Copper sulphate

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    Materials: Metals: • 15 pieces of Cu(s) (copper) • 7 pieces of Mg(s) (magnesium) • 7 pieces of Zn(s) (zinc) Solutions: • H2O(l) distilled water • HCl(aq) hydrochloric acid • CuSO4(aq) copper (II) sulphate • ZnSO4(aq) zinc sulphate • MgSO4(aq) magnesium sulphate • SnCl2(aq) tin (II) chloride • ZnSO4(aq) zinc sulphate • FeSO4(aq) iron (II) sulphate • • Tweezers • Two Spot Plates • Distilled Water Bottle • Safety Glasses • 1 piece of paper • Pen / Pencil Procedure: 1. Gathered all the required

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    Determining the amount of Water of Crystallization Hydrated to Copper Sulphate Daniel Benda October 11th 2014 Hl Chemistry Block: H Word Count: 1354   Data Collection and Processing: Raw Data: Table 1: Raw data of Trials vs Mass of crucible and contents before and after heating Trials Empty mass of crucible (±0.001g) Initial filled mass of crucible (±0.001g) Final Filled weight of crucible (±0.001g) T1 36.093 43.516 40.783 T2 48.160 56.218 53.143 T3 31.503 44.537 39.705 T4 34.345 38.677 37.082

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    solubility of my solutes. My decided solutes are sugar, salt and copper sulphate pentahydrate. I decided I would be using 100mL of water as my solvent due to the abundance of solutes available and that fact that 100mL is a nice, easy number to work with. I also spoke to Mrs Rach and she informed me she has a surplus of copper sulphate so I don’t have to be careful with how much I use. She also gave me some measurements on how much copper sulphate should dissolve into 100mL of water at varying degrees. It’s

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    sample of copper sulphate using colorimetry. In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate

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    Task 7:  Titrations: Method: 1. Firstly you need to need to measure accurately 0.50g of your copper sulphate solution into a 100cm³ beaker 2. Then add about 50cm³ of distilled water ensuring you continue to stir until crystals have dissolved. Then transfer the solution into a 100cm³ volumetric flask 3. Next rinse out the beaker with small amounts of distilled water and transfer the washings to the volumetric flask to ensure none of the solution is wasted affecting the end result. 4. Once the beaker

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    Concentration of the acid The denser the solution, the slower the reaction. The slower the reaction, the less copper is deposited in the given time period. Everyone used the same amount of copper sulphate solution Current passed through the circuit If it wasn’t constant then the time, intervals wouldn’t be equal. If the current is larger, there will be more electrons flowing around the circuit and more copper will be deposited. The use of a ammeter tells you the current stayed constant Power Supply Effects

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    Completion Date: Introduction We are studying the reaction between zinc and sulphuric acid, the reaction is catalysed by copper sulphate and this experiment is to test whether the amount of drops effect the rate of reaction. Word Equation Zinc(s) + Sulphuric acid(aq) à Hydrogen(g) + Zinc Sulphate(aq) Symbol Equation Zn + H2SO4 à H + ZnSO4 This reaction is catalysed by Copper sulphate (CuSO4) Ionic Equation - Cancel Spectator ion (SO42-) Zn + 2H+ à Zn2+ + H2 For this reaction to work there must

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    Copper Research Paper

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    Copper is a metal, that people obtain from chalcopyrite and bornite ores and minerals, by smelting, leaching and electrolysis, which are chemical reactions. Yet, it belongs to a sub-group of metals called ‘Transition Metals’. Existing as an element, it’s small particles (atoms) are very close to each other (most common state for copper is solid), but aren’t chemically bonded. Consequently, it is a 26th element on the periodic table, meaning that it’s atomic structure consists of 26 protons, and

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    Cufee Industry Analysis

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    Chemistry Assessment Task 2 Identify the metal ore from which copper is extracted. Copper is extracted from chalcopyrite ore, its chemical formula is CuFeS2. Chalcopyrite is a brass-yellow mineral with a chemical composition of CuFeS2. Most sulfide mineral deposits in Australia contain chalcopyrite ore and has been the most valued ore of copper for thousands of years. Describe the mining and extraction process of commercial copper ore deposits Copper can be extracted from the chalcopyrite ore by: 1. Traditional

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    process of extraction of copper varies depending of what ore, copper is being extracted from. Chalcopyrite (CuFeS2) is a sulphide ore and it is one the most common ores of copper. The process of extracting copper from chalcopyrite is a quite complex procedure in which both physical and chemical processes are involved. As chalcopyrite is around 0.5% copper and 99.5% “unwanted rocky material”, the first step to extract copper from chalcopyrite is to increase the concentration of copper in the ore to high

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