The first experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 21°C. In order to determine these values, the experimental data as well as the chemical reaction of calcium hydroxide was used. The molarity of OH- and Ca2+ was discovered to be 0.028 M and 0.014 M respectively. The Ksp was found to be 1.144 x 10-5 and ΔG was discovered to be 27.470 KJ/ mol. The second experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 60°C. The molarity of OH- and Ca2+ was discovered to be 0.029 M and 0.014 M respectively. The Ksp was found to be 1.316 x 10-5 and ΔG was discovered to be …show more content…
The ΔG is our y-value, the T is our x value and therefore the slope of the line acts as the entropy of the calcium hydroxide and the y-intercept of the line acts as our enthalpy. Based upon literature values, entropy for calcium hydroxide is 83.4 J/K mol and if entropy is converted to the correct units, this displays a value of 119.3 J/K mol (Thermodynamic quantities for substances and ions at 25˚C). Possible explanations for a greater experimental data value than true value will be discussed the Conclusions section of this report. Based on the literature values, enthalpy for calcium hydroxide is -986.1 KJ/ mol (Thermodynamic quantities for substances and ions at 25˚C). The value appears to be off by a factor of 100 according to experimental data value of entropy which is -7.9384 KJ/ mol. Possible explanations for a significantly lower experimental data value than true value will be discussed in the Conclusions section of this