Question

At a particular temperature the value of [Ba²⁺] in a saturated solution of barium sulfate is 1.060 x 10⁻⁵ M. Starting with this information, calculate the Ksp of barium sulfate at this temperature.

Answer 1

The Ksp for barium sulfate, given the concentration of barium ions [Ba²⁺] in a saturated solution, is calculated as the product of the concentrations of barium and sulfate ions, resulting in a Ksp value of 1.1236 x 10⁻⁹.

Step-by-step explanation:

To calculate the Ksp (solubility product constant) for barium sulfate (BaSO4), we use the provided concentration of barium ions [Ba²⁺] in a saturated solution. Given that [Ba²⁺] = 1.060 x 10⁻⁵ M, and knowing that the stoichiometry of the dissolution of BaSO4 is 1:1, the concentration of sulfate ions [SO︲⁺⁺] will be the same, 1.060 x 10⁻⁵ M.

The formula for the Ksp is:

Ksp = [Ba²⁺][SO︲⁺⁺]

Substituting the values, we get:

Ksp = (1.060 x 10⁻⁵ M)(1.060 x 10⁻⁵ M) = 1.1236 x 10⁻⁹ (rounded to four significant figures).

Therefore, the Ksp for barium sulfate at this temperature is 1.1236 x 10⁻⁹.