The lack of basicity within amide is due to the C=O, or carbonyl group, within the amide as it has electron withdrawing properties causing the lone pair of electrons within nitrogen to become delocalised. The Amide functional group is also a moderate Electron Donating Group (EDG), meaning that it donates some of its electron density to conjugated
Danielle Pitter CHEM 137 Professor D’Amelia 3/1/17 Extraction of a Neutral Compound from Acid and Base Impurities Discussion: The diethyl ether solvent is nonpolar; therefore, based on the expression like dissolves like, other nonpolar molecules will dissolve in it. The 9-fluorenone is a nonpolar molecule; therefore, it will dissolve in the nonpolar diethyl ether. The benzoic acid has a polar carboxyl group; however, the ring is nonpolar. The nonpolar ring in the benzoic acid is what makes it soluble in the diethyl ether. The ethyl-4-aminobenzoate is similar to benzoic acid, in that it has a nonpolar ring and has polar attachments.
My Citrate (CIT) result was turquoise so that meant the test was positive, and the Hydrogen Sulfide (H2S) had no black precipitate so it was negative. The Urea (URE) and Tryptophane Deaminase (TDA) results were both an orange color, which meant they were both negative. For Indole (IND), my result was yellow so it was negative. My result was colorless for the Voges Proskauer (VP) test so it was negative. The Gelatin (GEL) test result had no diffusion of pigment so that showed it was negative.
17.5% endodontists and 18.6% non-endodontists opted chlorhexidine as the irrigant with the best antimicrobial action. It has been suggested that chlorhexidine is sporostatic but not sporicidal 13, and is said to have a disadvantage of not dissolving organic tissue, and therefore cannot be considered as the irrigant with best antimicrobial action. Only 23.3% non-endodontists agree that sodium hypochlorite is the inevitable irrigant during root canal
This supports the isolated product is majority made of the desired product and is largely pure. Mass spectrometry of the crude product shows the molecular ion peak is 162.1, which is the largest fragment in the mass spectrum (Figure 4) and corresponds to the molecular weight of methyl trans-cinnamate (Table 1). The base peak is 131, inferring the fragment lost is 31 m/z in size. This 31 m/z matches the OCH3 fragment of the ester, and would not result from a trans-cinnamic acid. This is evidence the product was successfully
The Z product was a liquid, while the E product was a solid. The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.
As you can see from my sample that our aspirin sample contains a small amount of pure aspirin and a lot of salicylic acid. Therefore this means that my sample wasn’t pure as it still had remnants of salicylic acid which suggests to me that the reaction hadn’t been fully completed, however my sample did contain a small amount of pure aspirin which means that the reaction is partially had taken place. The sample would have been pure if there was no salicylic acid on the card then my sample would match the pure aspirin sample which means there would have been a fully completed reaction. 2. State what practical techniques used during the procedure and explain how they influence the purity of the sample.
The average equivalent mass for the acid is 135g/mol H+. 3. The answer obtained in Question #2 is the equivalent mass of the acid rather than the molar mass because the acid could be polyprotic, which would mean the equivalent mass is different from the molar mass since it is depending on moles of H+ per molecule, and there could be multiple moles of H+ ions in one mole of a molecule. 4. The KHP and the acid samples must be dried, because there would still be extra water which would skew the molarity.
The formula for sodium acetate is NaC2H3O2, it is quite soluble in water, soluble in ether and slightly soluble in ethyl alcohol. While the chemical compound melts at 622.8℉, it does not have a boiling point for it will decompose. A hydrate is a chemical compound that forms when one or more water molecules are added to the molecules of another substance. Since sodium acetate is a trihydrate (NaC2H3O2·3H2O), it has three molecules of water for every molecule of sodium acetate and because of this, anhydrous sodium acetate quickly transitions into a trihydrate. This is due to sodium acetate being quite hygroscopic, meaning it readily absorbs moisture from the air.