Richard Romero October 01, 2019Standardization of NaOH DrafAbstractThe purpose of this experiment is to standardize a solution of NaOH by accurately and precisely determining the concentration used in a titration with Potassium Acid Phthalate. Some techniques include using titrations as well as phenolphthalein as our indicator to tell us when to stop titrating the solution as it is standardized. Overall, found that the concentration that was standardized from a sample of NaOH and KHP was relatively close in concentrations of all 4 successful titrations with the RSD of 2.7 %, aiming for less than 3% which is how precise the concentration was. The average found was 0.1155 M with a percent error of 2.1%. IntroductionThe purpose of this experiment is to standardize a solution of NaOH by accurately and precisely recording the concentration used in a titration. The reaction studied was Potassium Acid Phthalate (KHP) and NaOH to make H2O and NaOH, as shown in equation (1) below. KHPwas used as the acid to standardize the solution. KHC8H4O4 (aq) + NaOH (aq) NaKC8H4O4(aq) + H2O (l)Using KHP was a good choice because when measuring out the solid it is easier to get a better measurement with a solid than a liquid. Also, KHP has a 1:1 mole ratio with NaOH as shown in equation (1). With a mole ratio of 1:1, it is easier to convert from one chemical substance to another. When distinguishing between which indictor to use, it is important to show a clear distinction of when the solution is standardizing. Phenolphthalein will change to pink at a pH of 8, to make a titration you need an indicator to help tell you when the solution
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concentration is met. After recording three good trials of the titration, the amount of KHP (g) andthe volume of NaOH titrated into KHP (mL), along with the final concentration of that trial will be used to calculate the NaOH concentration using equation (2) below After the solution is
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