TITLE: Solubility and Thermodynamics PURPOSE: The purpose of the lab was to determine the thermodynamics variables of ∆H‚ ∆S‚ and ∆G for the dissolution reaction of potassium nitrate in water. The solubility of potassium nitrate in mol/L was measured over a range of various temperatures by finding out at what temperature crystallization began for solutions of different molarities. Then‚ the equilibrium constant was calculated and a graphical relationship between the natural logarithm of the
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Marcela Rodriguez Ricardo Sarabia January 16‚ 2013 Mariana Mendoza Alvaro Puccini Maria Quin Solubility Lab Purpose: The main purpose of doing this lab is to learn how to interpret solubility graphs and how the temperature does affects the solubility of different substances. There are other objectives of the lab which are learning what are concentrated‚ diluted‚ supersaturated‚ and saturated substances and how can they be identified. The hypothesis
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general discussion of the solubility/miscibility behavior observed in procedure A-D. For part A of the procedure we worked with the solubility of solid compounds in various solvents. The three solid compounds that were worked with during this procedure were benzophenone‚ malonic acid‚ and biphenyl. These three solids were then mixed with water (highly polar)‚ methyl alcohol (intermediately polar)‚ and hexanes (nonpolar). When benzophenone is mixed with water the results turned out to be insoluble
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Precipitates are electrically uncharged. In this experiment all of the precipitates result from the exchange of positive and negative ions between reacting solutions of two ionic compounds. Thus‚ in this example the precipitate must be either silver chloride‚ AgCl or sodium nitrate‚ NaNO3. Sodium nitrate dissolves readily in water and is therefore soluble. Thus we can conclude that silver chloride is the insoluble precipitate. We can represent the formation of this precipitate by a net ionic equation:
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Week-2-Solubility Name: ___________________________________________________ Section: ______________ For Instructor Use Only POST-LAB REPORT FOR THE SOLUBILITY EXPERIMENT I) Conclusion: Write the conclusions regarding your observations and results obtained from each part 2A‚ 2B‚ 2C
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NH4Cl at 50oC. According to Table G‚ if the temperature is lowered to 10oC‚ what is the total amount of NH4Cl that will precipitate? (1) 5.0 g (2) 17 g (3) 30. g (4) 50. g Answer--> Choice 3; 52g-32g=30g 1/03 1 Solubility data for four different salts in water at 60oC are shown in the table below. Which salt is most soluble at 60oC? (1) A (2) B (3) C (4) D Answer--> Choice D =0.5g/g H2O 2 Base your answers on the information below
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RECRYSTALLIZATION OF ACETANILIDE ABSTRACT Recrystallization is the primary method for purifying solid organic compounds through the differences in solubility at different temperatures. In this experiment‚ a suitable solvent was first determined. Acetanilide was produced by acetylation of aniline with acetic anhydride. The crude acetanilide was dissolved in a solvent in a heating water bath. The hot solution was filtered and the filtrate‚ cooled slowly in an ice bath as crystals started forming
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laboratory is to calculate the solubility of a substance under a variety of temperatures and construct a solubility curve based on experimental data to see the effect of temperature on solubility. Data collection and quantitative observation VOLUME H2O/ml/±0.05 TEMPERATURE/°C/±0.1 5.00 71.3 6.00 59.3 7.00 52.4 8.00 47.2 9.00 41.8 Mass of NaCl: 3.0±0.05 g Data Processing To calculate the solubility‚ we need to use the formula: Solving for x‚ the solubility of salt‚ we get the formula:
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Separation of the Components of a Mixture General Chemistry 1 (Chem 101)‚ ISP SCUHS Report 2 January 26‚ 2014 Abstract The analyses of mixture were to distinguish and identify homogeneous mixture by using the techniques of decantation and sublimation. By performing these techniques‚ we examined our solutions such as SiO2 (sand)‚ NH4Cl (ammonium chloride)‚ and NaCl (sodium chloride) and mixed H2O (water) with each solution after being heated. After examining our solutions‚ we made calculations
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The Effect of Temperature on Solubility By Aviraj Singh Rogers 2 Background: The solubility of most solid substances is generally said to increase as the temperature of the solvent increases. However‚ some substances‚ such as ytterbium sulfate‚ do the opposite. This can be explained through the Second Law of Thermodynamics which states that “in all energy exchanges‚ if no energy enters or leaves the system‚ the potential energy of the state will always be less than that of the initial state”
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