Equilibrium & pH: Concentration of Ba2+ in Saturated BaCrO4

[phatpenguin]

What is the concentration of Ba2+ in a saturated BaCrO4 solution?

 

[Kushal]

do you happen to know the Ksp of BaCrO4?

 

[Blueshift5]

The concentration of Ba2+ in a saturated BaCrO4 solution can be determined using the equilibrium expression for the dissociation of BaCrO4:

BaCrO4(s) ⇌ Ba2+(aq) + CrO42-(aq)

At equilibrium, the concentration of Ba2+ and CrO42- ions will be equal, and the equilibrium constant (Ksp) can be used to calculate their concentrations. The Ksp for BaCrO4 is 1.17 x 10^-10 at 25°C.

Ksp = [Ba2+][CrO42-]

Since the solution is saturated, we can assume that the concentration of BaCrO4 (solid) remains constant. Therefore, we can rearrange the equilibrium expression to solve for the concentration of Ba2+:

[Ba2+] = Ksp/[CrO42-]

Substituting in the value of Ksp, we get:

[Ba2+] = (1.17 x 10^-10)/[CrO42-]

Since the concentration of CrO42- is equal to the concentration of Ba2+, we can represent it as [Ba2+]^2:

[Ba2+] = √(1.17 x 10^-10) = 1.08 x 10^-5 M

Therefore, the concentration of Ba2+ in a saturated BaCrO4 solution is 1.08 x 10^-5 M. It is important to note that this value may vary depending on temperature and other factors that can affect the solubility of BaCrO4.