Essay On Titrating Vinegar With Sodium Hydroxide

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Titrating Vinegar with Sodium Hydroxide (NaOH)
Introduction
Acids are anions that have at least one hydrogen cation tacked onto their molecular formulas. The Bronsted definition of an acid states that acid is a proton, H+, donor.3 Acids can fall into one of two categories: they can be strong or weak. Strong acids completely dissociate their H+ and weak acids only partially dissociate their H+.3 This means that a strong acid cannot return to its initial state once it undergoes a reaction. On the other hand, a weak acid can return to its initial state. Bases are cations that have a hydroxide anion added into their molecular formulas. Bronsted defined bases as a proton acceptor.3 Just like acids, bases can be either strong or weak. Strong bases completely dissociate their OH- after a reaction and weak based only partially dissociate their OH-.3 Meaning strong bases cannot return to their initial state, yet weak bases can return to their initial state. Vinegar, common in
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That proton, then, becomes a part of the base. This reaction is known as neutralization. When an acid or base are neutralized, its pH level goes to 7 or neutral. On the pH scale, acids range from 1-6 and bases range from 8-14. An example of neutralization is when one mole of HCl and one mole NaOH are mixed to make table salt and water. The pH of water is 7, but salt does not have a pH and does not interact with water molecules.3 Therefore, the pH of the solution is 7, or neutral. To determine how much of a base is required to neutralize an acid, acid-base titration is used. A titration measures how much of a substance, titrant, with a known concentration is required to react completely with a substance, analyte, with a known volume.4 This is known as the equivalence point. Once the volume of the titrant is found, the concentration of the analyte can be determined

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