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    Coagulation of Proteins

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    4A.2 RRL 4A.2.1 Coagulation of Proteins Coagulation of protein refers to sticking together‚ like a blood clot‚ usually as a result of denaturation or coming out of solution due to abnormal ionic strength or a change of solvent. Definite characteristics of the proteins are changed when they are coagulated‚ among which is loss of solubility in water and dilute salt solutions. In some instances and under certain conditions the coagulation process may be reversible. (Campbell‚ et.al‚ 1979) 4A.2.2

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    Analysis of an Antacid

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    find out which will be the most effective at neutralizing acids. We will test this by seeing how much drops of hydrochloric acid (HCl) are required to neutralize a certain amount of the antacid. Antacids are used to resist heartburn. We sometimes use them to treat this because antacids are a mild base that can neutralize acids in our stomachs‚ such as HCl. The purpose of this lab is to see how well each antacid neutralize hydrochloric acid. Procedure: 1. Obtain two burets‚ one for use with the

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    The Organic Chemistry

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    CLASSIFICATION TESTS A. Acids There are relatively few suitable tests for carboxylic acids. Classification is based mostly upon solubility tests. If the compound is water soluble‚ test the aqueous solution of your compound with pH paper (also check the pH of the original water). If the compound is water-insoluble and it dissolves in 5% (1.5M) sodium hydroxide and 5% NaHCO3 solutions as performed in your solubility tests‚ it can be classified as a carboxylic acid. Establish an equivalence value

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    from the original solution? Materials: 1 M copper (II) nitrate 3 M hydrochloric acid 2 M sodium hydroxide 600 mL beaker 250 or 400 mL beaker Ice water Distilled water Stirring rod Bunsen burner Ring stand Al wire‚ 18 gauge or heavier Graduated cylinder pH paper Watch glass‚ 90 mm Goggles Acetone Procedures: Conversion 1: THIS IS ALREADY COMPLETED FOR YOU!!! Copper reacts with nitric acid to produce a brownish-orange gas called nitrogen dioxide. The blue color

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    3.1 Overview The experiment was divided into three parts. In the first part was the preparation of empty CNPs. The second part was the preparation of CNPs loaded with single drug which was AA and TQ meanwhile the third part was the preparation of CNPs loaded with dual drug (AA and TQ). The last part was the analytical testing conducted to investigate the properties performance such as smaller or larger in trend as well as to characterize the entrapment efficiency of drugs. The chemicals and technique

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    Stirring rod Evaporating dish Magnet Magnifying glass Crucible tongs Spatula Balance Meeker burner Ring stand Iron ring Wire gauze Forceps Sulfur Iron filings Sodium Bicarbonate Sodium Chloride Sugar Sand Magnesium ribbon Hydrochloric Acid Distilled water Filter paper 9 disposable dishes Procedure: 1. Label 7 of the dishes with the names of the following products: Sulfur‚ Iron‚ Sodium Bicarbonate‚ Sodium Chloride‚ Sugar‚ Sand‚ and Magnesium. Place small samples of each in

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    chem lab 3

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    Did you observer any chemical changes in this experiment? Yes What evidence did you use to decide that something was a chemical change? I observed during the application of the hydrochloric acid to some of the substances bubbling‚ and smoking Give at least two examples of chemical changes you observed. Green changed from blue to application of HCL to Mg smoking and bubbling and CuCO3 Classify the following properties of sodium

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    Chem experiments

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    UTAR FHSC1134 Inorganic Chemistry Trimester 3 Experiment 1 ________________________________________________________________________ Title: Investigating the Properties of Period 3 Oxides Aim: To examine the oxides of Period 3 elements and describe their structure and bonding. Introduction: Generally‚ there are oxides of metals and non-metals. Metals burn in oxygen to form basic oxides while non-metals form acidic oxides. Structurally‚ they are covalent or ionic compounds. You are to

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    Measuring cylinder • Teat pipette • Rack with 3 small test tubes • Beaker Chemicals: • Butan-1-ol (harmful and flammable) • Sodium bromide • Concentrated sulphuric acid (very corrosive) • Anhydrous sodium sulphate • Concentrated hydrochloric acid (corrosive) • Ethanol (highly flammable) • Dilute nitric acid (corrosive) • Dilute sodium hydroxide (corrosive) • Silver nitrate solution‚ approximately 0.1 M • Sodium bromide solution‚ approximately 0.1 M Procedures:

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    Chemistry Copper Lab

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    Chemistry 11 Final Examination Review - Answers Part A - True or False. Indicate whether each of the following statements is true or false. Correct the false statements. F 1. The mass of an electron is equal to the mass of a proton. The mass of an electron is less than the mass of a proton. T 2. The mass of a proton is approximately equal to the mass of a neutron. T 3. The atomic number represents the number of protons in a nucleus. T 4. The proton has a mass of approximately

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