the pH of the reaction with the use of a color indicator. We also learn about the standardization of bases (NaOH) and acids (HCl) which is basically making a dilution to change the molarity. The first reaction consists of titrating sodium hydroxide (NaOH) into potassium acid phthalate (KHP or K[HC8H4O4]): K+[HC8H4O4]- + Na+OH- => K+Na+[HC8H4O4]- + H2O The second titration we did was hydrochloric acid (HCl) with sodium hydroxide (NaOH): HCl(aq) + NaOH(aq) => NaCl(aq) + H2O(l) Procedure: You need
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and Johnson A.R.‚ Biochemistry and Methodology of Lipids. John Wiley and Sons‚ Inc. 1971. [9]Analysis of Lipids [10] Ghatak‚ K.L. Techniques and Methods in Biology. PHI Learning Private Limited:New Delhi. 2011 [14] Saponification [15] High Quality Sodium Hydroxide and Potassium Hydroxide for Making Soap. http://www.certified-lye.com/lye-soap.html. (accessed Feb 27‚ 2013). [16] Fatty Acid Composition and Properties of Oils Chart. http://thesoapdish.com/oil-properties-chart.htm (accessed Feb 27‚ 2013)
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The overall objective of this experiment is to determine the mass percent of NaClO‚ sodium chloride‚ in standard bleach. The purpose of part 1‚ is to standardize Sodium Thisulfate‚ Na2S2O3‚ with the primary standard Potassium Iodate‚ KIO3. The standardized Na2S2O3 will then be used in Part 2‚ to help determine the mass percentage of sodium chloride in bleach. The chemical equation used in standardizing sodium thisulfate is‚ IO3- (aq) + 5I- (aq) + 6H+(aq) ---> 3I2 + 3H2O followed by I2 (aq) +
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HEALTH THE BHOPAL DISASTER Ashay Chitre‚ a film maker living in Bhopal’s prestigious Bharat Bhawan‚ built by the state government to attract artists to this central Indian city‚ heard a commotion outside his window early in the morning at about 3 a m. It was a chill December and all the windows of Chitre’s house were closed. As Chitre and his wife Rohini‚ seven months pregnant‚ opened the window‚ they got a whiff of gas. They immediately felt breathless and their eyes and noses began to
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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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Acid-Base Titration Pre-Lab Discussion In the chemistry laboratory‚ it is sometimes necessary to experimentally determine the concentration of an acid solution or a base solution. A procedure for making this kind of determination is called an acid-base titration. In this procedure‚ a solution of known concentration‚ called the standard solution‚ is used to neutralize a precisely measured volume of the solution of unknown concentration to which one or two drops of an appropriate acid-base
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Δ(Product) Δ(Time) http://www.one-school.net/notes.html Rate of Reaction = 1 Δ(Product) Δ(Time) ONE-SCHOOL.NET Chemical Reaction Precipitation of Sulphur 2HCl(aq) + Na2S2O3(aq) ⎯→ 2NaCl(aq) + S(s) + SO2(g) + H2O(l) Na2S2O3: Sodium thiosulphate Notes: 1. Yellow precipitate (sulphur) is formed. 2. The reaction is slow. Potassium Dichromate (VI) with Ethanedioic Acid Cr2O72- + 14H+ + 3C2O42- ⎯→ 6CO2 + 7H2O + 2Cr3+ Notes: 1. In the reaction‚ the orange colour of the solution
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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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(NH4)2S2O8 + 2KI -> I2 + (NH4)2SO4 + K2SO4 This can be simplified to: S2O82- + 2I- -> I2 + 2SO42- These equations can only be carried out and be visible after the iodine has completely reacted with thiosulphate added – two moles of thiosulphate for every mole of iodine. Once all the thiosulphate has been used up in the reaction‚ the colour will start to appear. Results and Conclusions 1. Contained in the following chart:
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(H2CO3)‚ citric acid (HC6H8O7) and phosphoric acid (H3PO4). B. Objectives At the end of this exercise‚ you must be able to: Prepare and standardize a solution of Sodium hydroxide solution Determine the acidity of the two soft drink samples using the standardized solution Perform the right titration techniques II. Materials A. Reagents Sodium hydroxide (NaOH) pellets Potassium acid phthalate (HKC8H4O4) Phenolphthalein Soft drinks samples B. Apparatus 250-ml beaker 250-ml Erlenmeyer flask 100-ml
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