Then an estimated (by trial and error) 1-3 grams of hydrated copper sulfate was added to a crucible with the lid on top. The total mass of the hydrated copper sulfate was recorded by subtracting the total mass of the crucible, lid, and sample from the mass of the crucible and lid (described in table 1.3). By attaching the wire triangle to the ring, the crucible was able to sit securely while having the bunsen burner underneath. Lighting the burner once again, each substance was heated for several minutes until estimated that the compound had changed color. Once a prevalent color change had been observed at approximately 4 minutes (blue green color) the crucible was set on the counter using the tongs to cool for approximately 5 minutes. The appearance after this period resulted in another color change back to white. The crucible, lid, and hydrated copper sulfate was weighed again to calculate the mass of water lost by dehydration (described in table 1.3). This was done by subtracting the final mass by the initial mass of the crucible, lid, and compound. The mass of the crucible would remain unchanged while the mass of the compound would be altered. This trial was repeated 3 times and 1 extra set of data was taken from 2 separate groups to include
Materials: The materials that I will be utilizing during these experimentations are three to four ice cubes, one cup for measuring, six unblemished cups, one stopwatch, one hot water source, three tablets of Alka-Seltzer, one thermometer that measures from negative
A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved. While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved. The magnetized zeolite was then cooled for 5 minutes. For both zeolite and magnetized zeolites, the solutions were placed in two centrifuges with equal amounts of solution and placed in both tubes. The tubes were placed in the centrifuge for 10 minutes at 5000 rpm. The liquid in the tube after the centrifuge was poured into a 200 mL waste
Process: get and wear goggles, set up a Buchner funnel and flask and measure its mass. Put the foil into a 250 mL beaker. Get 25 mL of 3M KOH solution, add 5 mL KOH solution into the beaker and stir the beaker. Keep the reaction proceeding until all of the foil is dissolved and use ice bath to make it cool down. Pour the reaction mixture through Buchner funnel and filter flask setup, rinse the filter paper with a small amount of distilled water. Wash the beaker with distilled water and run the rinse solution through the Buchner funnel. Put the filtered liquid back into the beaker, then, clean up the Buchner funnel and filter
In the lab “All That Glitters” the objective that was focused on during the lab was calculating the density, volume and mass of various substances. The method that was used in finding the volume of the samples is called the displacement method. This is a process where the volume of the water in the graduated cylinder is calculated before and after the sample is placed. In this lab, the goal of the experiment was to identify and come to consensus about what the unknown substance might be. For this experiment, the required materials were ten pre and post pennies, unknown sample, graduated cylinder, weigh boat, water, paper towels and a weighing scale. To start off, dry the pre pennies, post pennies and the unknown substance completely with paper
Regarding reaction 4, the duration was changed to 480 seconds. After the Styrofoam cups were restacked, 100mL HCl was added. The lid was added and the probe was instered. A watch glass was weighed, then weighed again after scooping on 1.0g MgO. After 3-4 readings were recorded, the MgO was added with the spatula, which was stirred constantly with the stir bar. The watch glass was weighed again with the remains of the MgO.
To begin, there are several different goals, techniques, and claims to note in the experiment involving hydrated copper sulfate. The overall goal of this experiment is to find the empirical formula and compare it with a literature value. Yet, in finding the empirical formula of hydrated copper sulfate, there are several process for it to get through, like finding the percentages of copper, water, and finally sulfate. One possible claim
In trial one, the weigh boat was first zeroed on the scale. Five grams of the white unknown mixture was measured on to the weigh boat. A two-hundred and fifty milliliter(ml) flask was zeroed out on the scale. Fifty milliliters of HCl was put into the flask and weighed. The unknown mixture was poured into the HCl while
This equation will provide for the ability to calculate the moles of both the given and desired substances, which can be divided to find the theoretical yield. An experiment will then take place: first, it is important to properly clean a working station and to wear goggles and a lab coat. A beaker can then be filled with 10 mL of of water before gathering 2 g of solid copper (II) sulfate pentahydrate, 2 mL of 6 molar hydrochloric acid, and approximately .25 g of aluminum foil as provided; a scale can be used to keep these measurements accurate. Using a stirring rod, stir the hydrochloric acid into the water before placing the solid copper (II) sulfate pentahydrate into the beaker of water. Let the hydrochloric acid and solid copper (II) sit in the water for two minutes as the next portion of the experiment is prepared. Heat up a heating pad to 275 degrees °F before placing the beaker on top of the heating pad. Using a pair of tweezers, carefully drop the pieces of aluminum foil into the water. Allow mixture to sit on the heating pad until dissolved, constantly stirring. Once completed, turn the heating pad off. Measure the beaker on the scale once more and subtract the weight of the 10 mL of water as well as the measurement of the
As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear. The glass rod was used instead of the metal spatula because the metal from the spatula could have reacted with the copper ions in place of the aluminum wire, which would have interfered with the calculations of the solid copper’s
The procedure for this lab is fairly simple. First fill up an erlenmeyer flask with 50 mL of warm tap water, then put it on a hot plate and bring it to a boil. Inside a tray to catch any spills set up a ring stand about 6 inches high. After the water has started to boil remove it from the hot plate and let it cool slightly by setting it on the lab table, after about a minute place the rubber stopper in the flask and carefully flip the flask over and place it in the ring stand. Rub an ice cube on the top of the flask and watch it boil. Then clean up the lab when you are
As a young man, Ira Remsen was intrigued by science, leading him to perform an experiment that he saw in a textbook. This experiment involves a series of chemistry topics, triggered by the reaction that occurs between nitric acid and copper. The experiment involves an elevated flask, plug, a hose, and a container of water the set up is diagrammed below:
This particular experiment is done as part of my Organic Chemistry course. I was really interseted to do this experiment and I worked out well in this experiment.
Copper is essential for all life, but only in small quantities. Copper appears in the periodic table at the top of Group 11 in the 4th period above silver and gold. Copper is one of the most important metals. Specifically, it is a transition metal on the periodic table. Copper is reddish with a bright metallic lustre. It is malleable, ductile, and a good conductor of heat and electricity (second only to silver in electrical conductivity). Its alloys, brass and bronze, are very important.
Divide the mixture into equal halves of 25g weighed using an electronic scale to ensure accuracy, using a different crucible