Data Table 1: Determination of KHT Saturation Temperatures Mass of Flask: 120.88 g Mass of Flask + KHT: 121.98 g Mass of
Posted: Fri Jul 15, 2022 4:44 pm
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 1 (45.56 KiB) Viewed 38 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 2 (37.71 KiB) Viewed 38 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 3 (68.66 KiB) Viewed 38 times
Data Table 2: Observation of the Common Ion Effect
Part 1: Determination of KHT Saturation Temperatures Be sure to show all calculations required, and don't forget proper units! 1. Refer back to the introduction of this lab and write down the two equations provided to solve for ΔG. 2. Set the two equations equal to each other and isolate In Ksq on one side of the equals sign by dividing both sides by (-RT). 3. Create a graph using Excel plotting lnKsp on the y-axis and 1/T (make sure the units for temperature are Kelvin) on the x-axis. a. Use the value obtained for the s.'spe of the graph to solve for ΔH∘ using the equation derived in Question 2. b. Use the value obtained for the y-intercept of the graph to solve for ΔS∘ using the equation derived in Question 2. 4. Calculate ΔG∘ at 298 K using the equation provided in the introduction - this represents the free energy associated with dissolving KHT in water at 25∘C. 5. To calculate the standard enthalpy change of a reaction (ΔHrxn∗) for the process KHT(s)⇌KHT(aq) the following equation can be used: ΔHrxn∘=∑ΔHf∘( products )−∑ΔHf∘ (reactants) Given the following information, calculate ΔHrxn′′ and compare to the experimentally obtained value (Question 3a). Calculate the percent error between the theoretical and experimental values. ΔHf∘ of KHT(s)=−1545 kJ/molΔHf∘ of KHT(aq)=−1497 kJ/mol