 kJmo! Ba2+ + 2OH- (g) Y X Ba2+ (aq) + 2OH- (g) Ba(OH)2 (5) Z ΔgolGo Ba2+ (aq) + 2OH(aq)

Ba2+ (aq) + 2OH- (aq) a. What is the value of X? (do not write the equal sign or the units) b. What is the value of Y? (do not write the equal sign or the units) c. What is the value of Z? (do not write the equal sign or the units) d. Derive a formula that you would use to calculate the enthalpies of solution for Ba(OH), (in a format similar to A+B+C) a e. From the formula you have derived, calculate the enthalpy of solution for Ba(OH), (write the sign and the units) f. What does the value of the enthalpy of solution tell about the dissolution of Ba(OH), in water? g. What factor accounts for the dissolution behaviour of Ba(OH), in water?