detergent manufacture‚ water treatment etc. It can be a pure compound of sodium carbonate‚ sodium bicarbonate or sodium hydroxide or the mixture of the three with compatible percent compositions. These compositions are determined by acid-base titrations‚ a volumetric process in determining the concentration of a substance in a certain solution which uses a base or acid as the titrant. The reaction between sodium carbonate and hydrochloric acid occurs in 2 stages‚ with the formation of
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smaller electrode potentials as compared with the other oxidants‚ gaining them the advantage of imparting a degree of selectivity essential in the determination of strong reducing agents amid the presence of weak agents. Although regular re-standardization was essential for Iodine solution due to its lack of stability‚ it was still suitable for titrations due to its advantage of having sensitive and reversible indicator [5]. Reduction-oxidation titrations involving iodine were classified mainly
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Making up Hydrogen Peroxide Volume required 250 cm3 and concentration required 0.1 moldm-3 Given concentration of H2O2 = 1.7 moldm¬-3 Number of moles (n¬¬¬¬¬¬¬¬¬¬¬) = Concentration (moldm-3) x Volume (dm-3) = 0.1 x 0.25 = 0.025 mol Volume (dm-3) = Number of Moles (n) X 1000 Concentration (moldm-3) = (0.025/1.7) x 1000 = 14.7 cm3 Distilled water required: 250 cm3 – 14.7
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SCH4U7-02 Monday‚ October 21‚ 2013 Designing an Experiment to Investigate Factors Affecting Rate of Reaction Introduction Hydrogen Peroxide (H2O2)‚ is the most simple peroxide and commonly used in several household items such as toothpaste or as an alternative to bleach. However hydrogen peroxide it is a very dangerous substance when accumulated in large amounts. If that situation occurs this substance must be decomposed. But how can we decompose this reaction? Well it decomposes by itself
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CHAPTER ONE INTRODUCTION Croton is an extensive flowering plant genus in the spurge family‚ Euphorbiaceae‚ established by Carl Linnaeus in 1737. The plants of this genus were described and introduced to Europeans by George Eberhard Rumphius. The common names for this genus are rush foil and croton‚ but the latter also refers to Codiaeum variegatum. The generic name comes from the Greek κροτον (kroton)‚ which means "tick" and refers to the shape of the seeds of certain species (Gledhill‚ 2008).
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of simple acid-base reactions; b) to review the stoichiometric calculations involved in chemical reactions; c) to review the basic lab procedure of a titration and introduce the student to the concept of a primary standard and the process of standardization; d) to review the calculations involving chemical solutions; e) to help the student improve his/her lab technique. Theory: Titration was used to study acid-base neutralization reaction quantitatively. In acid-base titration experiment‚ a solution
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CHEMISTRY-WINE MAKING | Investigating the effectiveness of common fining agents on homemade fruit wine with respect to Turbidity‚ Sediment level‚ Ph and Alcohol content. | | Year 12 Chemistry | Extended Experimental InvestigationA comparison of chemical flocculation agents | Mario Mitov | Mrs Cullen 2011 | | Contents: 1.0- Abstract 2.0- Introduction/Background
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Titration Objective: • To learn some technique in volumetric analysis: Redox titration. • To review the stoichiometry of an oxidation-reduction reaction. • To practice the titration technique. • To determine the concentration of an unknown sodium oxalate (Na2C2O4) solution by titrating it against standardized potassium permanganate solution (KMnO4). Principle: Redox reaction is just like an acid-base reaction. An acid can show its acidic properties in the presence of base only. Like
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will use this experience to experimentally determine the concentration of acetic acid in an unknown solution. There are three parts to this experiment‚ they are 1. Preparation a standard solution of oxalic acid (~0.07 M) 2. Preparation a sodium hydroxide solution (~0.1M) which will be standardized using the standard oxalic acid solution. 3. Determination of the concentration of acetic acid in an unknown vinegar solution. (0.1-0.2M) Introduction Standard solutions are solutions
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This shows that the tri-iodide ions are reduced back to iodide ions by the thiosulphate ions. Thus‚ the iodine that is formed in reaction (1) is immediately transformed into iodide ion and we do not see the blue-black colour of the starch-iodide complex until all of the thiosulphate ion has reacted with I 2(aq) and is exhausted. I3- (aq) + starch  Starch-I5- complex + I-(aq) Once the thiosulphate ion has been exhausted‚ the tri-iodide ion can react with the starch‚ forming the
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