as we move down the group Mg, Ca, and Ba, what happen to the solubility of (a) sulfates, (b) hydroxides, (c) carbonates?
As we move down the group from Mg to Ca to Ba, the solubility of sulfates, hydroxides, and carbonates increases. This is due to the increase in atomic size and decrease in ionization energy as we move down the group, which leads to a decrease in the lattice energy of the compounds. As a result, the compounds become more soluble in water.
Specifically:
(a) The solubility of sulfates increases as we move down the group Mg, Ca, and Ba. Magnesium sulfate (MgSO4) is slightly soluble in water, while calcium sulfate (CaSO4) is moderately soluble, and barium sulfate (BaSO4) is highly insoluble.
(b) The solubility of hydroxides also increases as we move down the group. Magnesium hydroxide (Mg(OH)2) is slightly soluble in water, while calcium hydroxide (Ca(OH)2) is moderately soluble, and barium hydroxide (Ba(OH)2) is highly soluble.
(c) The solubility of carbonates follows the same trend. Magnesium carbonate (MgCO3) is slightly soluble in water, while calcium carbonate (CaCO3) is sparingly soluble, and barium carbonate (BaCO3) is more soluble.