Change the units of your temperature to Kelvin. Educ. Thermodynamics_of_Solubility_Lab_Report.docx - Thermodynamics of Solubility of Potassium Nitrate Lab Report Abstract The problem posed by this, 1 out of 1 people found this document helpful, Thermodynamics of Solubility of Potassium Nitrate Lab Report, The problem posed by this experiment was how Ksp of potassium nitrate could be determined. Heat the solution again until the crystals just barely dissolve completely. Laboratory 10: Thermodynamics of Solubility, To determine the thermodynamic variable for the solubility of \(\ce{KNO_{3}}\). Purpose: To determine the thermodynamic quantities (H( and (S( for the solvation reaction of borax in water, by measuring the solubility product constant over the temperature range from 55 to15 (C. a. Thermodynamics of the Solubility of Borax Purpose: To determine the thermodynamic quantities H and S for the solvation reaction of borax in water, by measuring the solubility product constant over the temperature range from 55 to15 C. Na2B4O710H2O(s) 2Na \[\ce{K_{sp}} = \ce{[K^{+}]}\ce{[NO_{3}^{-}]} \label {2}\]. Avoid shock, heat and contact with combustible materials. The solution must be disposed of in the hazardous waste container. For each ionic compound, decide if the dissolution reaction is product-favored or not, and enter that information in the table. CAUTION: Potassium nitrate is a strong oxidizer and skin irritant. One very useful thermodynamic variable is G, the Gibbs free energy. Be sure to properly label your plot, including title. Title: Microsoft Word - Thermodynamics of the Solubility of Borax 2010 Author: We know the mass of potassium nitrate we added, so we need to calculate moles and then divide by the volume at the temperature we used. Thermodynamics of the Solubility of Potassium Nitrate, Thermodynamics of the Solubility of Potassium Nitrate.pdf, Thermodynamics of solubility of potassium nitrate lab report JP Denny.docx, Full Lab Report - Solubility and Thermodynamics of Potassium Nitrate, Portland State University • CHEMISTRY 227, Portland State University • CHEMISTRY 229, North Carolina State University • CHEMISTRY 104, Portland State University • CHEMISTRY 228, Portland State University • CHEMISTRY CHEM 229. 4. • Answer the pre-lab questions that appear at the end of this lab exercise. Chemistry Lab: Thermodynamics of KNO 3 p. 6 b. Solubility and Thermodynamics: An Introductory Experiment Robert G. Silberman View Author Information SUNY-Cortland, Cortland, NY 13045 Cite this: J. Chem. because solubility and Ksp are closely related. The mathematical relationship between the change in the Gibbs free energy, \(\Delta\)G and the solubility product, \(\ce{K_{sp}}\), as function of temperature is given in Equation 3, \[\Delta G =\; -RT\; ln K_{sp} \label{3}\], where \(\ce{R}\) is the ideal gas constant (8.314 \(\frac{J}{mol^{. When saturated solutions are prepared the volume of the resulting solution must be determined experimentally. experiment provided results of a enthalpy of formation of -454.74 kJ/mol, with a percent error of. Watch the recordings here on Youtube! Ksp is the solubility product of a salt and can be, used to solve for various unknown details of salts. Repeat the cycle (steps 6 and 7) until you have obtained at least five good data points. Equation 5 relates the overall change in Gibbs free energy, \(\Delta\)G, to the changes in \(\ce{K_{sp}}\) as given in Equation 3. Potassium nitrate is a highly soluble compound (large \(\ce{K_{sp}}\)) compared to other insoluble compounds that you have studied. The equation will have the form of the linear relationship y = mx + b, where m is the slope of the line, –(DH°/R), and b is the y- intercept (DS°/R). 1. Record the temperature at which the crystals first are visible in the solution. Have questions or comments? Course Hero is not sponsored or endorsed by any college or university. Y = –654.31 x + 2.1295 R2 = 0.9952 c. Calculate ΔH and ΔS. Pre-Lab Questions. You will determine three thermodynamic values associated with the solubility of potassium nitrate. Cool slowly while stirring. 10-2 The Thermodynamics of the Solubility of Borax This equation can be studied by constructing a graph where y = ln K and x = (1/T). Using Excel or some spreadsheet application: Calculate the concentration of the ions at equilibrium; \(\ce{[K^{+}]}\) and \(\ce{[NO_{3}^{-}]}\). For instance if the data of ln(Ksp) vs. 1/T was plotted for the molecule the line would have a positive slope. In this experiment you will obtain the thermodynamic values \(\Delta\)G, \(\Delta\)H, and \(\Delta\)S, associated with the solubility of \(\ce{KNO_{3}}\).

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