A saturated solution of (Al(OH)3) was measured to have 5.01 10–7 M of hydroxide ions at 25 degrees celsius . Calculate the solubility product constant of (Al(OH)3)
To calculate the solubility product constant (Ksp) of (Al(OH)3), we can use the following equation:
Ksp = [Al3+][OH-]^3
Given that the concentration of hydroxide ions ([OH-]) is 5.01 × 10^(-7) M, and assuming that the concentration of aluminum ions ([Al3+]) is also 5.01 × 10^(-7) M (since the compound is Al(OH)3 and the ions should have a one-to-one ratio), we can substitute these values into the equation:
Ksp = (5.01 × 10^(-7))^2 × (5.01 × 10^(-7))^3
Simplifying this expression gives:
Ksp = (5.01 × 10^(-7))^5
Ksp ≈ 1.258 × 10^(-34)
Therefore, the solubility product constant (Ksp) of (Al(OH)3) is approximately 1.258 × 10^(-34).