Molar hydrochloric acid Toluidine blue stain 2 watch glasses or small sample tubes Hollow glass blocks Pipettes Microscope slides and cover slips Pair of fine forceps Filter paper Microscope with magnifications of x100 and x400 Stop watch Method: 1. Firstly cut out about 1cm from several root tips of growing garlic roots. Choose root tips which are white and have rounded edges‚ not ones that are turning brown 2. Place the root tips in a hollow glass block containing 2cm of 5M hydrochloric acid solution
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gas will be used in order to determine the reaction stoichiometry Magnesium is used to react with hydrochloric acid in order to produce hydrogen gas. One of the purposes of this experiment is to determine X in the equation below The mass of the magnesium used is measured before the use in the experiment via an analytical balance. The known amount of magnesium is then reacted with excess hydrochloric acid which causes the magnesium to be the limiting agent in this particular reaction. The amount
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was the most effective out of all 3 of them. To figure out which one was the most effective‚ the antacid which took the most amount of drops of Hydrochloric Acid (HCl) to neutralize the antacid would be most effective. Based on the results‚ Life Brand Milk of Magnesia was the most effective out of the three antacids because it took 120 drops of hydrochloric acid (HCl) to neutralize the antacid. The active ingredient in Life Brand Milk of Magnesia is magnesium hydroxide (“Nonprescription Medicines and
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products 1 Goggle-safety 1 Well-Plate-24 1 Well-Plate-96 1 Pipet‚ Empty Short Stem 1 Aqueous Ammonia‚ 1M -1mL 1 Bromthymol Blue‚ 0.04% - 2 mL in Pipet 1 Copper (II) Sulfate‚ 0.2 M – 2 mL in Pipet 1 FDC Blue Dye #-1.0.1% - 2 mL in Pipet 1 Hydrochloric Acid‚ 1.0M-1 mL 1 Lead (II) Nitrate‚ 0.2 M- 2 mL in Pipet 1 PhenolphthaleinSolution1%1mL 1 Potassium Iodide‚ 0.1 M-2 mL in Pipet 1 Silver Nitrate‚ 0.1 N – 2 mL in white Dropper Bottle 1 Sodium Bicarbonate‚ 1 M – 2 mL in Pipet 1 Sodium Hydroxide
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of solid sodium hydroxide in water. NaOH(s) ---> Na+(aq) + OH-(aq) + heat Reaction 2: The reaction of solid sodium hydroxide with dilute hydrochloric acid. NaOH(s) + H+(aq) + Cl-(aq) ---> Na+(aq) + Cl-(aq) + H2O Reaction 3: The reaction of sodium hydroxide solution with dilute hydrochloric acid solution. Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) ---> Na+(aq) + Cl-(aq) + H2O Objectives: To measure and compare the amount of heat involved in
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can affect Reaction Rate. The experiment will be performed by heating equally sized and weighted lime stones with equal amounts and concentration of Hydrochloric acid at different temperatures. The temperatures will be 35˚C and 40˚C. We will measure the reaction rates by observing gas release of the reaction between lime stones and Hydrochloric acid. The amount of gas release at different temperatures will be compared afterwards to see if temperature can affect Reaction Rate. Hypothesis:
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weight of magnesium by measuring the amount of hydrogen gas evolved when hydrochloric acid reacted with magnesium. In order to measure the atomic weight I needed to measure the amount of the hydrogen gas that was evolved in reaction to the acid of the magnesium. The reaction used was: Mg + 2HCl --> H2 + Mg2+ (aq) + 2Cl- (aq). The major findings of this experiment were that there was a chemical reaction between hydrochloric acid and magnesium‚ and the reaction produced the hydrogen gas. The results
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IGCSE Complete Chemistry Notes Unit 1: States of matter Everything is made of particles. Particles in solid are not free to move around. Liquids and gases can. As particles move they collide with each other and bounce off in all directions. This is called random motion. In 2 substances‚ when mixed‚ particles bounce off in all directions when they collide. This mixing process is called diffusion. It’s also the movement of particles without a force. The smallest particle
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substance being tested. pH 3.5 Acetate Buffer— Dissolve 25.0 g of ammonium acetate in 25 mL of water‚ and add 38.0 mL of 6 N hydrochloric acid. Adjust‚ if necessary‚ with 6 N ammonium hydroxide or 6 N hydrochloric acid to a pH of 3.5‚ dilute with water to 100 mL‚ and mix Hydrochloric Acid‚ Normal (1 N) HCl‚ 36.46 36.46 g in 1000 mL Dilute 85 mL of hydrochloric acid with water to 1000 mL. Sulfuric Acid‚ Normal (1 N) H2SO4‚ 98.08 49.04 g in 1000 mL Add slowly‚ with stirring‚ 30 mL of
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green. There is probably a chemical in the dry ice that is reacting with the universal indicator which is causing the substance to change colors. Hydrochloric acid changes the color of the mixture and makes it green to yellow but when you add more hydrochloric acid then the first time the color becomes darker and eventually turn purple. The hydrochloric acid reacts with the solution and makes the colors change‚ when you add more than a certain amount the color becomes darker. When the tablet
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