until they have just reacted entirely. This method is recognized as performing a titration. In general‚ the features of acid-base titrations has one of the
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0.01 g Volume of HCl added = 50.00 ± 0.5 〖cm〗^3 Volume of solution = 250.0 ± 0.3 〖cm〗^3 Volume of NaOH pipetted = 25.00 ± 0.03 〖cm〗^3 Titration number Rough 1 2 Initial burette reading of NaOH/ ± 0.05 cm3 0.00 0.00 0.00 Final burette reading of NaOH / ± 0.05 cm3 11.80 11.70 11.20 Volume of NaOH titrated / ± 0.10 cm3 11.80 11.70 11.20 Titration table: data collected from burette of amount of HCl used for the colour of the solution with methyl orange to change Qualitative observation
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Complexometric Titration Topics to be discussed: • Complex ions & ligands. • EDTA in complexometric titration. • Indicators for complexometric titration. • Titration curve • Application of complexometric titration. 1 Complexometric titration method • An analytical method involving complex formation reactions. • A complex ion (or coordinate complex) is formed from electron donating compound & a metal ion. 2 Coordination Complex • The electron donating compound is a neutral organic molecule
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| |brand of green tea sample |volume of green tea sample used to |volume of DCPIP solutions |titrate boiling water with DCPIP | | |reach the endpoint of titration of |time to brew the tea bag sample |solution. | | |DCPIP solution and green tea sample |mass of tea bag sample |
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Project Report - Determination of the Dosage of Bleaching Powder Required for Sterilization of Different Samples of Water CONTENTS 1. INTRODUCTION 2. GENERAL METHODS USED 3. THEORY 4. REQUIREMENTS 5. PROCEDURE 6. OBSERVATION TABLES 7. CALCULATIONS 8. RESULT 9. CONCLUSION INTRODUCTION Water is the major constituent of all living beings. Water necessary to sustain all types of life. The water used for drinking purpose by human beings should full the following
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after each titre. For example‚ the volume used in the first titre would be calculated by: 25-21.3=3.7 mL Uncertainty: (Uncertainty of the previous volume + uncertainty of volume after titration) = (0.05+0.05) =0.1mL Calculating the rest of the titres in a similar fashion (previous volume-volume after titration) the following table of results is obtained: Table 3: Table of the volume of 0.201moldm-3 sodium hydroxide (NaOH) used to titrate 25mL (±0.03mL) of unknown acid X in mL
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Apparatus: Safety spectacles Weighing bottle Balance capable of weighing to within 0.01g Spatula Stirring rod with rubber end Dropping pipette Wash bottle of distilled water Funnel Volumetric flask‚ 250 cm3 Beaker‚ 250 cm3 Retort stand Burette clamp Burette‚ 50cm3 Pipette‚ 25cm3 Pipette filler Beaker‚ 100cm3 White tile Conical flask‚ 250cm3 Reagents used: Distilled Water Hydrated Sodium Borate 1.0 M Hydrochloric acid Screened methyl orange Sodium Borate solution
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5ml of Tropicana fruit juice and 25ml of oxalic acid prepared in a boiling tube was heated at 80oC for 5 minutes in a hot water bath. The solution is then titrated with DCPIP solution from orange to pink color. The volume of DCPIP needed for the titration process was recorded. The experiment is then repeated using time interval 20minutes‚ 35minutes‚ 50 minutes‚ and the volume of DCPIP needed to reach end-point is recorded. The concentration of Vitamin C is 0.48 mg cm- 3 at 0 minute‚ 0.48 mg cm-3 at
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this the experiment was split into two parts; part A and Part B. in Part A of the experiment a standardized 0.05 M solution of HCl was titrated into a 25 mL solution of saturated Ca(OH)2 which contained 2 drops of orange methyl identifier. Once the titration began‚ the HCl was added until the methyl orange endpoint was reached‚ and as a result the volume of the HCl needed for the endpoint to be reached could be used in determining the moles and in turn the molar solubility and the solubility constant
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value was rejected because experimental errors are never to exceed theoretical values‚ which are taken on assumption that the experiment is carried out in entirely ideal environmental settings‚ which are impossible to attain entirely. In 4B‚ redox titrations were used to calculate the relative composition of oxalate within the iron (III) oxalate salt. The millimoles of oxalate were found to be.64#‚ .63#‚ .62#‚ and .62#‚ for trials A-D‚ respectively. The weight percentages for each trial (A-D) were
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