emission spectrum that shows colors of different spectrums hydrogen for example shows 4 colors …etc Materials: 1- Benson burner 2- A wire loop ( wake sure it ’s clean ) 3- 4 filter papers 4- 4 Unknown test solid as directed by instructor (potassium ‚ sodium ‚ calcium ‚ barium / chloride ) 5- A beaker 6- diluted HCL ( to clean the wire loop with it ) 7- A spatula
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providing this information in an editable file which can be sent to an instructor. obseRvations The color of the flame is expected to be as follows: Metallic ion Flame color Sodium Na+ Yellow/Bright Orange Strontium Sr2+ Red Potassium K+ Light Purple Barium Ba2+ Green Copper Cu2+ Green Lithium Li+ Red Calcium Ca2+ Orange Unknown Red-Strontium Questions A. All chemical used in this test are binary compounds. What portion of the periodic table is responsible
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Emission Spectra & Flame Tests Intro The emission spectrum is used in modern chemistry to help further studies of wavelengths and the spectrum. When a metal in a compound reacts in a flame and produces a color‚ it helps to show the strongest color in the emission spectrum. The purpose of performing these operations on the flame was to see how different metals would react. Using a spectroscope‚ it is possible to observe the line emission spectrum produced by sunlight‚ artificial light‚ and
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Kinetics of a Reaction I. List of reagents & products 1. 1.0 M Copper(II) nitrate (Cu(NO3)2‚ 0.10 M Hydrochloric Acid (HCl)‚ 0.010 M Potassium Iodide (KI)‚ 0.040 M Potassium Bromate (KBrO3)‚ 0.0010 M Sodium Thiosulfate (N2S2O3)‚ 2% Starch solution‚ Water (H2O) II. Summary of Procedure. Part 1: Find the Volume of One Drop of Solution 2. Fill pipet with 3ml of distilled water 3. Mass a beaker and record 4. Put 5 drops of water into beaker and record
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this experiment you will determine the percentage of oxygen in potassium chlorate. You will calculate the theoretical value from the chemical formula and compare your experimental value to the theoretical value. Background: When potassium chlorate (KClO3) is heated‚ it undergoes chemical decomposition. Oxygen gas (O2) is given off and potassium chloride (KCl) remains as the residue. The equation for the decomposition of potassium chlorate is: 2 KClO3 (s) 2
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iodine (part 2). For part 1 of the experiment‚ this was done by titrating a solution of 50 cm3 of diluted 0.0225M persulphate and 250 cm3 of 0.4M potassium iodine against a 50 cm3 solution of 0.01 M solidum thiosulphate‚ using 3 ml of 2% starch as an indicator. For part 2‚ a solution of 25cm3 of iodine and persulphate‚ and 25 cm3 of 0.04M potassium chloride was titrated against the same amount of thiosulphate. Using the titre values Tt (ml)‚ time (s) and Tinf‚ graphs were plotted in order to
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Determining the enthalpy change for the thermal decomposition of potassium hydrogen carbonate into potassium carbonate. Controlled Variables: 1. Volume of HCl ± 0.5 cm3 (± 2%) 2. Concentration of HCl‚ 3. Same mass of K2CO3 and KHCO3 within specified ranges of 2.5 – 3.0g and 3.25 – 3.75g respectively 4. Same calorimeter used i.e. polystyrene cup is used in this experiment 5. Same thermometer will be used ± 0.10K 6. Same source of K2CO3‚ KHCO3 and HCl Raw Data Results: The raw
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This experiment contains three separate procedures in which Aluminum Potassium Sulfate(Alum) will be melted‚ massed out and mixed with Barium Nitrate‚ along with distilled Water. Procedure one we completed two trials of melting two separate 0.01g of Alum and making a comparison to the literature temperature of 92.5‚ to do this we attached an Alum filled capillary tube to a thermometer and inside a beaker placed over a Bunsen burner. Procedure two consisted of placing 2.00 grams of Alum into a crucible
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down. Verses if the water is hot with salt. (15 points) 4. Use the data from Part 1 of the procedure to complete the data tables and graphs. Answer: Station 1: Potassium Chloride (KCl) Beaker Temperature of water (°C) Amount of KCl at saturation (g) A 5.0 25 B 30.0 12 C 54.8 20 D 70.1 32 Station 2: Potassium Chlorate (KClO3)– Beaker Temperature of water (°C) Amount of KClO3 at saturation (g) A 5.2 20 B 28.7 10 C 43.9 15 D 68.2 28 (3 points) 5. Use the data from Part 2 of the
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The Solubility of Potassium Nitrate Aim: The aim of this experiment is to find out by how much the solubility of potassium nitrate into distilled water increases when the solution is heated‚ and if yes‚ by how much. Hypothesis: According to data on the internet‚ 3.75 × 10¹ moles of potassium nitrate dissolve in 100g of water. I believe this information may be correct. I also believe that as the solute is absorbing outside heat‚ the energy is increased causing it to dissolve both faster‚ with
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