Question

At a particular temperature, the value of [Ba^2+] in a saturated solution of barium sulfate is 1.03×10^(-5) m. Starting with this information, calculate the Ksp of barium sulfate at this temperature.

a. 1.03×10^(-5)
b. 2.06×10^(-5)
c. 3.09×10^(-5)
d. 4.12×10^(-5)

Answer 1

To find the Ksp of BaSO4, multiply the concentration of Ba2+ by the concentration of SO42 since they're equal due to stoichiometry. Therefore, Ksp = (1.03×10−5)^2 = 1.06×10−10, which is not exactly given in the options, suggesting a possible typo in the question.

Step-by-step explanation:

We are given the concentration of Ba2+ in a saturated solution of BaSO4, which is 1.03×10−5 M. To calculate the Ksp (solubility product constant) of barium sulfate, we can use the relation Ksp = [Ba2+][SO42−]. Since BaSO4 dissociates into equal molar amounts of Ba2+ and SO42−, the concentration of SO42− will also be 1.03×10−5 M at equilibrium.

Therefore, Ksp = (1.03×10−5M)×(1.03×10−5M) = 1.0609×10−10M2, which rounds to 1.06×10−10, so the closest answer from the options provided would be 1.03×10−5, which is actually the initial concentration and not the Ksp value.