Ksp for X(OH)2 in a certain temperature equal (3.6x10-13), pH value for its saturated solution equals:

To determine the pH value of a saturated solution of X(OH)2, we need to consider the dissociation of X(OH)2 in water.

The dissociation of X(OH)2 can be represented by the equation: X(OH)2 ⇌ X2+ + 2OH-

The equilibrium constant for this dissociation reaction is known as the solubility product constant, Ksp. In this case, the Ksp for X(OH)2 is given as 3.6x10-13.

Since X(OH)2 dissociates into X2+ and 2OH-, we can assume that the concentration of X2+ is equal to the concentration of OH- in the saturated solution. Let's represent the concentration of X2+ and OH- as [X2+] and [OH-], respectively.

Using the stoichiometry of the dissociation reaction, we can write the expression for Ksp as: Ksp = [X2+][OH-]^2

Since [X2+] = [OH-], we can substitute [X2+] with [OH-] in the Ksp expression: Ksp = [OH-][OH-]^2 Ksp = [OH-]^3

Now, we can solve for [OH-] by taking the cube root of Ksp: [OH-] = (Ksp)^(1/3) [OH-] = (3.6x10-13)^(1/3)

Finally, to find the pH value of the saturated solution, we need to calculate the concentration of H+ ions. Since water undergoes autoionization to produce equal concentrations of H+ and OH- ions, the concentration of H+ is also equal to [OH-].

Therefore, the pH value of the saturated solution of X(OH)2 is equal to the negative logarithm (base 10) of the concentration of H+ ions, which is equal to [OH-].

pH = -log[H+] pH = -log[OH-] pH = -log((3.6x10-13)^(1/3))

By evaluating this expression, you can find the pH value for the saturated solution of X(OH)2 at the given temperature.