CAL Biology Practical 2 – Identification of Biochemicals in Pure Form Name :……………………………………………………………. MARK: Class :……………………………………………………………. PRACTICAL 2: IDENTIFICATION OF BIOCHEMICALS IN PURE FORM CAUTION: Any heating that has to be done in the following tests should be carried out in a water bath at the boiling point of water. Direct heating of test-tubes should not take place. Introduction Biochemical Tests Qualitative - present/ absent Semi-quantitative - present in >/<
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Practical 12: Digestion in Humans Aim: To distinguish between 5 liquids to come to a conclusion from which region of the alimentary canal it was extracted from. Hypothesis In this practical‚ we have been given 5 unknown solutions hence it is not possible for us without any logical analysis to come up with a conclusion regarding the positioning along the alimentary canal. We cannot come up with a proper answer or predict results without running through the tests. I though can base my
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The structure and function of carbohydrates A carbohydrate is an organic molecule containing only Carbon‚ Hydrogen and Oxygen with the general formula Cn(H20)n. They are made up of individual molecules called monomers which are joined together by condensation reactions to make a longer chain called a polymer. Carbohydrates are categorised in to three main groups; monosaccharides‚ disaccharides and polysaccharides. Monosaccharides are single sugars and are sweet tasting soluble substances such
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EXPERIMENT 1: Aim: To range the metals copper‚ lead‚ silver and zinc together with hydrogen. Start with the strongest reducing agent. Hypothesis: The nobler a metal is‚ the worse reducing agent. Apparatus/requirements: Sandpaper‚ strips of; zinc‚ lead‚ silver and copper‚ solutions containing aqueous; Zn2+‚ Pb2+‚ Cu2+ and Ag+ ions (0.2 M)‚ hydrochloric acid (5.0 M)‚ emery paper‚ test-tubes. Method: Burnish the three metal strips to get a shiny surface‚ after drop a drop of each of the metal
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Determination of the concentration of chlorine ions Aim: To compare the concentration of chloride ions in pool and tap water respectively. Background: Tap water contains a variety of dissolved ions such as Ca2+‚ Mg2+‚ Na+‚ HCO3- and Cl-. In this experiment we will determine the concentration of the Cl- ions‚ and comparing it to the concentration found in a sample of pool water. The method used is the standard one for determining the concentration of chloride ions: titration with
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Report Submitted: September 4‚ 2013 Title: Observations of Chemical Changes Purpose: To observe some properties of chemical reactions and to associate chemical properties with household products. Procedure: In this experiment I used a 96-well plate to hold each of the chemical reactions that occurred during this lab. Using a pipet‚ I added two drops of one chemical with two drops of another chemical and observed the effects of each reaction. Data Table 1: Experimental Data Well # |
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Chemical Change Lab Name Data Table 1: |Chemicals |Well # |Reaction on White Paper |Reaction on Dark Paper | |NaHCO3 + HCl |A6 |Remains clear. |Remains clear. | |HCl + Blue Dye |B6 |Orange color. |Cannot distinguish color
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Fungal contribution in the etiology of infections has increased considerably. However‚ as medical technology has improved‚ The number of infections by intrinsically drug-resistant species has increased rapidly. Despite the constant introduction of new and effective synthetic drugs to the market‚ medicinal plants‚ which are the historical basis of therapeutic health care‚ represent an alternative that is economical‚ accessible‚ and applicable to various pathologies‚ particularly in developing countries
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| Soluble | All negative ions are with | All positive ions | Soluble | Nitrate NO3- ions are with | All positive ions are | Soluble | Acetate CH COO- ions are 3with | All positive ions are | Soluble | Chloride‚ Cl-Bromide Br-Iodide I- | CuAll other positive ions | Low SolubilitySolubleSoluble | Sulfate SO 2-4 | BaAll other positive ions | Low SolubilitySoluble | Sulfide S -2 | All positive ions | Soluble | Hydroxide‚ OH- | Ba | Soluble | Phosphate PO 3-4Carbonate CO
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manufacturer ’s specification. Principle In this analysis‚ certain amount of iodine solution‚ which is known in excess‚ is added to acidified ascorbic acid solution. Brown iodine can be easily reduced by acidified ascorbic acid to form colourless iodide ion: ← Equation I The excess iodine is then back titrated by standard sodium thiosulphate solution‚ by using a burette and starch solution (used as end point indicator) Similarly‚ iodine can also
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