Thermodynamics of Ca(OH)2

The purpose of this experiment: to measure the solubility of calcium hydroxide by titration with hydrochloric acid at two different temperatures and to use these solubilities to estimate Ksp, ΔGş. This allows your to determine ΔHş and ΔSş for the specific chemical reaction

This experiment is a paragon of elegant simplicity and ingenious breadth of concept. This semester, you have studied equilibrium, free energy, enthalpy, and entropy and the relationships between them. In this experiment, you will use relatively simple measurements to determine the equilibrium constant, ΔGş, ΔHş and ΔSş. So for the solution of a sparingly soluble compound, Ca(OH)2;
Ca(OH)2(s) <--> Ca2+(aq) + 2 OH-(aq)
From the volume of hydrochloric acid, you can determine the moles of hydrochloric acid used to neutralize the Ca(OH)2. The reaction is
Ca2+(aq) + 2 OH-(aq) + 2 HCl(aq) ---> Ca2+(aq) + 2Cl-(aq) + 2 H2O(l)
So you can determine the concetrations of Ca2+ and OH- and calculate the Ksp for Ca(OH)2
Ksp = [Ca2+][OH-]2

The free energy is related to the equilibrium constant by the equation
ΔGş = -RTln(Ksp)
where R = 8.314 J/mol•K and T is the temperature in degrees Kelvin.

In the next part of the experiment, you will titrate a saturated solution of Ca(OH)2 at a higher temp ( ~90oC). By the same method just discussed, you can calculate the Ksp and ΔG for this higher  temperature.
Because ΔGş = ΔHş - TΔSş, knowing ΔGş at two temperatures allows you to calculate ΔHş and ΔSş--two equations and two unknowns. Ahhh, algebra. Yummy.

Procedure

1. Find the solubility of calcium hydroxide in water at room temperature. A solution of calcium hydroxide will be stirring at room temperature in the laboratory. Draw off approximately 40 mL of this solution and record the temperature. Filter the solution using a long stem funnel. Pipet 10.00 mL (volumetric pipet) of the filtrate into a clean 125 mL Erlenmeyer flask and add 25 mL of distilled water and ~10 drops of bromothymol blue indicator. Titrate with the standard HCl solution (~0.02 M) until the yellow endpoint. Repeat twice more.
2. Find the solubility of calcium hydroxide of a hot solution. There will be a boiling hot Ca(OH)2 solution in the lab as well. Carefully (using a centrifuge) spin out ~12 mL, note the temperature from your thermometer and immediately draw off 10.00 mL of the solution, and place in a 125 mL flask. Process (read: add water, indicator, titrate, etc.) as with room T runs. You will only be doing one high T run.

Lab Report: Short form memo. Last one of term? Your goal, remember is to get ΔHş and ΔSş of a chemical reaction, so you best include that equation in your report.

Pre-lab Question (worth 5 points):

Consider the solubility of Sr(OH)2 as given below. Two solutions of Sr(OH)2 are allowed to equilibrate: one at 0 °C and the other at 25 °C. A 10.00 mL aliquot (a fancy term for 'portion') of each solution is titrated with 0.2000 M HCl. 3.37 mL of the acid are required for the 0 °C solution; 62.90 mL for the 25 °C solution. From this information, calculate the amount of hydroxide ion present originally from the Sr(OH)2. (VHCl → molHCl → molOH → [OH]) You can then determine the [Sr+2] in the original solution. You can then determine the value of Ksp for Sr(OH)2. Using ∆G = -RTlnKeq, you can calculate ∆G for the reaction at that temperature. Doing the whole calculation again for the other temperature will give another value of ∆G. The equation ∆G = ∆H - T∆S can be setup twice (once for each temperature) and the values of ΔH° and ΔS° for the reaction can be determined (2 equations, 2 unknowns) Box your final answers for ΔH° and ΔS°

~MEO 03.26.08