Students first prepped for the lab by cleaning out the crucible. Three boiling chips were added in the crucible once it was wiped out with a paper towel. The crucible was then placed on a clay triangle two finger widths above the Fischer burner. After 10 minutes of the crucible being directly under the flame, the it was clean and students allowed time for it to cool down. Next, the students from then on used tongs to transport the crucible from weighing it and back to the clay triangle.
In addition, when heat is applied, 36.1% of water is lost from the hydrate. Using theoretical yield with the average atomic masses, I calculated the molar mass of the copper sulfate hydrate (CuSO4 ᐧ 5H2O) to be 249.685 grams, then found the percentage of water lost from the hydrate by dividing 5 water molecules, 90.0764 grams, with the entire hydrate. After doing that, 36.1% is the actual percentage of water that was lost when heat is applied to the hydrate. However, with the experiments, we had lost only 34.5% of water, so it is important to understand how to determine the percent of water in a hydrate that was lost, but also the error percent because knowing the percent error will help me understand what was done wrong, so next time more accurate results would be concluded. For example, because of the 4.4% error, some of the weight may have been lost due to heat circulating in the evaporating dish after applying heat to the hydrate.
In this experiment, four white powders were tested. After visually inspecting the powders, Powder A appeared to be white, lumpy, and possessed no lust, Powder B appeared to be white, soft, and lumpy, Powder C appeared to look smooth, white, and soft, and Powder D appeared to be lumpy, solid, and whitish-yellow. The materials that were utilized in this lab were cornstarch, baking powder, baking soda, powdered sugar, spot plate, scoopula, dropper, water, vinegar, iodine, toothpicks, and paper towels. The physical property that was observed was solubility, the ability of something to be dissolved, and the chemical property that was observed, reactivity, is the tendency of a substance to undergo chemical change. Knowing both chemical and physical properties of the substances is important because they give more information about the identities of the substances and back up observations
A hydrate is a compound, where water molecules are chemically bounded to another compound or element. An anhydrate is the substance remaining after removing water from a hydrate. The hydrate in this lab was Copper Sulfate. The hydrates formula is CuSO4 times xH2O. The purpose of this lab was to pull the water from a hydrate to expose the anhydrate and calculate what the hydrate is by finding the formula for the
The overall purpose of this lab was to develop a lab procedure in order to separate and measure the mass of each containment obtained the provided sample. In addition, this experiment was conducted in order to provide the EPA with a plan to remove all contaminants from a heterogenous mixture which purifies the water, making it accessible for the society. Furthermore, the sample consisted of the following contaminants, sand, rock, wood, plastic, salt, water, and an unknown metal. When it came to separating the contaminants, the wood and plastic were taken out through the use of tweezers, while the rocks were separated by decanting the mixture of sand and rocks from the water.
Finding the empirical formula for hydrated copper sulfate using calculations to find the amount of each element present in the copper ion, sulfate ion, and water while also comparing the empirical formula to a literature value. Christian Cooper Alexis Powers CHM1210-18M/Gregory Bowers 11-5-15 Purpose: 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.
Water is added to the crucible in order to neutralize the magnesium nitride that was subsequently produced through heating. The magnesium has completely reacted when sparks stop being produced. Two more sources of error include not allowing for proper cooling and heating times, and not adding water after the magnesium’s first heating.
The goal of this experiment is to find out what is the identity of the unknown hydrate? To answer this question first, we should know what a hydrate, and how to identify a hydrate using the law of constant proportions. A hydrate is a pure substance because it contains water molecules embedded in its crystal structure that does not vary. By heating the unknown hydrate, we can calculate the mass of the hydrated, and the percentage of water in the hydrate.
The chemical state of the water varies widely between different classes of hydrates, some of which were so labeled before their chemical structure was understood. 2: Specific to your hydrate. What are common uses of your hydrate? Magnesium sulfate heptahydrate, or MgSO4
Equipment: List the equipment you need to conduct the experiment in alphabetical order. Draw a labeled diagram clearly showing what the equipment is and how it is used, preferably large and easy to understand. Procedure: List the steps you follow to conduct the experiment. -Every
- A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.
The objective of the lab Mixed Substances, is to see how properties of individual substances compare with properties of mixed substances. This means comparing one item to a pair of items. The cornstarch is a white, fluffy substance with no smell to it. Also the cornstarch is lightweight and soft to tough. The second substance is water.
The first step of the creation of verdigris was preformed using the following reaction (1): 4CuSO4*5H2O(aq) + 6NH3(aq) CuSO4*3Cu(OH)2(s) + 3(NH4)2SO4(aq) + 14H2O(l) Based on this chemical equation, four moles of hydrated copper sulfate reacted with six moles of ammonia to produce a precipitate of copper sulfate tribasic along with aqueous ammonium sulfate and liquid water. It was known that a chemical reaction was occurring when the ammonia was being added via the color change from light blue to dark blue. The precipitate formed from this solution was acquired via vacuum filtration, which involved the solution being separated from the precipitate via air pressure flowing out of the flask. The air pressure flowing out of the flask was caused by a faucet that was running water which was attached to a tube that was attached to the collection flask.
Weight a clean, dry, porcelain evaporating dish on the electric balance and record this mass on an appropriate data table. If the crucible needs to be washed before use, then heat the crucible in the Bunsen burner flame for a few minutes and remove any residual water. Then allow it to cool before continuing. Fill the crucible about 1 gram with the hydrated salt and reweight. Assemble the ring stand, ring, clay triangle, and Bunsen burner