standard solutions and titrations are prepared in industry P2 demonstrate practically the ability to prepare chemical solutions and test their accuracy Scenario: You are working as a scientist for ‘Edvisprog’ – a company producing visual aids for education. The team is currently working on a web-based program to help students understand the key features of the periodic table and information to guide students to help the teaching and understanding of the use of titrations. You have to
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the amount could always been found‚ even there is a loss during the transport‚ and this makes the result accurate. Gravimetric analysis also does not require a strict temperature condition. Since the substances are usually solid and there is no titration performed during the experiment‚ temperature difference gives a small influence on gravimetric analysis‚ and this makes the experiment more accurate when perform in a normal experimental environment. Disadvantages of Gravimetric Analysis When
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known concentration of 0.1molL-1. The equation of the reaction between ethanoic acid and sodium hydroxide is as follows: CH3COOH + NaOH CH3COONa + H2O When the titrations end point is determined and volumes of reactants are measured the concentration of the ethanoic acid can be calculated. Keywords: Titration‚ Sodium Hydroxide‚ Ethanoic Acid‚ Equivalence Point‚ pH Meter‚ Standard Solution Method: Using a bulb pipette 25cm3 of vinegar was measured into a 250cm3 standard
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12‚ 2012‚ and March 19‚ 2012 Purpose: The purpose of this experiment was to discover the unknown concentration of acid in six different Pepsi products; Pepsi‚ Diet Pepsi‚ Dr. Pepper‚ Diet Dr. Pepper‚ Pepsi Wild Cherry‚ and Pepsi Max. Titrations find the point at which equal moles of a known concentration react with equal moles of an unknown concentration giving the equivalence point. Also‚ the pKa was observed which conveys the equivalence point by graphing the results and determining
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Experiment 1 : Redox Titration Using Sodium Thiosulphate Abstract This experiment is to determine the concentration of oxidizing solution using the iodine/ thiosulphate titration where the reducing solution is potassium iodate solution and the oxidizing solution is sodium thiosulphate solution. Potassium iodate solution which is an oxidizing agent is added into an excess solution of acidified potassium iodide. This reaction will release iodine. Potassium iodide is acidified with sulphuric acid
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Lab 4: Titration of a Redox Reaction The purpose of this experiment is to standardize a solution of Mohr’s salt‚ and to use titration to determine the volume ration of ferrous solution to the permanganate standard and calculate the concentration of the ferrous solution. First‚ Mohr’s salt was mixed with H2SO4. Then‚ the solution was titrated until the end point was reached. The volumes were recorded‚ and used to calculate the molarity of the ferrous solution. The major
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Virtual Chem Lab 6-2 & 6-3 Anonymous CHM/110 June 16‚ 2014 Zamir Deen Virtual Chem Lab 6-2 & 6-3 Ranking Salt Solutions by pH 6-2: Ranking Salt Solutions by pH In this assignment you will be asked to rank aqueous solutions of acids‚ bases‚ and salts in order of increasing pH. This is most easily done by first identifying the strong acids that have the lowest pH‚ the strong bases that have the highest pH‚ and the neutral solutions that have a pH near 7. The weak acids will have a pH between
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I. Purpose: In this experiment we experimented with titration. We saw the effects of titration on an acid and then on a base. The acid we used was hydro chloric acid and the base was ammonia. The acid turned pinkish red when properly titrated and the base turned clear. We used phenolphthalein as the titrate which turns red in acidic solutions and clear in basic solutions. The control aspects of this lab were the hydrochloric acid and ammonia. The independent variable was the titrate the phenolphthalein
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ANSWERS TO QUESTIONS: 1. What are the significant regions in the titration curve? Relate the characteristics of each region to the pH results obtained. - There are four significant regions in each titration curve‚ namely the initial‚ pre-equivalence‚ equivalence‚ and post-equivalence points. These points are named according to its position relative to the equivalence point. The equivalence point signifies the volume of titrant at which the solution becomes neutral. This is represented in the
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water-soluble and is an enantiomer of ascorbic acid. (Commercial vitamin C is often a mixture of ascorbic acid and other ascorbates.) Ascorbic acid‚ C6H8O6‚ is a reducing agent that reacts rapidly with iodine (I2). As the iodine is added during the titration‚ the ascorbic acid is oxidized to dehydroascorbic acid‚ while the iodine is reduced to iodide ions as shown in the following equation: (studymode.js‚ 2010). Ascorbic acid + I2 (aq) -----------> 2I- (aq) + dehydroascorbic acid Due to this reaction
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