This experiment investigated the following research question: "How does hydrogen bonding change in a solvent like Propanone, which is a Polar Aprotic solvent and water, a polar solvent are added separately into pure Alpha Hydroxy compounds like Glycerol, Ethylene Glycol, and Propylene Glycol by measuring the ΔH (Change in Enthalpy) changes by Calorimetry?”
Aprotic solvents may have hydrogen atoms in the compound, yet they need O-H or N-H bonds, and along these lines, they are unable to frame hydrogen bonds with themselves.These solvents have expansive dielectric constants (>20) and substantial dipole movements, however, they don't take part in hydrogen bonding (no O-H or N-H bonds). Their high polarity enables them to break down charged species, for example, different anions utilized as nucleophiles (e.g. CN(- ), HO(- ), and so forth.). The absence of hydrogen holding in the dissolvable implies that these nucleophiles are generally "free" in the solution, making them more responsive to the reactions. For our purpose, these solvents don't partake in the reaction.
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Moreover, these O-H or N-H bonds can fill in as a wellspring of protons.In addition, polar protic solvents have a tendency to have high dielectric constants and high dipole movements. Moreover, since they have O-H or N-H bonds, they can likewise participate in hydrogen bonding. These solvents can likewise fill in as acids (a source of protons) and weak nucleophiles (framing bonds with solid electrophiles).They are most usually utilized as the dissolvable for their conjugate bases. (e.g. H2O is utilized as