1. What can you conclude if your dry aspirin sample has a lower melting point than the literature value? The presence of impurities generally decreases the melting point. The lower melting point than literature value indicates that the aspirin sample contains impurities. 2. If the yield of your dry aspirin is greater than 100%, what must you do experimentally to obtain a more reasonable yield? To obtain reasonable yield we can do either recrystallization or column chromatography. By doing the impurities in the sample can be removed, 3. Would the product isolated after Part A. 3 have a higher or lower melting point than that isolated after Part A 5? 4. If the endpoint is surpassed in the analysis of the aspirin sample in Part B. will its percent purity be reported too high or too low? Explain 1
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Preparation of aspirin day 1 1. Mass of salicylic acid (g) 2. Mass of filter paper (g) 3. Mass of dried filter paper plus sample (g) 4. Theoretical yield of aspirin (g) 5. Experimental (actual) yield of aspirin (g) 6. Volume of water used in experiment 7. Mass of aspirin dissolved in the experiment 8. Experimental yield, corrected for solubility (g) 9. Percent yield show calculations for the theoretical yield and the actual yield of aspirin here. Label each and circle your answers.
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Oxides can react with water to form acids or bases. Identify each of the following oxides as acidic or basic. Write the chemical formula of and give the name of the acid (include 'acid') or base formed upon reaction with water.
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Oxides can react with water to form acids or bases. Identify each of the following oxides as acidic or basic.
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For a mixture of 0.0786 mol of C2H4 and 0.1214 mol of CO2 in a 700.0-cm3 container at 40°C, calculate the pressure using (a) the ideal-gas equation; (b) the van der Waals equation, data in Table 8.1, and the C2H4 critical data Tc = 282.4 K, Pc = 49.7 atm; (c) the experimental compression factor Z = 0.9689.
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