A sparingly soluble salt is given by the formula MX2, where the metal M forms ions of the type M+. How would the solubility product constant be defined in terms of the concentration of the ions? A B Ksp = [M2+] [X^ ] Ksp = [M2+][2X-] Ksp = [M2+ ] [X=]2 Ksp = [M+] [2X-12 OA. O B. OC. OD. A Moving to the next question prevents changes to this answer. ME de in 5 K