The mixture was decanted again in to the same beaker. Next, we added boiling chips to the liquid and evaporated the solvent over the hot plates under the hood. After the solvent was evaporated and the flask was cooled, we used a spatula to remove a small amount of the crude product and took its melting point. We determined the melting point range of the sample to be 43.0-46.0 degrees Celcius.The crude product was yellow colored when it was warm and orange in color when cooled and sticky. We then recrystallized our sample using 5 ml of warm acetone that was heated on a hot plate under a hood.
In this report I will be looking at the effect of temperature in the solubility of sugar (sucrose) in water when it dissolve in different temperature of water and how long it takes to dissolve. I will also use different scientific explanations to support my findings. In order to do this this experiment I have used three different variables which are:- * Independent (temperature) * Dependant( time taken to dissolve) * Control ( volume of solvent and volume of solute) Equipment needed for the experiment is * 100 ml beaker * Sucrose (sugar) * Timer * Tea spoon * Kettle with boiling water * Thermometer * Ice cubes The methods of this experiment are as follows * First I will boil the water at 100 degree and then put the required amount of boiled water in the beaker. * Use thermometer to measure the temperature and record and then add the required amount of solute and start the timer and stirring until it completely dissolves. * Document the time it takes .I will repeat the process three times and take the average amount of time it took for the solute to dissolve in the solvent of high temperature.
Record the initial temperature of the liquid in the calorimeter. Watch the thermometer until maximum temperature is achieved. Weigh out 2.0g of NaOH pellets. Record the temperature of the distilled water in the calorimeter until the temperature is constant then add all of the pellets at once. Gently stir the pellets until the acid is dissolved by shaking the the apparatus.
As we know the equation C1V1=C2V2, we can get a set of concentration (g/L) of different ratio of Red #40. Introduction The goal which the experiment designed to achieve is perform a Beer’s law analysis to determine a solution’s concentration, and determine a percent composition. To build the calibration curves for each food dye, we need to measure the absorption of different solutions of known concentration. One rather quick way to make a solution of known concentration is by exact dilution from a more concentrated solution of known concentration. We rinsed a pipette with some of the sample, filled curettes between 2/3 and 3/4 full with the samples, put a curette in the cell holder and make absorbance measurements.
* 12.00 mL of the K2CRO4 solution was slowly poured into the beaker containing the Pb(NO3)2Vsolution while stirring the Pb(NO3)2 solution. * The K2CrO4 beaker is rinsed with 10 mL of 5% nitric acid solution and added into the beaker. * The beaker is heated on a hot plate in the hood for 2-3 min. * Our professor demonstrated the correct filtration technique. * The mass of a piece of filter paper is determined to the nearest milligram.
Materials and Methods Materials The compounds used in this lab are listed in the table below: Procedure We boiled 2 NoDoz tablets in grinded form with 60 mL of water in a 100 mL beaker and allowed it to cool to room temperature after it had been sitting on the hot plate for 5-10 minutes. Next, we performed a hot gravity filtration by pouring the hot aqueous solution of water and NoDoz (caffeine and insoluble binder) through a large Buchner funnel into an Erlenmeyer flask. We discarded the collected insoluble binder collected inside of the Buchner funnel and performed an extraction by mixing the aqueous solution collected in the Erlenmeyer flask (aqueous solution of water and caffeine) and 15 mL of methylene chloride in a separatory funnel and swirled until the layers had separated to form an aqueous layer on top and an organic layer containing the solvent and caffeine at the bottom of the funnel. We drained the lower layer into an Erlenmeyer flask and repeated the extraction. Next, we added anhydrous sodium sulfate to the Erlenmeyer flask, which contained the combined organic layers of the 2 extractions,
I then poured the mixture on to a solid white piece of paper. I then used a magnet wrapped in clear plastic bag to separate the iron from the mixture. I weighed the iron and calculated and recorded the mass in table 1. I put the remaining mixture in a beaker with 50 mL of distilled water and heated to a boil and removed, then poured the liquid from the beaker into a paper cup. I then added 15 mL of distilled water and heated to a boil and removed, then poured the liquid from the beaker into the same paper cup that held the previous liquid.
the purpose of this is to properly identify the metal given to us. In this experiment we added heat to a container of water. meanwhile we took the mass of our metal sample. We then placed the metal sample into a glass test tube and placed the test tube into the boiling water. We measured out 100 mL of water and transfered it to a styrofoam cup from our graduated cylender.
Also, we watched as the water boiled and made observations as the temperature as it started to boil. This is done on a Virtual Lab. Materials: (Virtual Lab) * Water * Ice * Water-heating device or heater * Metals(Aluminum, Steel, Copper, Lead) * Electrical Balance Procedures: SPECIFIC HEAT OF METALS: * Weigh the mass of the metal samples * Fill up the calorimeter to 100mL. It should be at 25C * Heat up the Aluminum Sample to 200C * Drop the Aluminum Sample in the water and record the temperature changes. * Repeat with the rest of the samples.
Once dissolved, 24.9734 (± 0.0045)mL of acid was pipetted into an Erlenmeyer flask along with 25mL of cool (recently boiled) distilled water. Three drops of acid-base indicator, phenolphthalein, is added to the acid solution. Acid is titrated with the unknown base from the burette as the Erlenmeyer flask is consistently being swirled. Near the endpoint of 24mL, drops of base are added to the acid solution until a light pink colour persists within the solution. Titration is repeated 3 more times in order to achieve more accurate results.