A saturated aqueous solution of Ca(OH)2 is prepared (Ksp34.68 x 10).a. Classify Ca(OH)2 as strong acid, weak acid, strong base, or weak base.Strong baseb. Is the boiling point of this solution greater than, less than, or the same as pure water?greater thanWrite the solubility product equilibrium constant expression and determine theequilibrium concentration of the [OH-].С.d. What is the pH of this solution?12.8e. This solution is used in a titration of HCO2H. What is the conjugate of HCO2H formed?ICO2H-f. 150. mL of HCO2H solution of unknown concentration is titrated with 650. mL of theCa(OH)2 solution when endpoint is reached. What is the original concentration ofHCO¿H?

Since you have posted a question with multiple sub-parts we will solve the first three for you. To get the remaining sub-parts solved please repost the complete question and mention the sub-parts to be solved. In order find the concentration of the OH- ions we first write down the given data: Ksp= 4.68×10-6. Answer for the first sub-part (a): Calcium hydroxide is a strong base because it completely ionizes when dissolved in water. Answer for the second sub-part (b): Since it is a strong base its boiling point will be greater than the pure water. It has a boiling point of 2,8500 C. Answer for the third sub-part (c): Calcium hydroxide is AB2 type of salt. Hence the solubility product equilibrium constant expression for Ca(OH)2 is written as follows: Answer for the fourth sub-part (d): We know that, pOH= -log[OH-]. = -log[2.112×10-2] = 1.67. We know that, pH + pOH= 14. pH= 14-1.67 = 12.32.