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- Click ‘Get Form’ button to access the Solubility and Thermodynamics of Potassium Nitrate form and open it for completion.
- Begin by providing your name and the name of your lab partner in the appropriate fields at the top of the data sheets.
- Proceed to Table 1 and record the mass of KNO3 you will weigh out for your experiment. Ensure you note the actual mass recorded.
- In Table 1, fill out the moles of KNO3 by calculating them based on the mass you've recorded and the molecular weight of KNO3.
- Next, denote the total volume of KNO3 solution in Table 1, along with the temperature at which the first crystals appeared during observations.
- Update the molar concentrations of KNO3, K+, and NO3- in Table 1 post-calculations based on the experimental data gathered.
- Move to Table 2 to record the temperature in Kelvin and calculate the natural logarithm (ln) of Ksp for each trial. Ensure accuracy in your calculations.
- Complete Table 3 by calculating 1/T for each trial and determine the slope for the linear graph you will construct based on the lnKsp data.
- In Table 4, calculate and document the entropy change (ΔS) based on your findings from the graph and reference values.
- Once all sections have been completed, review your work thoroughly for accuracy, then save your changes and prepare to print, download, or share your form as necessary.
Complete your Solubility and Thermodynamics of Potassium Nitrate document online today for a smoother laboratory experience.
If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water. Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water.
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