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Equilibrium Lab Report

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To find chemical equilibrium, the following chemical equation is used in the experiment: Fe3+(aq) + SCN-(aq)  FeSCN2+(aq). When iron (III) and thiocyanate react, thiocyanoiron (III) is produced. When the concentration of all ions at equilibrium are known, the equilibrium constant can be calculated by dividing the equilibrium concentration of the reactant by the equilibrium concentration of the products. In this experiment, four equilibrium systems containing different concentrations of three different ion types (Fe(NO3)3, KSCN-, and distilled water) are made and used to determine equilibrium concentrations. The equilibrium concentrations are used to calculate the concentration that all of the components of the chemical equation are at equilibrium. Using a colorimeter or spectrometer to determine the equilibrium concentration of FeSCN2+(aq) and …show more content…

Prepare the standard solution of FeSCN2+ pipetting 18 mL of 0.200 M Fe(NO3)3 in a 20 * 150 mm test tube labeled five. Pipet 2 mL 0.0020 M KSCN into the test tube and stir. 6. Prepare a blank. Fill the plastic cuvette ¾ full with distilled H2O. Properly clean the cuvette and handle only by the top ribbed edge while wearing gloves. Dislodge any bubbles by tapping on a hard surface and position the cuvette in the spectrometer so light passes through the clear side. 7. Connect the spectrometer to Labquest and select a new file. Calibrate the spectrometer by placing the blank inside and allowing the lamp to warm up. The optimal wavelength for the standard curve and data collection can be started at this stage. Empty the blank and use the solution from test tube one to rinse the cuvette twice. Fill it ¾ with solution one, wipe the outside, and place it in the spectrometer. 8. Start data collection and display a full spectrum graph. Stop the data and the wavelength of maximum absorbance will be identified. Under the Meter tab, select mode and then events with entry. Type in the name as concentration and the units as

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Coursework Equipment List • Boiling tubes (8) I will use these because this is where I will mix both the sodium carbonate and the strontium nitrate in order to form the precipitate. I need 8 because I am going to add 8 different amounts of strontium nitrate (1-8cm³) to the 8cm³of sodium carbonate. • Measuring cylinder (1) I will use this to measure the 8cm³ of sodium carbonate and the varying amounts of strontium nitrate to put into the test tubes. • Sodium Carbonate (enough to fill 8 boiling tubes with 8cm³/64cm³)

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The cuvette was placed in the spectrophotometer with the arrows, on both the cuvette and the SpectroVis, facing the same side. After the recording, the cuvette was removed from the SpectroVis and the content was poured back into the original volumetric flask. The absorbance as well as the maximum wavelength of each solution was recorded in Table 3 and

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The colorimeter must be set to the correct wavelength setting. In this experiment, the wavelength must be set to blue so it can

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Step 2: Mix both test tubes , shake gently and time the reaction. Step 3: The same step as procedure 1, and step 3 which is to record the observed color step 4: use the palette/color chart to help you identify the observations you make. Safety precautions: Pull your hair back Safety eye goggles Closed toe

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Fill each cuvettes with its respective solution. Turn on the spectrophotometer, so it can warm up then calibrate it to 0% absorbance. Put the corresponding extract blank and set the spectrophotometer to 100% transmittance, then calibrate it to 540 nm. Once catechol is added in the cuvettes, make sure the solution is mixed. Place carrot cuvette in the spectrophotometer and record the resulting transmittance.

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That is where stoichiometry comes along, which is the quantitative relationships or ratios between two or more substances undergoing a physical or chemical change in a balanced equation. It identifies the mole ratio between reactants and products. To understand stoichiometry you have to understand the products and reactants, which involves how to solve balanced reactions. This allows chemists to determine how many moles of a product will be produced from a specific number of moles of a recant or how many moles of reactant are needed to produce a specific amount of a product.

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Before starting the heating process, measure the weight of the crucible with its cover first and then tare the balance, and after that adding about 1 gram of the sample to the crucible with its cover, and then weigh it. Moreover, it is possible liberating harmful gases during the process of heating; therefore, being careful is important. The heating process ends when this sample changes the color to brown because water of hydration is removed to the sample. Additionally, give time to the small cool down and measure its weight. Next, transfer the sample to a 50 mL beaker and mixes with distilled water, which gets by rinsing the crucible with its cover in 8mL, so the solution is generated.

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This type of lab heavily utilizes the concepts of stoichiometry. Stoichiometry looks into the relationship between the relative amounts of substances that are part of a reaction. You can also use stoichiometry for unit conversions, in this case, moles. Moles are a vital unit of measurement that is used to calculate and compare large quantities of small things. Chemists use moles rather than mass when determining relationships between multiple substances because they work with extremely small particles, so using the mass wouldn’t be productive.

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Continue to heat the solution until it reaches about 55℃. Using the test tube holder, transfer the liquefied solution tube to the 25℃ water and record the temperature at 30-second intervals using a clock or stopwatch using a pencil until the solution reaches 35℃ or close to the temperature due to experimental error. While cooling, gently stir the solution using the thermometer until the solution begins to solidify. Once all the data is collected, reheat the solid solution tube in the warm water until it melts and remove the thermometer and wipe it off to avoid the solution adhering to the thermometer. After the data has been recorded, clean-up the lab station and put away the lab

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A spectrophotometer is used to read the absorbance value of the cations in a flame that emits a photon read by the machine. Different elements will emit different lengths of photons which in turn produces an absorbance value. The absorbance values are then plotted on a calibration graph to determine the unknown concentration. EDTA titrations require much less equipment since it is more of a chemical test. An indicator EBT is added to a known volume of your water sample and should turn blue.

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Mika Nijhawan 9/29- 10/10 2 MENTOS AND SODA LAB REPORT State the Problem Does the type of soda affect the size of the explosion, after mentos are added? Develop a Hypothesis If seven mentos to a 2L bottle of Diet Pepsi, then it will create the biggest geyser out of Coke, Fanta, & Root Beer because Diet Pepsi has potassium benzoate, aspartame, and the carbonation which react to mentos. Design an Experiment Materials List: 1 clear test tube 35 original flavored Mentos candies (2 1/2 rolls) 1 3x5 index card 4 2L bottles of soda (all different flavors/types) 1 2L bottle of soda water 1 100 mL graduated cylinder 1 400 mL beaker 1 pair of tweezers (preferably large) 1 small container Procedure: Stack seven mentos in the test tube When given permission take the test tube, soda bottles, index cards, and the remaining 25 mentos, to the designated area Place one of the four soda bottles on a flat area Open the soda bottle and place the 3x5 index card over it With the index card over the soda bottle, flip the test tube over and place it on the index card, so the test tube is lined with

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Introduction: The objective for the lab was to determine properties of materials by using a tension test. The properties that were determined was Young’s Modulus, ultimate tensile strength, and yield strength. Three aluminum alloys were tested. The first was the AA 2024 , which is high strength used in aerospace applications.

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