Flame Test Laboratory Report Introduction The purpose of this lab is to observe and identify metallic ions‚ using flame tests. The traditional flame test originated when Robert Bunsen invented the Bunsen burner to test two new alkali metals he and his partner had discovered. “A flame test is an analytic procedure used in chemistry to detect the presence of certain elements‚ primarily metal ions‚ based on each element’s characteristic emission spectrum” (Flame Test 1). Using this test‚ an element
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beakers contain the same compound. You may try some of the followings: * Dissolving in water * Dissolving in different chemical solution * Heating both substance to see if they come out with different results * Doing the flame test for both solution to see if they can come out with different results * etc * b. Would it be easier to prove that the compounds are the same or to prove that they different? Explain your reasoning. It is easier to prove that they
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Method 1. Sterilise all of your equipment with ethanol‚ blue flame or disinfectant if you can flame it. 2. Collect all equipment together ensuring you collect your goggles and gloves as you are using a flame and gloves and goggles are part of safety precautions. (don’t wear gloves with messing with Bunsen burner only goggles‚ but use gloves when messing with chemicals ensuring goggles on all the time) 3. Clean your surface with disinfectant to sterilise your lab work surface‚ this will prevent
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we recorded their mass. Then we measured 0.7 to 1.7 g of CaSO4.2H20 and added it into the crucible and recorded its combined mass. Next we placed the crucible above the burner flame and heated thoroughly for 4-8 minutes to drive off the all the water in the compound. After 8 minutes we removed the crucible from the flame and allowed it to cool to room temperature. Finally‚ we recorded the mass and calculated the amount of mass for both the anhydrous compound and the water. We repeated this experiment
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How to Carry Out Aseptic Techniques in a Batch Culture and in the Laboratory | | | | | | | | | |The batch vessel should be sterilised beforehand using steam. The nutrient medium that is added to the vessel |
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substitution reactions that are performed in organic labs. In this experiment 1-butanol was converted into 1-bromobutane by an SN2 reaction. The ending result of the experiment was to test if the product was correct by using a flame test that colorizes the product. The flame test turned green which in this case was an overall
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Flame test: - Clean wire loop - Dip the tip of the wire loop into solution (If solid‚ dip the tip in DIW then dip the soaked wire loop in to the solid) - Proceed to placing the tip into fire (from Bunsen burner) - Observe - Na+ = bright orange -Cu2+ = green - K+ = Violet (Can be masked by Na+) - Ca+ = Brick Red - H4N+ = no color Cobaltnitrite test for K+: -Heat NH4+ off -In a small test tube/vial‚ or spot plate and place 10-15 drops of solution to test -Then add a drop of 6M HAc and
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If the food is likely to melt when heated put it on a teaspoon instead of on the needle. f. Light the food using a Bunsen burner‚ and immediately hold it about 1 cm below the test-tube and make sure it is above a heat resistant mat. If the flame goes out‚ quickly relight it. g. When the food stops burning‚ stir the water with the thermometer and record the temperature. h. If there is a significant amount of unburnt food left on the needle‚ re-weigh this and record the mass remaining
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closed shoes & safety glasses.Dispose of contaminated bottles in appropriate‚ labelled contaminated waste container | 95% alcohol | Highly flammable.Irritant to eyes‚ respiratory system & skin. Toxic if ingested. | Keep away from naked flame. Keep bottle closed when not in use.If alcohol in bottle ignites place lid on bottle.In case of fire on bench cover with fire blanket.Inform laboratory staff if spill occurs | Nutrient agar plates | Non-hazardous | Wear personal protective clothing
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Flame Tests 12.01.2010 19.01.2010 Introduction The normal electron configuration of atoms or ions of an element is known as the “ground state”. In this most stable energy state‚ all electrons are in the lowest energy levels available. When atoms or ions in the ground state are heated to high temperatures‚ some electrons may absorb enough energy to allow them to “jump” to higher energy levels. The element is then said to be in the “excited state”. This excited configuration is unstable‚
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