The goal of the experiment that was conducted was to figure out both the molar concentration of NaOH and the standard mole ratio of the NaOH solution. In order to find the concentration of the NaOH solution‚ volumetric analysis was used. In volumetric analysis‚ a titration mechanism was utilized in order to find the reaction that the base will end up having with KHC8H4O4.‚ also known as KHP. Phenolphthalein‚ which is the indicator that was used in this experiment‚ assisted in figuring out at
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the particular substance in enough water to make a 1L solution. Monoprotic: HCL + NaOH H2O + NaCl Diprotic: H2SO4 + NaOH H2O + Na2SO4 N = __EW__ L EW= molar mass L = number of titratable protons To perform an acid-base neutralization using the titration technique to determine the concentration (normality) of the NaOH prepared in part A. C8H5O4K + NaOH H2O + KC8H4O4Na KHP: KHC8H4O4 *Acid base indicator- substances that have different colors in acidic and
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Standardization of a base (NaOH) using a primary standard (KHP) Standardization of an acid (HCL) with the standard base Titration analysis of unknown acids and bases (antacid tablets) Standardization of NaOH Materials: -Buret -250 mL Erlenmeyer flask -0.1 M NaOH -0.8 g KHP -Water -Three 150 mL beakers -magnetic stirrer A buret was rinsed with water and then with a small amount of the NaOH solution. Then the buret was filled with NaOH. The initial volume was read and
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undergoing a reaction with sodium hydroxide. Monoprotic: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Diprotic: H2SO4(aq) + 2 NaOH(aq) → 2 H2O(l) + Na2SO4(aq) Triprotic: H3PO4(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3PO4(aq) Any acid that has more than one proton that undergoes a reaction with a base is called a polyprotic acid. Citric acid is a weak‚ polyprotic acid that undergoes the following reaction with sodium hydroxide. H3C6H5O7(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3C6H5O7(aq) In this experiment you will be
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will be titrated to potassium hydrogen phthalate‚ solution and the second one is determining the molarity and percentage by mass of the acetic acid in vinegar. 6 g of NaOH solid is used to dilute with distilled water to prepare a 250 mL of 0.6M sodium hydroxide. pH electrode will be immersed into the solution and a grph of pH versus NaOH is obtained. The next part is to determine the molarity of acetic acid and mass percent in vinegar where the vinegar is diluted as the same way in previous part. The
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balance and hot plate. Preparation of 250 mL 1.0 M sodium hydroxide solution (from solid) The amount of NaOH needed to prepare 1.0M solution was calculated (10.0 g NaOH). The computed value was weighed using the top-loading balance and placed in a clean and dry 250-mL beaker. Enough amount of distilled water to dissolve the NaOH solid was added to the beaker and stirred. After the NaOH was completely dissolved‚ the solution was then transferred to a 250-mL volumetric flask quantitatively. Enough
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equilibrium between acids and bases during a titration can be used to determine several characteristics of the acid or the base. Sodium hydroxide was standardized to 0.1035 M in three acid-base titrations of potassium hydrogen phthalate (KHP). This standardized NaOH solution was then used in a series of other titrations with acids in order to gain information about those acids. The first acid tested was hydrochloric acid. This titration showed that the equivalence point occurred at a pH of 7.0. The
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of Na2CO3 through the preparation of NaOH and HCl standards. The molarity of the standards will be found through titration of KHP for NaOH‚ HCl vs the known NaOH‚ and the unknown Soda Ash sample vs the known HCl. II. Equations and Sample Calculations: Titration of HCl with NaOH: Complete Equation: HCl (aq) + NaOH (aq) H2O (l) + NaCl (aq) Net Ionic Equation: H+ + OH- H2O(l) Calculations (10mL 0.1M HCL‚ 100mL H20‚ 7.8mL NaOH): # mols NaOH = 0.1M (known concentration) x 0.0078L
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for this experiment was #14. The experiment began with the preparation and standardization of NaOH solution. It was calculated that 2.00 grams of NaOH pellets were needed to prepare 0.5 L of 0.1 M NaOH solution. The solution was then standardized by conducting three titration trials. It was calculated that 0.7148 grams of KHP were necessary to neutralize 35 mL of the 0.1 M NaOH. Three samples of KHP were weighed approximating this number (Table 1). Each sample was mixed with 40 mL of deionized
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instructor to dilute the 6M NaOH to 0.1M in 300mls instead of 500mls in Part B of Experiment 21. One objective for performing these two experiments was to observe qualitatively the reactions between common acids‚ bases‚ and the indicators phenolphthalein‚ methyl orange‚ bromothymol blue‚ and red cabbage extract. Another focus of this experiment was to perform a
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