Weak Acid Titration Abstract: Our method for determining the unknown weak acid was to determine the equilibrium constant K from the molecular weight of the weak acid from our titration data. In this lab the acid Potassium hydrogen phthalate and two unknown acids were titrated. We determined the molar mass of the Potassium hydrogen phthalate‚ for the unknown acids we calculated the molar mass and the Ka values. We used NaOH as the known base for titrating in all three of the titrations. Our ka
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Acid-Base Titration Objectives: 1. To titrate a hydrochloric acid solution of unknown concentration with standardized 0.10M sodium hydroxide. 2. To utilize the titration data to calculate the molarity of the hydrochloric acid. Materials: See handout for more info. Procedure: See handout for more info. Data and Calculations: Table 1: Volume of NaOH Required to Neutralize 10.00mL of Unknown HCl Molarity of NaOh | Trial 1 | Trial 2 | Trial 3 | Trial 4 | Initial Volume of NaOH(mL)
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Titration test Alfredo Verzo III We have been provided with two samples of vinegar‚ one removed from a restaurant and one removed from a take-away. Trading Standards suspect these two establishments of watering down the vinegar. They need evidence that the samples contain less acid than the standard vinegar sample provided. What is the purpose of this? I’m a worker in the Trading Standards which carries out tests to see if restaurants and takeaways are watering down the vinegar. We will
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An Introduction to Titration: Standardization of HCl and NaOH Lab Report Introduction: It is important to standardize solutions in order to have the accurate amount of concentration known. A standard solution can be prepared in either of two ways: A primary standard is carefully weighed‚ dissolved‚ and diluted accurately to a known volume. Its concentration can be calculated from this data. A solution is made to an approximate concentration and then standardized by titrating an accurately weighed
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experiment is to determine the concentration of acetic acid in vinegar by using 0.1 M HCl and NaOH solution. By performing three titrations to determine the concentration of the base‚ the concentration of the acid was determined to be 0.600 M. It was possible to determine its concentration by standardizing the sodium hydroxide solution used for the first three titrations and by using phenolphthalein to indicate its equivalence point. In conclusion‚ although there were sources of error‚ the hypothesis
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tion Experiment 1 Titration curves of amino acids General structure of amino acids (amphoteric type): Zwitter ion C * : α- carbon : α- amino acid NH2 : α- amino group‚ basic (proton acceptor) COOH : α- carboxylic group‚ acidic (proton donor) R : side chain of amino acid Classification of amino acids depending on the nature
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Lab 12: Titration of Acetic Acid in Vinegar Abstract: To lesarn how to titrate chemicals in a lab. Also to be able to determine the concentration of an acetic acid solution. Purpose: To learn how to titrate‚ and calulate the concentration of an acetiuc acid solution. In this case the concentration of vinegar‚ which is diluted acetic acid. Hypothesis: The sodium hydroxide used in this titration would balance out the acetic acid in vinegar. The phenolpthalein‚ a acid –base color indicator
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the 4 substances .titrate those to find how much vitamin the substances have. 27. To perform the titration take the pipette 20 mL of the sample solution into a 250 mL 28. Condition your buret and filled with titrant solution. You should check for air bubbles and leaks‚ before proceding with the titration. 29. Take an initial volume reading and record it in your notebook. Before beginning a titration‚ you should always calculate the expected endpoint volume. 30. Put paper on the top loading balance
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Chemistry: Strong Acid and Weak Base Titration Lab Cherno Okafor Mr. Huang SCH4U7 November 21st‚ 2012 Data Collection and Processing Concentration of the standard HCl solution: 0.1 M Data Collection: | Trial 1 | Trial 2 | Trial 3 | Final HCl Buret Reading ± 0.05 mL | 38.3 | 45 | 54.5 | Initial HCl Buret Reading ± 0.05 mL | 29.9 | 38.3 | 45 | Volume of NaHCO3 used ± 0.1 mL | 9.2 | 9.5 | 9.8 | Qualitative Data: * I used the
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Titration Lab of NaOH and KHP Aim: To titrate Sodium Hydroxide with Potassium Hydrogen Phthalate . To also determine the concentration of NaOH in the KHP solution. Hypothesis: When KHP is added to the solution of NaOH and the indicator‚ the solution will turn clear and neutralize. The concentration of NaOH is going to be very low because it is diluted. Materials required: pipette filler‚ volumetric flasks(2-4)‚ beakers(2)‚small white piece of paper‚ indicator( 2 drops)‚ conical flask‚ clamp
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