Acid Base Titration bre’ana March 1‚ 2013 Purpose: The purpose of this experiment is to determine the concentration of a solution of NaOH by titration with a standard solution of HCl. It was also the purpose to determine the concentration of a sample of white vinegar by titration with a standard solution of NaOH. Introduction: Using the method of titration is how the experiment gets to the conclusion of the concentration of a solution. When doing this experiment‚ measurement is very important
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Acid/ Base Titration Lab Design III Materials: Goggles HCl NaOH Distilled Water Label Beaker Graduated Cylinder Pipet Stirring rod Buret with clamp Stopper Ring Stand Utility Clamp Computer Computer Program pH probe Procedure: 1) 2) Goggles were put on. 3) 0.1 M NaOH solution was made using 0.4 g NaOH and 100 mL distilled water. The ingredients were added together in a beaker and stirred. 4) The buret was standardized by adding 10 mL of distilled water‚ rolling
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electrolytes such as NaOH‚ HCl‚ and HNO3 completely dissociate into its component ions in aqueous solutions where else weak electrolytes such as phenol only partially dissociates into ions in aqueous solutions. (Daintith‚ 2010). Experimental Procedure The experimental procedure used for this experiment was outlined in the CHEM 120L lab manual‚ Experiment #4. All steps were followed without deviation (Dept. of Chemistry‚ 2013). Experimental Observation Part A: Neutralization of NaOH with HCL Concentrations
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t Design and preparation of buffers effective at different pHs Abstract These experiments aimed to determine the optimum pH ranges various buffers are effective and provide opportunity for the use of the Henderson-Hasselbalch equation to prepare a buffer of a specific pH. Three different buffer systems were initially investigated; volumes of weak acid and weak bases of specified concentration were prepared and titrated against strong acid or strong base solutions with pH readings taken at frequent
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Acid/Base pH 0.1 M HCl (aq) 0.1 M HC2H3O2 (aq) 0.1 M NaOH (aq) 0.1 M NH3 (aq) Question 1. Both acids above have the same concentration‚ 0.1 M‚ but they exhibit different pH value. Explain. Question 2. Both bases above have the same concentration‚ 0.1 M‚ but pH of NH3(aq) is lower than that of NaOH. Explain. 7 III. a) Observation of HCl/NaOH product. b) Identity of the product: c) Write the reaction occurred between HCl and NaOH. __________________________________________________________________________
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Determining the Unknown Concentration of NaHCO3 (aq) Through Titration Introduction Titration is the accurate addition of a titrant- solution in a burette- into a measured volume of a sample (Kessel‚ 2003). There are many different types of titration‚ such as acid-base reaction‚ redox reactions‚ precipitation reaction and more (Dohrman). In this lab an acid base titration will be explored. In an acid-base titration‚ the concentration of an acid or base is unknown and is determined by the adding
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Table 1: Data Collection Table – Contains all of the primary data directly obtained from the lab. Indicator | Initial volume of NaOH in burette (ml) ±0.05 | Final Volume of NaOH in burette (ml) ±0.05 | Final – initial Burette Reading (Volume of NaOH used) (ml) ±0.1 | Qualitative Observations | Phenolphthalein | 0.00 | 0.90 | 0.9 | At first when the base was being dropped into the vinegar there wasn’t a color change‚ however when the solutions came close to full titration‚ the solution
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CH3COOH + NaOH >> CH3COONa + H2O Concentration of NaOH = 0.25mol/0.25L = 1.0 mol/L Mols of NaOH = 1.0(0.25) = 0.25 mol Great Value Mol of NaoH = Mol Of Vinegar Mol NaOH = 1.0(0.087) = 0.087mol 0.087 = mol of vinegar Concentration of vinegar = 0.087/0.10 = 0.87 Mol/L No Name Mol of NaoH = Mol Of Vinegar Mol NaOH = 1.0(0.085) = 0.085mol 0.085 = mol of vinegar Concentration of vinegar = 0.085/0.10 = 0.85 Mol/L Heinz Mol of NaoH = Mol Of Vinegar Mol NaOH = 1.0(0
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Stoichiometry February 28th‚ 2013 Abstract: The reactions of the Sodium Hydroxide and two acids‚ Hydrochloric Acid and Sulfuric Acid were performed. The heat given off by these two reactions was used to determine the stoichiometric ratio and the limiting reactants in each experiment. Introduction: Coefficients in a balanced equations show how many moles of each reactant is needed to react with each other and how many moles of each product that will be formed. Stoichiometry allows us to
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to carry out the liquid-liquid extraction. The studies is to determine the average time travel for each of the 10 out of 50 water droplets from top of the burette and to the bottom‚ the average volume of each of the water droplet and the volume of NaOH needed to neutralise the benzoic acid in aqueous solution. From the volume collected for 50 droplets surface area and radius is calculated for a droplet. The uses of the surfaces area and volume help to determined the concentration of benzoic acid
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