The amount of hydrogen peroxide was recorded after the reaction for the certain time given has taken place. We used sulfuric acid to stop the reaction with the catalase from occurring. This process is known as denaturing (Campbell 152). The potassium permanganate in this experiment was used as hydrogen peroxide indicator. It determined the amount of hydrogen peroxide remaining after the reaction occurred. Based on our experiment we observed that the time does play a crucial role on the catalase reaction
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The Effect of pH on the Rate of Enzyme Catalysis of Catalase Objectives: The objective of this lab was to develop a protocol to investigate the effect of an environmental variable on the catalytic function of an enzyme. More specifically‚ the objective was to perform an experiment in order to test the effect of pH on the function of the enzyme catalase. Introduction: Enzymes are proteins that act as catalysts for reactions. This simply means that enzymes lower the activation energy required
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solution. The area in which light is absorbed can provide information about the molecule‚ such as the concentration‚ by identifying the most preferentially absorbed wavelength.1 Food coloring and potassium permanganate: This method was used with red‚ blue‚ and purple food colorings and potassium permanganate. Wavelength measures energy in nanometers‚ from the top of one peak to the top of another peak‚ of a wave. Each wavelength
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Kinetics of the Harcourt-Essen Reaction Name: Manpreet Kaur Candidate Number: 7123 AS and A2 Aims: AS AIMS: 1. Investigate the effect of temperature on the rate of reaction. For this aim 3 sets of results will be obtained by timing how long it takes for the colour change to occur in different temperatures determined by the use of an electric water bath. With these results‚ the effect of temperature on the rate of reaction will be investigated. 2
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60). Label the remaining beaker “control”. 2. With the “control” beaker pour 10 mL’s of H2O2‚ add 10 mL’s of distilled water (in place of the catalase). Finally add the 10 mL’s of sulfuric acid. 3. Suck up 10 mL’s of potassium permanganate in the pipet. Add potassium permanganate one drop at a time to the beaker. After each drop‚ stir the mixture. Continue to add KMnO4 to the mixture turns brown and stays brown. 4. Invert the pipet and record the amount of KMnO4 left in the pipet. Subtract the
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Introduction In this Lab the students dealt with Osmosis‚ movement of water molecule or solvent from a high concentration to a low concentration‚ through selective permeability‚ a protective barrier that provide some particle the ’direct ’ passage in and out of the plasma membrane ( Lacerda L.2011) Allowing some molecules enter and exit the cell membrane‚ to create a balance in concentration inside and outside of the cell‚ by doing so the cell often become hypotonic‚ where the concentration
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Redox Titration Lab ABSTRACT: In this lab‚ 0.010 M purple-colored potassium permanganate solution was standardized by redox titration with iron (II) ammonium sulfate hexahydrate (FAS). The average mass of the three flasks of FAS was 0.483 grams. Once the concentration of the standard solution of KMnO4 (aq) was determined‚ it was used to determine the concentration of Fe2+ in iron pills. On average‚ there was 0.01813 L of solution used. With this information and the balanced net-ionic equation
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which is about 0.5% it also contains 0.52& to 1.81 citric acid and only a trace of oxalic acid is present. These acids in tomatoes‚ in combination with sodium and potassium either form sodium or potassium acid malate‚ citrate or oxalate. Their end products when oxidized in the body are carbon dioxide‚ water and the carbonates of potassium and sodium. The latter has alkaline reaction. Tomatoes thus leave an alkaline ash in the process of oxidized by the body. This increases the alkalinity of the blood
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what would be observed; and (ii) write an appropriate equation. (a) adding excess sodium sulphite solution to iodine solution (b) adding aqueous chlorine to potassium bromide solution (c) adding excess potassium iodide solution to acidified potassium permanganate solution 1 (d) adding excess iron(II) sulphate solution to acidified potassium dichromate solution (e) adding concentrated nitric acid to magnesium ribbons (f) (g) (h) (i) (j) (k) (l) (m) (n) 5. adding dilute nitric acid to zinc granules
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= 2.8g = 0.1N | Hydrochloric acid HCl‚ FW = 36.5‚ Density = 1.2 1M = 83mls = 1N (Use 86mls) 250ml 0.1M = 2mls = 0.1N 1 liter 0.1M soln = 8.6mls = 0.1N | Oxalic acid H2C2O4.2H2O‚ FW = 126.07‚ Eq. = 63g/l 250ml 0.05M = 1.575g = 0.1N | Potassium hydrogen phthalate KH(C8H4O4)‚ FW = 204.23‚ Eq. =204g/l 250ml 0.1M = 5.105g = 0.1N | Potassiun hydrogen iodate KH(IO3)2‚ FW = 389.92‚ Eq. 73.07g/l 250ml 0.1M = 9.75g = 0.1N | Sodium carbonate Na2CO3‚ FW = 106‚ Eq. =53g/l 250ml 0.05M = 1
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