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Acid Base TitrationsIntroductionMultiple titrations, of which involve acid-base reactions, are to be performed in this experiment. In the first portion, the titration is for the standardization of NaOH and the second portion titration is for the standardization of HCl. KHP will be used as the primary standard in the standardization of NaOH. Titrations will involve observing the end point, which can be observed by the color change in the solution due to the addition of the phenolphthalein indicator. What to look for will be a very pale pink rather than a “South Beach” pink, or hot pink. Also, thesolutions formed in this experiment will be used in the next lab.Theory and ConceptsA titration is a type of volumetric analysis and depends on addition of a known volume ofsolution. The reaction shows strong changes in pH near the equivalence point while at the end point, the millimoles of base is equal to the millimoles of acid. The concentration of diluted NaOH solution in this experiment must be found exact to four significant figures in a process known as standardization. This process can be completed using a primary standard that must be of high purity, known composition, and reacts with a known stoichiometry. To determine the molarity of NaOH, a reaction will be performed betweenthe diluted NaOH and the primary standard potassium acid phthalate, abbreviated KHP. The reaction in the standardization of NaOH is:K+[HC8H4O4]-+ Na+OH-(aq) K+Na+[C8H4O4]-2(aq) + H2O(l)The reaction in the standardization of HCl is:HCl (aq) + NaOH (aq) NaCl (aq) + H2O(l)Solution concentrations are normally expressed in units of molarity, which corresponds toone mole of substance per one liter of solution. In this experiment, they will be expressed a smaller form of the unit as millimoles per milliliters.