What is the solubility of Group 2 hydroxides and how does it relate to pH?

Group 2 hydroxides have varying solubilities and their solubility relates to pH.

Group 2 hydroxides, also known as alkaline earth metal hydroxides, are compounds formed by the reaction of Group 2 metals with water. The solubility of these hydroxides varies depending on the metal and the pH of the solution.

The solubility of Group 2 hydroxides generally increases as you move down the group. For example, magnesium hydroxide has a solubility of 0.00064 g/100 mL at 25°C, while barium hydroxide has a solubility of 3.7 g/100 mL at the same temperature.

The solubility of Group 2 hydroxides also depends on the pH of the solution. At low pH values, the hydroxides are insoluble, but as the pH increases, the hydroxides become more soluble. This is because the hydroxide ions react with the hydrogen ions in the solution to form water, which reduces the concentration of hydrogen ions and increases the pH.

A-Level Chemistry Tutor Summary: Group 2 hydroxides, like magnesium and barium hydroxide, increase in solubility as you go down the group. Their solubility is also influenced by the pH of the solution, becoming more soluble in higher pH environments. This happens because hydroxide ions in the solution react with hydrogen ions, forming water and increasing the pH.