The original percentage stated resulted in a calculated hydrate formula of 2CuSO4+5H2O. Engage students in your virtual classroom with Prezi … So you will get 1 copper sulfate and your amount of water should be larger than 1 when you divide by the smallest. 5. Mass the watch glass and anhydrate. in your lab notebook. 8. a) If the hydrate was heated too quickly, and some of it was lost or was splattered out of the container, this would drive out the water only leaving behind the copper sulfate anydrate CuSo4, which is white in color. In order to determine this information we heated the salt to get rid of the water. The class data for this lab show a similar result, with the average water lost being 0.365g and the percentage by mass of water in the compound being 30.3%. copper (II) sulfate.Break up any large crystals before placing them in the crucible. In solution, the partial charges of water molecules, called dipoles, are 2. We were trying to determine the empirical formula of the copper sulfate. A hydrate like cupric sulfate is any compound containing water. After the reaction occurred, the products were copper and zinc sulfate. Heat the hydrate on hot plate until all blue is gone. The reaction involved the reactants copper sulfate and zinc. When all the water has been evaporated from a hydrate it is known as an anhydrous compound. This salt exists also in a hydrous form. Lab Determining the Chemical Formula of a Hydrate - Free download as Word Doc (.doc), PDF File (.pdf), Text File (.txt) or read online for free. Copper(II) sulfate pentahydrate is the pentahydrate of copper(2+) sulfate.A bright blue crystalline solid. PRE-LAB ASSIGNMENT. Allow watch glass to cool. The products of the reaction were solid copper and aqueous zinc sulfate. Record all weighings accurate to the nearest 0.01 g. Carefully add a few drops of … I then found the number of moles of water and divided by the number of moles of copper (II) sulfate in order to get the ratio of water to copper (II) sulfate. Its formula is CuSO 4 5H 2 O. The copper(II) sulfate should be provided as fine crystals. Copper Sulfate Hydrate[1] - Free download as Word Doc (.doc), PDF File (.pdf), Text File (.txt) or read online for free. I found this by multiplying the grams of water evaporated by the conversion factor of 1 mole/18.01528g (the molar mass of H2O). An important hydrate is calcium sulfate dihydrate, CaSO 4 2H 2 O. I want to determine the chemical formula for a hydrate. Lab #4: Identification of an Unknown Hydrate of Copper (II) Sulfate Author: ncooke Last modified by: Office 2004 Test Drive User Created Date: 3/12/2007 10:34:00 PM Company: Conejo Valley Unified School District Other titles: Lab #4: Identification of an Unknown Hydrate of Copper (II) Sulfate Mass of cooled evaporating dish+ Anhydrous copper (II) sulfate (after heating) Final Color of hydrate. If large crystals are used, these should be ground down before use by students. Feb. 3, 2021. It contains a copper(II) sulfate. Carefully add a few drops of water to the watch glass and observe. Initial Color of hydrate. When the precipitated copper was washed, zinc ions were removed. Anhydrous copper(II) sulfate is the chemical compound with the formula CuSO 4. We were trying to determine the empirical formula for copper sulfate and magnesium sulfate. Some errors in the chemistry lab result from an unclear definition or expectation of what the experiment is supposed to record. Mass the watch glass and hydrate. This is because when copper sulfate is dissolved in water, it exists as the free ions Cu²⁺ and SO₄²ˉ. From this data we determined the empirical formula for the 2 compounds. chemical formula of copper (II) sulfate hydrate I found to be CuSO 4•5H 2 O. I determined this number by finding the number of moles of copper (II) sulfate. Application Questions: 4. Copper sulfate was aqueous and zinc was solid. What ions did you remove when you washed the precipitated copper? Add a small scoop of blue hydrate. If this lab were completed without any sources of error, the Law of Conservation of Mass would prove correct, and the final mass of copper would be identical to the starting mass. BACKGROUND INFORMATION: Hydrates are formed from ionic compounds which take up definite amounts of water as an integral part of their crystalline structures as they crystallize from aqueous solutions. These compounds are called hydrates. We found that there were 3 moles of water to one mole of salt and hydrate. This is very unlikely occur, for human and systematic errors prevent the amounts to be truly equal, but very close. : In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. In order to determine the percent composition and the empirical formula of a hydrate, you must know how much water is in the hydrate. Final Mass of the anhydrous copper (II) sulfate Mass of water (that evaporated from the original hydrate) Observations when cleaning the evaporating dish Post Lab Questions: You must show . What two things make up hydrates? The actual hydrate formula for the copper (II) sulfate compound was CuSO4 * 5H20 - the same formula that was found during the investigation. Calculating molar mass: What is the molar mass of this hydrated compound? This particular lab report shows my ability to work with quantitative data, and analyze the calculations and measurements from the lab.