ACIDS‚ BASES AND SALTS 1. What are indicators? What are the different types of indicators? An indicator is a dye which changes colour when put into an acid or a base. The different kinds of indicators are- Natural indicators- Litmus is a natural indicator‚ litmus solution is a purple dye which is extracted from a plant called lichen. Litmus turns red in acidic solutions and blue in basic solutions. Other
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LU 1 - Tutorial 1. Write the formulas for the following compounds: Compound Copper (II) chloride Iron(II) sulphate Sodium sulphate Ammonium nitrate Sodium nitrite Potassium sulphate Magnesium phosphate Formula Compound Lithium acetate Manganese (IV) nitrate Potassium permanganate Iron (III) oxide Potassium sulphite Potassium hydrogen carbonate Sodium iodate Formula 2. Express the following numbers in scientific notation: a) 0.000000027 b) 356 c) 47 764 d) 0.096 3. Express the following numbers
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Task 3: Tests for Anions: An Anion is an atom which is negatively charged therefore indicating a larger amount of electrons than proteins. Overall the tests for anions were mainly conclusive however 6 out of 8 of the anions we were testing for could only be determined from one specific result for example if a black precipitate formed following the tests the substance is therefore a sulphide however the same result would also show the presence of carbonate and hydrogen carbonate this therefore
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manipulated. At all stages‚ every method must be made to assure that oxygen is neither introduced to nor lost from the sample. Furthermore‚ the sample must be free of any solutes that will oxidize iodide or reduce iodine. Chemicals: Manganese(II) sulphate solution – prepared by dissolving 48 g of MnSO4.4H2O in water to five 100 cm3 solution; alkaline potassium iodide solution—prepared by dissolving 15 g of KI in about 25 cm3 of water‚ adding 66 cm3 of 50% NaOH‚ and diluting to 100 cm3; concentrated
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Total dissolved solids (TDS) 2.4.2.9 Total suspended solids (TSS) 2.4.3 Chemical characteristics of water 2.4.3.1 Hydrogen ion concentration (PH) 2.4.3.2 Hardness 2.4.3.3 Iron 2.4.3.4 Copper 2.4.3.5 Phosphate 2.4.3.6 Nitrate 2.4.3.7 Sulphate 2.4.4 Biological characteristics of water 2.4.4.1 Bacteria 2.4.4.2 Algae 2.4.4.3 Fungi 2.4.4.4 Protozoa 2.4.4.5 Viruses 2.5 Case studies on pipe borne water analysis 2.5.1 Chemical and inorganic parameters 2.5.2 Researches on microbiological
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91 Chapter 5 Sources of plant nutrients and soil amendments A large number of diverse materials can serve as sources of plant nutrients. These can be natural‚ synthetic‚ recycled wastes or a range of biological products including microbial inoculants. Except for microbial inoculants (biofertilizers)‚ all of these contain one‚ two or several plant nutrients in readily or potentially available forms. A certain supply of mineral and organic nutrient sources is present in soils‚ but
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Apparatus:Digestion VesselIncubator preheated to 150 ̊C‚ with holes for holding digestion vesselsMicroburetSilver Sulphate Sulphuric Acid (AgSO4)Potassium Dichromate MixTest SampleSpectrophotometerFigure 1-SpectrophotometerFigure 2-IncubatorFigure 3-Absolute Value Solutions Methodology:1.To ensure no contamination of sample occurs‚ cleanthe culture tubes and caps using 20% silver sulphate sulphuric acid (AgSO4)2.Insert 3.5ml of AgSO4‚ 1.5ml of potassium dichromate mixand 2.5ml of test sample
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●Glass stirring rod 20cmᶟ pipette ●Hydrated nickel(II) sulphate (NiSO₄.6H₂O) 100cmᶟ standard flask ●Standardised 0.10moll⁻¹ EDTA solution 250cmᶟ conical flask ●1 moll⁻¹ ammonium chloride Weighing bottle ●Murexide indicator Balance (accurate to 0.01g) ●0.88 aqueous ammonia 100cmᶟ beakers ●Deionised water 25cmᶟ measuring cylinder Wash bottle Pipette filler White tile Filter funnel Approximately 2.6g of hydrated nickel(II) sulphate was transferred to a weighing bottle and the contents weighed
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following may be used: * Fehling’s Solutions A and B * Sodium hydroxide and copper (II) sulphate solutions 1. Add 2 cm3 of the liquid food sample* to a clean‚ dry test tube 2. Add 2 cm3 of Biuret Reagent. Alternatively: * Use sodium hydroxide solution and copper sulphate solution instead. Add 1 cm3 of sodium hydroxide solution (40% or bench solution) and 1% copper (II) sulphate solution dropwise – drop by drop - to the food sample * Use Fehling’s A and B solutions instead
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White tile Wash bottle Glass rod Burette clamp and stand Pipette Funnel Thermometer (10-110oC) Materials: 0.2M KMnO4 solution Standard 0.1M iron (II) ammonium sulphate Standard 0.05M oxalic acid dihydrate 2M of sulphuric acid Procedure: A. Standardization of KMnO4 solution with standard iron(II) salt solution 1. 25.0cm3 of the given KMnO4 solution was diluted to exactly 250cm3 in a volumetric flask
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