Name: ____________________________________ Locker Number: ____________________________ CHEMISTRY 354-355 Experiment 2 SOLUBILITY 1. Part A. Solubility of Solid Compounds. Use your observations to complete the following table‚ rating each system as soluble‚ insoluble‚ or partially soluble. Organic Compound Benzophenone Water Methyl Alcohol Hexane Malonic acid Biphenyl 2. Considering the polarities of the compound and the solvent and the potential for hydrogen bonding‚ answer the
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range. Each group (I was with William Yung for this experiment) was tasked with testing one homogenate. The homogenate tested by our group was liquid spinach. Each team added HCl and NaOH to their homogenate. As we found out in our experiment‚ HCl was an acid so when added to the liquid spinach the pH lowered and NaOH‚ being a base‚ rose the pH level when added. The better the buffer the homogenate is‚ the less its pH changes
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General Chemistry II Lab (CHEM 1106) Determination of the Solubility Product Constant of a Salt Date Performed: March 1‚ 2011 INTRODUCTION If solid KHC4H4O6 is added to a beaker of water‚ the salt will begin to dissolve. The amount of solid diminishes‚ and the concentrations of K+(aq) and HC4H4O6-(aq) in the solution increase. When no KHC4H4O6 dissolves‚ the concentrations of K+(aq) and HC4H4O6-(aq) will not increase further and any additional KHC4H4O6 added after this point will remain
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BACKGROUND: Esterification is a reaction that combines an alcohol with an organic acid‚ with a water molecule is being taken out‚ and an ester is formed. A concentrated acid catalyst speeds up the esterification. In this experiment set up‚ sulphamic acid was used‚ as it is a solid acid and be added dry‚ without any water‚ which is a reactant in this experiment equilibrium. Esterification is a slow and reversible reaction. The equation for the reaction between an acid RCOOH and an alcohol RẬᶦ
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To hold the solution and mix the indicator and NAOH Burette To let me pour the HCL into the conical flask at a continuous rate Boss clamp To hold the burette Pipette sucker To pull up the chemicals Beakers To hold the chemicals into so they won’t spill Pipette To accurately measure out the 25 cm3 Measuring cylinder To accurately measure out the chemicals 50 cm3 of HCL To use in the experiment to see the concentrations 50 cm3 of NAOH To use in the experiment to see the concentrations
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between sucrose and water. 2. For solutes that are dissolved because of reaction with the solvent‚ write the balanced equation involved. Balanced Equation A C6H5OH + NaOH C6H5ONa + H2O D C6H5CHO + H2SO4 m-benzaldehyde sulfonic acid E C6H5CH2OH + H2SO4 C6H5CH2OH2+ + HSO4- G C6H5COOH + NaOH C6H5COONa + H2O C6H5COOH + NaHCO3 C6H5COONa + CO2 + H2O H C6H5NH2 + HCl → C6H5N+H3Cl- 3. On the basis of solubility behaviour‚ determine the best solvent to differentiate
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The first test performed was the Metal Hydroxide Test‚ wherein drops of 6 M NaOH were added dropwise to each tube until a precipitate was formed‚ or a total of 20 drops were administered. This process was repeated for each tube‚ with drops administered until a precipitate was visible. Drops were administered as follows:K+: 20 drops‚ Zn2+: 3 drops‚ Cu2+: 2 drops‚ Co2+: 2 drops 6 M NaOH added. The results were recorded following each cation‚ noting the color
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possible to extract the base from the mixture. Organic acids are highly soluble in aqueous NaOH. This reaction that the acid has with the dilute NaOH helps the acid compound be extracted from the mixture. We again used three 10 mL portions this time of NaOH. It is noted that after adding each portion‚ whether it was HCl or NaOH‚ the mixture was shaken for about five minutes‚ this helped the added HCl or NaOH mix thoroughly through out the mixture and react with the acid or base in the mixture. After
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Chemical Reactions Objective In this lab we took Fe(NO3)3 and NaOH and mixed 7 different mole ratios in graduated cylinders to determine what the mole ratio is. We also did the same thing with solutions of CuCl2 and Na3PO4. We determine the mole ratios by graphing the volume of reactant #1 vs. volume of precipitate for each reaction. Data Part 1.) Cylinder 1 2 3 4 5 6 7 Fe(NO3)3‚ 0.1 M‚ ml 5 10 12 15 17 20 24 NaOH‚ 0.1 M‚ ml 55 50 48 45 43 40 36 Fe:OH mole ratio 1:11
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10 Test Tube Mystery Introduction: The students were handed 10 test tubes with no identification. The students were supposed to design a method in determining what chemical was in each test tube. The list of chemicals is CuSO4‚ NH4Cl‚ NaOH‚ AgNO3‚ KI‚ H2SO4‚ NaBr‚ CaCl2‚ HCl‚ and Pb(NO3)2. The students are expected to determine the chemicals using physical properties‚ litmus paper‚ solubility‚ and the process of elimination. Physical properties‚ such as the color‚ can be determined by sight. Litmus
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