Purpose – The purpose of this lab was to be able to predict the phase of matter after a double replacement reaction‚ what the products were‚ and if the reaction was completed or not. Materials and Methods - • .1 M NaCl • .1 M AgNO3 • .1 M Na3PO4 • .1 M NaOH • .1 CuSO4 • Five droppers • Spot Plate • Pen/Pencil • Paper • Goggles • Apron Safety Precautions – • Wear goggles and apron at all time while inside the lab. • You may use rubber gloves o protect your hands from the chemicals
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| (NH4)Cl | Green- yellow | 7 | Neither | (NH4)2SO4 | Green- Yellow | 7 | Neither | AlCl3 | Red-orange | 3 | Cationic | Ca(NO3)2 | Murky green | 7 | Neither | Fe2(SO4)3 | Red | 2.5 | Cationic | Na2CO3 | Dark blue | 9.5 | Anionic | Na3PO4 | Orange-red | 3 | Cationic | K2SO4 | Green | 7 | Neither | KBr | Green | 8 | Anionic | (NH4)2C2O4 | Green | 8 | Anionic | NH4CH3COO | Blue green | 9 | Anionic | (NH4)2CO3 | Blue green | 9 | Anionic | Solution | Color of Univ Indicator
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less harmless. The uses of the stoichiometry cffffffffffffffffffffffffffffffffffeeeeer bags are located inside automobiles. The air bag is in front of the passenger seat inside the dashboard. Once the vehicle gets into a crash the air bag pops out. The air bags are filled nitrogen gas. Hazardous sodium metal is also produced with the nitrogen so the potassium nitrate adapts with the sodium to make the hazardous sodium oxide less harmless. The uses of the stoichiometry calculations are to figure out
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Mass relationships in a chemical reaction Introduction: The Law of Conservation of Mass dates from Antoine Lavoisier’s 1789 discovery that mass is neither created nor destroyed in chemical reactions. In other words‚ the mass of any one element at the beginning of a reaction will equal the mass of that element at the end of the reaction. If we account for all reactants and products in a chemical reaction‚ the total mass will be the same at any point in time in any closed system. http://www.nature
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from the front of the laboratory and the zinc coating on the iron nail was rubbed off using the steel wool. The iron nail was then weighed on a digital scale and its mass was determined to be of 6.5 grams. Two tablespoons of copper(II) chloride (CuCl2) crystals were then added to the beaker. The copper(II) chloride crystals were blue in colour‚ shown in Figure 1 below. Figure 1. Photograph of two tablespoons of copper(II) chloride crystals in a beaker. One hundred millilitres of water was
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will then test your predictions in the laboratory. 1. Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO‚ HCl‚ HCN‚ NaOH‚ NH3‚ NaCN‚ KNO3‚ H2SO4‚ NH4Cl‚ H2SO3‚ NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: H2SO4: This is because the first hydrogen is strong and completely ionizes and the second is weak and ionizes very minutely. It is also a lower pH than HCl because the second
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Stoichiometry in the Industry (Mining Industry) Prepared By: Ryan Khan and Michael McDonald Course code: SCH3U1 Teacher: Miss Kedzia Due Date: 22/4/2013 Date Submitted: 22/4/2013 What Is Stoichiometry? Stoichiometry as defined by our textbook is “the study of the quantitative relationships among the amounts of reactants used and the amounts of products formed in a chemical reaction”. Basically‚ Stoichiometry is the science of counting and studying the relationship between the amounts
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will then test your predictions in the laboratory. 1. Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO‚ HCl‚ HCN‚ NaOH‚ NH3‚ NaCN‚ KNO3‚ H2SO4‚ NH4Cl‚ H2SO3‚ NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: H2SO4: This is because the first hydrogen is strong and completely ionizes and the second is weak and ionizes very minutely. It is also a lower pH than HCl because the second
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Ionic Reactions Abstract This experiment is designed to study the nature of ionic reactions‚ and write net ionic equations for precipitation reactions‚ as well as to identify spectator ions‚ perception reactions and solubility of different compounds. Experiment and Observations In this experiment I was using a 96-well plate to add two drops of the following solutions into seven wells in rows A through E: cobalt (II) nitrate‚ copper (II) nitrate‚ iron (III) nitrate‚ barium
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.3455g Mole of water in hydrate .0192mol Mole of anhydrous salt: CuSO4 .004094mol CuCl2 .004859mol CoCl2 .005033mol Mole ratio of water to each of the anhydrous salts: CuSO4 4.69 CuCl2 3.95 CoCl2 3.81 Observations: The unknown
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