Final answer:
The solubility product constant (Ksp) of AB in a solution of C is calculated using the solubility given as 0.142 M, with the formula Ksp = [A+][B-] = s^2, which equals 0.020164. However, this calculation assumes no significant complex ion formation or common ion effects that could affect solubility.
Step-by-step explanation:
To calculate the solubility product constant (Ksp) of a slightly soluble compound AB in the presence of another ionic compound C, one must apply the concept of reaction stoichiometry and equilibrium expressions. Given that the solubility of AB is 0.142 M in a 1.000 M solution of C, the Ksp can be determined if AB dissociates according to the equation AB(s) ⇄ A+(aq) + B-(aq).
If we assume the solubility of AB is represented by 's' mol/L, then [A+] = [B-] = s, under the assumption that common ion effects or complex ion formation does not appreciably affect the solubility (as could be the case with different stoichiometries or additional reactions). Therefore, Ksp = [A+][B-] = s^2. Substituting in the given solubility, Ksp = (0.142)^2 = 0.020164.
Please note, however, that additional equilibrium reactions, such as complex ion formation or common ion effects, can alter the simple stoichiometric relationship used in this calculation. In such cases, additional information and a more complex equilibrium analysis would be required to determine the Ksp.