Question

Write the chemical equation for the dissolution of calcium hydroxide in water, and write its corresponding K_sp equilibrium expression. Write the balanced chemical equation for the reaction of HCl with calcium hydroxide, which yields water and calcium chloride. During the experiment, 25.00 mL of calcium hydroxide solution was titrated with 5.50 mL of 0.102 M HCl. Determine the mass of calcium hydroxide (in grams) used in the titration based on the data provided. Determine the solubility of the calcium hydroxide in 25.00 ml based on your answer to Part A. Determine the Ksp for calcium hydroxide based on the data provided. The literature value for the K_sp of calcium hydroxide is 7.90 times 10^-6. Calculate the % error for the data collected. The equation below can be used to determine the enthalpy and entropy change for the solubility of the calcium hydroxide. Ln K = (-delta H degree/R) 1/T + delta S degree/R If a plot of In K_sp vs 1/T produces a slope of +1.875 K and a y-intercept of -18.5, calculate the values of both delta H degree (in kJ/mol) and delta S degree (in J/K-mol). Use your value of K from question 3d and R = 8.314 J/K-mol for the calculations.
pls help me solve question 3 and 4 thank you.

Answer 1

(a) 15.50 mL×-- x1000 mLj (0.102 M) = 5.61×10-4 mol mol HCI = mol Ca(OH), -5.61x10-mo1x-_ 2.80% 10 mol Mass ofca (OH)= moles x molar mass = ( 2.805x10 4 mol)x(74.09 gmol) = O02078 g . mol Ca (OH)2.805x10* mol Solubility = = 0.01 122 mol/L volume 0.02500L Ca2+ I = 0.01 1 22 mol/L OH- | = 2(0.01 122 mol/L ) 0.02244 mol L K, = (0.01122)x(0.02244 5.65 x 10-6 = 7.90x10* 10-*)-(5.65x10-* 7.90x10-6 % error 100 = 28.5%