Irresistible? By Mikayla Messing 8/3/12 Section 623 Abstract To examine the effectiveness of buffers by titrating two sets of five different solutions using HCl and NaOH and monitoring the pH change of the various solutions. The data collected shows that the buffer systems made with sodium acetate and acetic acid were effect when titrated with the strong acid and the strong base. Comparison of all the solutions shows that the concepts of buffers holds true for the results from the experimentation
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prepared by a process known as saponification. Historically‚ soaps were made by boiling the fat of animal‚ lye and in a aqueous NaOH and KOH solution containing potash. Of course‚ this was done long time ago before anyone had any idea of understanding the chemical transformations. Now‚ we know that this process is a reaction of esters with a strong base such as KOH or NaOH. The esters‚ triglycerides are the main constituents of vegetable oil and animal fats. The triglyceride is a tri-ester come along
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Solution Abstract The aim of the experiment was how to determine the molarity of a solution. My hypothesis was if I have to determine the molarity of a NaOH solution‚ then I would have to use a standard solution of HCl solution because I would need to neutralize each other to determine the concentration of the solution of NaOH. The method that I used for this experiment was titration. Titration helped me achieved the result on figuring out the unknown molarity of the solution. Throughout
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equivalent point for the titration HCl-NaOH the pH is 7‚ which mans that is neutral‚ in other words there are enough NaOH mmol to neutralize the HCl mmol present; also‚ the solution contains only water and NaCl the salt derived from the titration made. On the other hand‚ at the equivalent point for the titration acetic acid-NaOH the pH is 8.67; consequently is more basic. This is something that it was expected because for a weak monoprotic acid (acetic acid)-strong base (NaOH) titration the pH at equivalence
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Standardization of Solution and Titration Lab Report‚ Preparing a Dilute HCl Solution from a Concentrated One Titrating NAOH Solution with HCl Solution (of Known Concentration) Chemistry lab report(by abdazino abdalla) International College Objective preparing a dilute HCl solution from a concentrated one titrating NAOH solution with HCl solution (of known concentration) Procedure Section A: Preparation of 100.0cm3 0.480 mol/dm3 HCl solution a)Determine the volume of the concentrated acid
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acids needed more drops of NaOH to reach its equilibrium then the less concentrated acids. Introduction Sodium Hydroxide (NaOH) is a strong base and when it is titrated with a strong acid the equivalence point will be expected to be a pH of 7 (wyzant.com‚ Feb. 12). NaOH is also known as caustic soda‚ it is soluble in water‚ ethanol‚ and glycerol but is insoluble in acetone and ether (nap.edu‚ Feb. 12). When Phenolphthalein a weak acid and when hydroxide ions (NaOH) is added the indicator is turned
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9.5 – 5.0 = 4.5. Therefore 4.5 mL of NaOH was needed to neutralize HCl. Table 3: The amount of NaOH (mL) needed to neutralize HCl in Condition 1‚ 2 ‚ and 3 and their 3 trials. Trial 1 (mL) Trial 2 (mL) Trial 3 (mL) Condition 1 4.5 4.0 4.0 Condition 2 8.0 8.0 9.0 Condition 3 9.5 9.0 9.5 2. Sample Average Calculation of Condition 1: Table 4: The average volume (mL) of HCl & NaOH in each Condition Average Volume of HCl & NaOH Condition 1 9.2 Condition 2 16.5
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dye with the chemical formula C25H30N3Cl and disassociates completely in solution. The relevant structure for this compound can be seen in figure 1 Figure 1 The base that is being used for the reaction is the strong base Sodium Hydroxide‚ or NaOH. This molecule also completely disassociates in water. Because measuring the concentrations of reactants is difficult in a simple lab setting‚ the reaction between Crystal Violet and Sodium Hydroxide will be measured through light absorbance. As
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in a commercial vinegar using titration method. Chemical reaction involved: CH3COOH(aq) + NaOH(aq)→ NaCH3COO(aq) + H2O(l) Apparatus: An electronic balance‚ a 10.0cm3 pipette‚ a 25.0cm3 pipette‚ a pipette filler‚ a 250.0cm3 volumetric flask‚ a burette‚ stand and clamp‚ a conical flask‚ a white tile‚ 3 large beakers‚ a small beaker‚ a dropper‚ a boiling tube‚ a rinsing bottle Chemicals: 0.1M NaOH(aq)‚phenolphthalein indicator‚ commercial vinegar (5% acidity)‚ distilled water Procedures:
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Titration for Acetic Acid in Vinegar Purpose: The Primary Purpose of this Experiment is to Determine the Percent Content of Acetic Acid in a Household Bottle of President’s Choice Vinegar‚ using Titration Techniques. In addition‚ a Secondary Purpose for this Experiment that Derives Directly from the Primary Purpose is to Gain Hands On Experience in Titration Techniques‚ as a Vital Tool in our Quest to Understanding the Chemical Aspect of the World around Us. Procedure Conducting a Titration
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