NEET Chemistry pH & Buffer Solutions MCQ Question
Calculate the solubility product constant (Ksp) for barium sulfate (BaSO4) if the concentration of Ba2+ in a saturated solution is 1.0 x 10^-5 M.
0 x 10^-10
0 x 10^-15
0 x 10^-20
0 x 10^-25
Correct Answer
Detailed Explanation
The solubility product constant Ksp is calculated using the formula Ksp = [Ba2+][SO4 2-]. Given [Ba2+] = 1.0 x 10^-5 M, and because BaSO4 dissociates into one Ba2+ and one SO4 2-, [SO4 2-] is also 1.0 x 10^-5 M. Therefore, Ksp = (1.0 x 10^-5)(1.0 x 10^-5) = 1.0 x 10^-10.
Found an issue with this question?
Related Questions
More from
In the diagram shown above, which graph best represents the change in concentration of H2 as the reaction H2(g) + I2(g) → 2HI(g) proceeds to equilibri...
Assertion (A): For a dibasic acid H2X, the equilibrium constant for the first ionization step (Ka1) is generally greater than that for the second ioni...
Assertion (A): The solubility of a sparingly soluble salt is affected by the presence of a common ion. | Reason (R): The solubility product constant (...