POST-HARVEST PHYSIOLOGY (GTN 3700) PRACTICAL 2: DETERMINATION OF SOLUBLE SOLIDS CONCENTRATION USING HANDLED REFRACTOMETER Name: Noor Fareeza Juliana Bt. Abd. WahabMatric No.: UK32565 Program: Bac. Sc. Agrotechnology (Postharvest Technology) Group: 8 INTRODUCTION The major soluble solid in fruit juices is sugars‚ so the soluble solids can be used as an estimate of sweetness. Soluble solids concentration measurement in the flesh of each fruit by removing the peel and seed
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DATE PERFORMED: JANUARY 6‚ 2011 SPECTROPHOTOMETRIC DETERMINATION OF THE EQUILIBRIUM CONSTANT OF A REACTION ABSTRACT The objective of the experiment was to determine the equilibrium constant of the reaction forming ferric thiocyanate through the use of Spectrophotometry. For the calibration‚ five standard solutions were prepared‚ then their respective absorbance values that were obtained through the use of the spectrophotometer‚ were plotted versus the concentration of the analyte so that a calibration
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and Potentiometric Determination of its Purity and Dissociation Constant ------------------------------------------------- Abstract The purpose of the study is to synthesize salicylic acid from the ester‚ methyl salicylate‚ and determine the acid’s dissociation constant and purity. The ester was converted to salicylic acid by base hydrolysis. The products were refluxed and recrystallized‚ to ensure maximum purity‚ and filtered‚ dried‚ and weighed. The melting point of the product was determined using
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Reviewer’s Name: Sanjeev Mishra UMN ID Number: 4585009 The Photoelectric Effect: A Determination of Planck’s constant Ian E. Jaeger School of Physics and Astronomy‚ University of Minnesota – Twin Cities 116 Church St. S.E.‚ Minneapolis‚ MN 55455 Abstract The photoelectric effect was explored to determine an experimental value of Planck’s constant‚ h. Included is a brief introduction to the history leading up to Einstein’s discovery of the photoelectric effect as well as the theory behind
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Experiment 19 - Determination of the equilibrium constant for the reaction Fe3+ (aq) + SCN( (aq) = FeSCN2+ (aq) Object: To determine the equilibrium constant by a colorimetric method Theory: Colorimetric methods of analysis are usually applied to the determination of small concentrations of either inorganic or organic materials in a solution. The constituent sought must be coloured or must be capable of reacting with a reagent to produce a substance having a suitable colour. Beers Law‚ which
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Name SOLUBILITY CURVES Answer the following questions based on the solubility curve below. Which salt is least soluble in water .. at 2O° C? 2. How many grams of potassium chloride can be dissolved in 200 g of water at 80° C? IO 3. At 40° C‚ how much potassium _ __nitrate coin be dissoiu$tl ^n 30D.g of water? ------W- ’1 80 70 ...- O --60 0 5© 40 4. Which salt shows the least change 30 In solubility from 0° - 100° C? 20 10 At 30° C‚ 90 g of sodium
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SPECTROPHOTOMETRIC DETERMINATION OF THE EQUILIBRIUM CONSTANT OF A REACTION Methodology The following stock solutions were prepared: 1.0 M HCl‚ 0.1 M HCl‚ 0.1 M KSCN‚ 0.002 M KSCN (in 0.1 M HCl)‚ 0.2 M FeCl3 (in 0.1 M HCl)‚ and 0.002 M FeCl3(in 0.1 M HCl). Using the prepared stock solutions‚ the standard (Table 1) and Unknown (Table 2) solutions were prepared. Table 2. Preparation of Standard Solutions 0.10 M KSCN 0.002 M FeCl3 0.1 M HCl Blank 2.0 ml 0.0 ml 8 ml S1 2.0 ml 0.1 ml 7
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solution that contains more dissolved substance than a saturated solution does. This occurs when a solution is prepared at a higher temperature and is then slowly cooled. This is a very unstable situation‚ so any disturbance causes precipitation. Solubility can be understood in terms of two factors: The natural tendency toward disorder favors dissolving. The relative forces between and within species must be considered. Stronger forces within solute species oppose dissolving. Stronger forces
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compounds which dissolved in the solvent are soluble‚ while those which are slightly dissolved are moderately soluble and the undissolved ones are not soluble. However‚ nothing crystallized due to an excess amount of each solvent. For the second part of the experiment‚ approximately 25 mL of distilled water was combined with 1 g of salicylic acid and it took 6 mL of water to dissolve the sample at the boiling point. When it was crystallized‚ the product was almost white to colourless and it formed
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solvent mixed together Sodium hydroxide- Soluble Copper Oxide- insoluble Calcium hydroxide- Insoluble Silver iodide- insoluble Aluminium nitrate- soluble Most ionic substances will dissolve in water but covalent substances usually wont dissolve. Solubility of a solute = mass of a solid required to a saturate 100g of water at a particular temperature. Calculating Solubility 2g potassium chlorate dissolves in 20g water at 28oC what is its solubility? 2 x 100/20 = 10.0g potassium chlorate/100g
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