The solubility product of Al(OH)3 is 2x10^32. Calculate its solubility in pure water
To calculate the solubility of Al(OH)3 in pure water, we need to use the concept of solubility product constant (Ksp). The solubility product constant describes the equilibrium between the dissolved ions and the solid compound in a saturated solution.
The solubility product constant (Ksp) expression for Al(OH)3 is given as:
Ksp = [Al3+][OH-]^3
where [Al3+] represents the concentration of Al3+ ions and [OH-] represents the concentration of OH- ions in the saturated solution.
Since Al(OH)3 dissociates into Al3+ and OH-, we can assume that the concentrations of Al3+ and OH- are equal.
Let's assume that the solubility of Al(OH)3 is "s". Therefore, [Al3+] = s and [OH-] = s.
Substituting these values into the Ksp expression:
Ksp = [Al3+][OH-]^3
2x10^32 = s * s^3
2x10^32 = s^4
To solve for "s", we need to take the fourth root of both sides of the equation:
s = (2x10^32)^(1/4)
s = 8x10^8
Therefore, the solubility of Al(OH)3 in pure water is 8x10^8.