Pb+2 Separation of Pb+2 from Fe+3‚ Al+3‚ Cu+2‚ and Ca+2 Out the five cations in the mixture‚ only lead ion will precipitate‚ as PbCl2‚ when hydrochloric acid is added to the solution. Pb2+ (aq) + 2Cl- (aq) PbCl2 (s‚white) Equation 1 The solid PbCl2 is separated from the solution containing the
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Bunsen Burner 150 mm test tubes (14) 6.0 mol/L HCl Solid NaCl 0.50 mol/L NaCl 0.50 mol/L NaNO3 0.50 mol/L LiNO3 0.50 mol/L Sr(NO3)2 0.50 mol/L KNO3 0.50 mol/L Ba(NO3)2 0.50 mol/L Cu(NO3)2 0.50 mol/L Ca(NO3)2 0.50 mol/L Ni(NO3)2 50 mL beaker Bunsen Burner lighter Procedure: See handout Flame Colours of Metal Ions Observations: Substance being tested Appearance Flame colour Solid NaCl White‚ grainy Orange NaCl Colourless solution Bright
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AP Chemistry 12/13/11 Round-Trip Copper Reactions Lab The purpose of this lab was to evaluate our skills of decanting a supernatant liquid without losing the solid and successful completion of a series of reactions. This was done through five chemical reactions involving copper. In this lab‚ elemental copper was put through five different chemical reactions in order to convert it into different compounds. By the end of the fifth reaction‚ the copper was back to its elemental state. In the
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naphthalene. Sublimation is the process when a solid evaporates from a warm surface and condenses as a solid on a cold surface. The crude naphthalene had a melting point range of 85°-90° C while the 35.4% yield of pure naphthalene had a melting point range of 70°-76° C. Recrystallization was used to purify the salicylic acid. Recrystallization is the process of dissolving the original solid in a hot solvent and then allowing the solution to cool to let the solid crystallize again. The crude salicylic
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Differentiate between boiling and evaporation. 6.If external pressure decreases ‚ what change will be seen in the boiling point of water? 7.List the various factors which affect the rate of evaporation of a liquid. 8.Give reasons: a) Two solids kept together do not intermix but two miscible liquids or gases intermix fast. b)Clothes dry faster on a dry windy day than on a humid day. c) We sweat more on a humid day than s hot dry day. d) We feel cold when a cologne is sprayed on our
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Cycloaddition product is 0.358g (maybe it was not completely dry when I weighted.) The % yield of Diels-Alder reaction is 99.4% For the hydrolysis: The theoretical yield of hydrolysis is 0.396g The experimental product yield is 0.28g (some solid left on the filter paper and some for the melting point measurement.) The % yield of hydrolysis is 70.7% Discussion: The cycloaddition of a conjugated diene and a dienophile‚ which is drove by forming new σ-bonds from π-electrons of the diene
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particles. These tiny particles move around in water when it is in its liquid form‚ but as the temperature gets lower these particles slow down and hardly move. When it gets cold enough they stick together and then what was once a liquid has now became a solid we all know as ice. Ice turns into water‚ back to a liquid‚ when the temperature of the ice cube is rising which cause the particles in the ice to move faster and is the converted into water. There are actually some things that cause ice to
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AgCl to form instead of the desired solid PbCl2. The mixture was then centrifuged in order to let the solid particles of the three ions to fall to the bottom. Another drop of HCl was added to test if the reaction had been completed. If the solution were to turn milky white again then it would’ve signaled an incomplete reaction between the cations and HCl. The next objective was to separate the lead(II) ion from the mixture. The test tube with all three solids precipitated at the bottom was heated
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were to be answered in experiment 2. The equation of this reaction is as follows (and is the same as that found in experiment 2):  During this experiment‚ we used recrystallization methods in order to help in the purification of the unknown solid‚ as well as drying and vacuum filtration. We then ground the unknown and combined it with different chemicals (such as acetanilide or phenacetin) and used the melting point ranges to determine the identity. We used the Mel-Temp method in order to measure
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VI: Conclusion: The melting point of a compound is the temperature at which the solid is in equilibrium with its liquid. A solid compound changes to a liquid when the molecules acquire enough energy to overcome intermolecular forces holding them together in an crystalline lattice structure. The melting point range is defined as the span of temperature from the point at which the crystals first begin to liquefy to the point at which the entire sample is liquid. This data can be tabulated experimentally
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