Titration Experiment

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Titration is used to determine the equivalence point of a reaction, or the point when the moles of acid are equal to the moles of base in a mixture. Titration is used to determine the concentration of an unknown solution by using an already known solution. This process is important because it is commonly in the medical field. For example, pharmacists use titration in the creation of drugs. In addition, doctors also titration when determining the concentration necessary to give their patients of different medicines. Without titration, doctors and pharmacists would not be able to treat patients.
Acids and bases can be recognized by their individual properties. According to the Arrhenius theory, an Arrhenius acid contains the hydrogen ion when dissolved in water. An Arrhenius base contains the hydroxide ion when dissolved in water. According to the Bronsted-Lowry theory, a Bronsted-Lowry acid is a proton, or hydrogen ion, donor, while a Bronsted-Lowry base is a proton acceptor. Acids are characterized by their sour taste, electrical conductivity, reaction with a base to form water and a salt,
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We predict that if we known the concentration of the acid, HCl, then we can determine the concentration of the base, NaOH because using the standardized NaOH solution, we will determine the concentration of acetic acid because hydrogen ions neutralize hydroxide ions. The experiment was conducted by using a buret and an indicator in order to be able to tell when the mixture had reached the equivalence point. Results showed that the concentration of acetic acid in vinegar can be determined by first calculating the average of the concentrations of the NaOH in three different trials, then replacing the HCl with vinegar to calculate the concentration of the acetic acid in the

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