I have a lab report to write on an experiment titled Thermodynamics of a compound. We titrated 10ml of Ca(OH)2 with 8.7 ml 0.1M HCl at room temperature. Then we heated (to boiling) a different batch and performed three titrations that took an average 0f 2.0ml HCl. We are supposed to figures out the concentrations of Ca and OH and get the ksp to use in deltaG =-RTlnKsp. We will use the room temp of 293.7K and a second time with the heated temp of 373K. Eventually we are to find entropy and gibbs free energy but I am still stuck at finding ksp. I know that the moles of hydroxide are twice the calcium .I figured the moles of HCl to be 0.0087Lx 0.1M = 0.00087 and thus equal to the moles of base at equivalence point so do I divide by 2 or multiply by 2 to get [Ca] [OH]2 to get ksp. And then I think there is another step in there. Do I use the volume of base somewhere?
I have a lab report to write on an experiment titled Thermodynamics of a compound. We titrated 10ml of Ca(OH)2 with 8.7 ml 0.1M HCl at room temperature. Then we heated (to boiling) a different batch and performed three titrations that took an average 0f 2.0ml HCl. We are supposed to figures out the concentrations of Ca and OH and get the ksp to use in deltaG =-RTlnKsp. We will use the room temp of 293.7K and a second time with the heated temp of 373K. Eventually we are to find entropy and gibbs free energy but I am still stuck at finding ksp. I know that the moles of hydroxide are twice the calcium .I figured the moles of HCl to be 0.0087Lx 0.1M = 0.00087 and thus equal to the moles of base at equivalence point so do I divide by 2 or multiply by 2 to get [Ca] [OH]2 to get ksp. And then I think there is another step in there. Do I use the volume of base somewhere?
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