Safety goggles were put on‚ hair was tied back and sleeves were rolled up. One cm of CuSO4·5H20 was added to a cleaned dried test tube. The test tube was heated until no furthered changes were observed. All observations were recorded then the substance was then disposed of in the waste container provided. 1/3 of a test tube was filled with
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Introduction: Molarity (M) is used to determine concentration. Molarity is found by dividing the number of moles of a solute by the volume of the solution in liters. Multiple series of solutions with different concentrations can be used by diluting the concentration. The dilution technique is: Number Moles Concentrated Solution = Number Moles Dilute Solution. An instrument called a spectrophotometer detects the amount of light that passes through the sample and the percent transmittance can be recorded
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8. Wash your hands and return safety equipment. Observations: Refer to the back of pre-lab Discussion: 1. Formula for Zinc’s reaction: Zn + CuSO4 ZnSO4 + Cu Formula for Tin’s reaction: Sn + CuSO4 SnSO4 + Cu Formula for Magnesium’s reaction: Mg + CuSO4 MgSO4 + Cu Formula for Iron’s reaction: Fe + CuSO4 FeSO4 + Cu 2. For Zinc‚ during the chemical reaction it was decaying and turning into a different colour. My observations concluded to
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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using metals‚ this is important. Manufacturing cars‚ or producing construction supplies all ties in with the activity series. Without it‚ cars or buildings could very well be rusting and dissolving around us. Metal/ Cation or Solution HCl H2O CuSO4 ZnSO4 MgSO4 SnCl2 Fe(NO3)3 Cu NR NR NR NR NR NR NR Mg R NR R R NR R R Sn R NR R NR NR NR NR Zn R NR R NR NR R R Fe R NR R NR NR R NR Steel (FeAl) R NR R NR NR R NR Table 1 : Predictions Metal/Cation Or Solution
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TITLE : The copper cycle IN TRODUCTION The purpose of the experiment is to recognize that change of state‚ change in colour‚ formation of a precipitate‚ or the evolution of heat are associated with a chemical change; to study reactions of copper. Copper is an element that can be found in nature in a variety of different compounds. The most common natural ore is the sulphide‚ known as chalcocite‚ Cu2S. This mineral is an important source of copper metal because it is about 80% copper by
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Stoichiometry lab By: James Stewart Purpose: To calculate mole ratios Introduction: There are two types of chemical analysis; qualitative analysis which is the identification of a substance present in a material‚ and qualitative analysis which measures the amount of the substance. In this lab‚ you will perform a quantitative analysis of a two-step reaction. Copper(II) oxide will be synthesized from a known mass of copper(II) sulfate pentahydrate. Using the relationship of the balanced equation
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understand that: 1. Matter is made of tiny particles. 2. There is empty space between the particles. 3. The particles are in constant motion. 4. There are forces that act between the particles. METHODOLOGY Materials and Apparatus CuSO4 (size of a rice grain) Phenolphthalein indicator Ammonia solution (1 M NH3) Iodine crystals (I2) Graduated cylinder Procedure: Part 1 Diffusivity 1. Place a small
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having the copper (II) oxide solid used was washed with 6.00M H2SO4 thus having a reaction of: CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l) It was noted that from the colorless or clear filtrate‚ it changed into blue. Also‚ there was a formation of blue precipitate when 6.00M H2SO4 was added. The CuSO4 solution obtained was then added with zinc dust having a chemical equation as follows: CuSO4(aq) + Zn(s) ZnSO4(aq) + Cu(s) During the addition of more zinc dust‚ it was observed that there were bubbles
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Procedure: 1. In the first table‚ write down a description of what KSCN and Fe(NO3)3 look like. 2. Clearly mark the 4 beakers‚ 1 thru 4‚ to ensure you know what substance is added to each beaker. 3. Observe a solution of potassium nitrate KNO3. Describe the appearance of the solution in the first table. 4. Put approximately 25 ml of 0.0020M potassium thiocyanate solution‚ KSCN‚ in
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