… This lab used the idea of hydrates and molar mass to figure out the molecular formula of the hydrated cupric sulfate. Along with you introduction and procedure, construct a data table for the lab. Mass the watch glass and hydrate. The class average for the percentage of water in the hydrated copper (II) sulfate compound was 28.79%. Thus, in this experiment it is our goal to determine the percent of water in an unknown hydrate as well as the formula of the hydrate. 3. The hydrate is Copper(II) Sulfate or CuSO4 After conducting the experiment I found the mass percentage of this compound is: 28.4% water 71.6% copper(II) sulfate This is how I find the number of hydrates in the solution: CuSO4.xH2O (where x is the number of hydrates) Assume 100 g sample I Composition of a Copper Sulfate Hydrate Lab The purpose of this lab was to calculate the empirical formula for copper sulfate. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. Five strategies to maximize your sales kickoff; Jan. 26, 2021. This would decrease the calculated percent by mass of water in the compound. (Our balance only read up to 3 sig figs for the percent error, so we just used 3 sig figs) 5a) My answer is 0.0144321931 mol for the moles of water evaporated. The data obtained from the lab is here: Determining the Chemical Formula of a Hydrate Purpose Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. 2. Sources of error: Not all the H2O might have evaporated during heating Copper (II) Sulfate therefore the mass of anhydrous would be too high. The ratio is 1 mole copper (II) sulfate to 5 moles water. 6. would be too high. Aside from the colour change, what qualitative evidence suggested that the copper (II) sulfate … The previous reaction that took place involved aqueous copper(ii) sulfate and solid zinc. The copper sulfate moles should be the smaller. Allow watch glass to cool. CuSO4 Perform calculations to determine the mass percent of water in an unknown hydrate Introduction: Certain compounds form crystals with a definite proportion of water molecules incorporated in the crystal structure. 7 benefits of working from home; Jan. 26, 2021. Blog. Determination of hydration number: show how you obtained your “answer” for the formula of the unknown hydrate of copper (II) sulfate. For instance, several chemists might get different answers when measuring a piece of rope or rubber band if they do not know what the tension is supposed to be. This will be done through a knowledge of finding empirical formulas and percent composition. This is a lab report for my General Chemistry class. Determine the mass of the covered crucible and crystals to the nearest 0.01 g, and record the mass in your data table. After calculating the empirical formula of the copper (II) sulfate hydrate, analyze this data using percent composition. I did a lab in chem and I have to write a lab report and we need to have a source of error (assumptions) in the lab report. In this lab we trying to find emperical formulas. The ions removed in this step were zinc and sulfate ions as part of the zinc sulfate mixture that was "aq" as well as copper and sulfate ions that may be part of the unreacted part of the last reaction which included copper sulfate. Place the crucible with the copper sulfate hydrate on the triangle, and again position the cover so there is only a … b) The molecular formula would be CuSO4. The actual hydrate formula for the copper (II) sulfate compound was CuSO4+5H2O. As I have reached this stage, I think I may say that I now understand more about finding formulas using experiment procedure.MgSO 4 . Procedure. (the hydrate is CuSO4(nH2O, what is the value of n?) Heat the hydrate on hot plate until all blue is gone. ALL WORK. Finding the Formula of a Hydrate QUESTION: What is the formula of an unknown hydrate? Weigh the empty crucible, and then weigh into it between 2 g and 3 g of hydrated copper(II) sulphate. Remove watch glass from hot plate, turn off hot plate. Clean up. The assignment was to create a formal lab report that expresses data and observations, lab procedure, and a discussion of the data with a conclusion. Then we measured the mass again. Mass the watch glass and anhydrate. 1. 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