The solubility products of MA, MB, MC and MD are 1.8 x 10^-10, 4 x 10^-3, 4 x 10^-5 and 6 x 10^-5, respectively. If a 0.01 M solution of MX is added dropwise to a mixture containing A, B, C and D ions then the one to be precipitated first will be
Correct answer: A. MA
- A. MA
- B. MC
- C. MB
- D. MD
Explanation
The explanation is: To determine which compound will precipitate first when a 0.01 M solution of MX is added dropwise to a mixture containing A, B, C, and D ions, we need to compare the solubility product constants (Ksp) of the compounds. The compound that will precipitate first is the one with the lowest solubility product constant because a lower Ksp value indicates lower solubility. Given the solubility product constants of the compounds: Ksp(MA) = 1.8 x 10-10 Ksp(MB) = 4 x 10-3 Ksp(MC) = 4 x 10-5 Ksp(MD) = 6 x 10-5 Comparing the values, we can see that the solubility product constant of MA (1.8 x 10^-10) is the lowest among the given compounds. Therefore, when a 0.01 M solution of MX is added dropwise to the mixture, compound MA will precipitate first because it has the lowest solubility product constant.
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