To find the formula of hydrated copper(II) sulfate Introduction In this experiment, the water of crystallization is removed from hydrated copper(II) sulfate. The mass of water is found by weighing before and after heating. This information is used to find x in the formula: CuSO4.xH2O. Note that x must be an integer (a whole number). Diagram Method Safety: Wear eye protection Find the mass of your crucible. Place 2–3 spatulas of blue copper(II) sulfate crystals in the crucible and weigh. before Heat until the crystals have gone completely white, but do not heat so strongly that they start to blacken. Allow to cool then reweigh. after Once you have made all measurements: This reaction …show more content…
Crucible and anhydrated copper sulphate 28.84 Measured by using a weighing scale Hydrated CuSO4 2.04 Found by subtracting the weight of step B. and step A. B. - C. = Hydrated CuSO4 29.50 - 27.46 = 2.04 grams Anhydrated CuSO4 1.38 Found by subtracting the weight of Step C. and step A. C. - A. = Anhydrated CuSO4 28.84- 27.46 = 1.38 grams H2O 0.66 Found by subtracting the weight of Step B. and step C. B. - C. = H2O 28.84 - 29.50 = 0.66 grams Table 3: Showing Process Performed of How to Find the Mr, Moles and Empirical Formula from the Compounds Anhydrous CuSO4 and H2O Compound Processing: Explanation of how I figured out the calculation Process Anhydrous CuSO4 H2O a. Mass in grams (g) 1.38 0.66 Refer to Table 2. process b. Molecular Mass (Mr) (Add the Ar of each element together) 160 18 Molecular mass of Anhydrated CuSO4: Cu = 64 S = 32 0 = 16 x 4 = 64 CuSO4= 64+32+64 CuSO4= 160 160 is the molecular mass of CuSO4, this is done by adding up each Ar of each element in the compound CuSO4 together Molecular mass of Anhydrated H2O: H = 1 x 2 = 2 O = 16 H2O = 2+16 H2O = 18 18 is the molecular mass of H2O, done by adding up each Ar of each element in the compound H2O …show more content…
To re iterate this process is written on table three, finding the formula of hydrated copper(II) sulfate, it was processed by first finding the molecular mass of each compound; 160 Mr for CuSO4 and 18 Mr for H2O, in other words each Ar of each element was added together to form the Molecular mass. Next, by dividing the molecular mass by the measured mass, on table two, the number of moles was processed; 0.008625 moles for CuSO4 and 0.03666666667 moles for H2O. Finally to find the mole ratio I divided each number of moles by the smallest number of moles, being 0.008625. Once after rounding the divided number I concluded to one molecule of CuSO4 and four molecules of
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
Purpose: The purpose of the lab was to perform a series of chemical reactions in order to transform copper within different reactions in order to start and end with solid brown copper.
In the first part of this project, two cation elimination tests and one cation confirmation test were performed. 10 drops of 4 cation solutions: potassium, zinc(II), copper(II)
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
* Note the mass down in the table at the end of the first page.
Using the previously calculated Kf, the molar masses of unknown substances A, C, and D were able to be calculated. However, given that the original Kf was slightly larger than the theoretical value, the molar
Mass of KClO3 = Mass of crucible, cover and KClO3 (Step # 3) - Mass of crucible and cover (Step # 1)
In this experiment there were eight different equations used and they were, molecular equation, total ionic equation, net ionic equation, calculating the number of moles, calculating the theoretical yield and limiting reagent, calculating the mass of〖PbCrO〗_4, calculating actual yield, calculating percent yield (Lab Guide pg.83-85).
7.) After you have heated them to the right temperatures, pour the excess water into a dry evaporating dish. ( Be sure not to get any of the substance in your solution. )
It is essentially using the the mass of the product to figure out the original mass that we are looking for. Thus, the purpose of our experiment was to compare the final mass in our reaction to the initial mass and determine the change in mass. In our experiment, we utilized the hydrate cobaltous chloride. Hydrates are crystalline compounds in which one or more molecules of water are combined with each unit of salt. Cobalt (II) chloride hexahydrate is an inorganic compound which has a deep rose color in its hydrated form.
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
1. Obtain a clean, dry crucible and lid, then heat them for approximately 5 minutes over a Bunsen burner
Once the alloy has been quenched in this condition it is now stronger because all of the 4% of Copper has been dissolved into the solution and ductile because the brittle crystals of the Cu〖Al〗_2 compound are now absent.
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
of Copper Sulphate. To do this I plan to work out the amount of water