To calculate the pH of a 0.05M solution of Al(OH)3, we need to consider the hydrolysis reaction of Al(OH)3 in water. This reaction can be represented as follows:
Al(OH)3 + 3H2O ⇌ Al(OH)4- + 3H+
The Al(OH)3 will hydrolyze to form Al(OH)4- ions and release H+ ions. Since Al(OH)3 is a weak base, we can assume that it dissociates completely.
To calculate the pH, we need to determine the concentration of H+ ions in the solution. Since Al(OH)3 dissociates into 3 H+ ions, the concentration of H+ ions will be 3 times the initial concentration of Al(OH)3.
So, the concentration of H+ ions in the solution will be 0.05M * 3 = 0.15M.
Using the pH formula, pH = -log[H+], we can calculate the pH:
pH = -log(0.15) ≈ 0.82
Therefore, the pH of a 0.05M solution of Al(OH)3 is approximately 0.82.
