Dehydration of copper(II) sulfate pentahydrate Mass of empty crucible Experimental mass of hydrate (CuSO, SH,0) Mass of beaker after crucible after heating 31, 63g 300g 35,09 2,079 Mass of Cuso, (experimental) RETO Moles of Cuso. IV. Many compounds exist as hydrates. This particular lab explores the relationship between the anhydrous salt and water in a hydrated sample; it helps students to better understand the concept of the Law of Definite Proportions. The hydrate compound Copper (II) Sulfate was added to the crucible and the mass of the substance and the crucible was found using the scale. If you don't heat the hydrate enough, you won't get all the water to . So I did a lab determining the chemical formula of a hydrate. In its liquid or powdered form it's most commonly called basic copper sulfate, BSC copper fungicide, CP basic sulfate, or tri-basic copper sulfate. No of moles of = = 0.012 0.001moles. water/moisture. This is because although it occurs below the boiling point of water, you are . These are called hydrates. Conclusion. The unit formula for the salt appears first, and the water formula is last. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. For example, copper(II) chloride exists as anhydrous (no waters of hydration) or as a dihydrate (2 waters of hydration). Heat the blue copper(II) sulfate until it has turned . Over time anhydrous copper sulfate reabsorbs . Since the only component (other than H2O and Cu 2+) is the sulfate ion, SO 4 2-, we can now determine the complete formula of the hydrated copper(II) sulfate. 5 H2O. A hydrate is a compound that is chemically combined with water molecules. The initial and final moles of copper are supposed to be the same . If a CHEM 101 student has 14.367 g of CuSO4.5H20, how many grams of water should be driven off? of a Hydrate Lab Wednesday October 29, 2014 Chemistry Honors Purpose This lab was done to determine the percentage of water in a hydrate, which was CuSO4 ?H20. We used three chemistry concepts which are: a hydrate is a compound that contains water, an anhydrous compound is a compound that has had the water driven off of it, and water of hydration is the water that is . The molar mass of CuSO 4 . The initial and final masses of copper are supposed to be the same, but they are different. 'Chalcocite', the anhydrous form of copper sulfate . 1001309 Mass H 0 (experimental) Moles H,O 0,93g. Hydrated copper sulfate 4.32 g Anhydrous copper sulfate 3.145 g Water 1.175 g. Questions: 1. This would decrease the calculated percent by mass of water in the compound. In the equation I took the no of moles of water as x because it is unknown. Purpose. Prohibitions on mixed storage : KEEP SUBSTANCE AWAY FROM: reducing agents. Our percent error, we found , was about 2.22% because our value for the percent water was lower than the expected value--35.2% instead of 36%. Copper Sulfate's Water of Hydration Lab Calculation Sheet. Five should be used as the theoretical value in the percent composition calculation and the number you calculated from your lab data should be used as the actual or . the water that's a part of the compound, evaporates and leaves you with just the anhydrous form - in your case, #CuSO_4#. _____g CuSO 4 Determine the mass of water lost from Hydrate. Utilisations identifies pertinentes de la . 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. This results in a calculated hydrate formula of copper (II) sulfate pentahydrate, CuSO4 5H2O. This is written CuSO4. 31 du Rglement (CE) 1907/2006. Prediction. After the water had completely evaporated, the copper (II) Sulfate . CuH14O11S. copper (ii) sulfate heptahydrate. Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. Lab- Hydrate Ratio of Epsom Salt Goggles must be worn! Hydrated copper sulphate is blue in color while anhydrous copper sulphate is white in color.CuSO4 is white, the pentahydrate crystal (CuSO4.5H2O) and the aquous solution (Cu2+(aq) ions) are royal . A hydrate like cupric sulfate is any compound containing water. Or not. Copper sulfate 1. It turns from blue crystals to a colorless white powder and is odorless 2. (strong) bases. This is written CuSO4 . But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. The data obtained from the lab is here: Determining the Chemical Formula of a Hydrate. This is a class experiment suitable for students who already have a . The copper sulfate is dissolved in 100ml of water that is distilled and contained in . The compound's formula is CuSO4 . The composition of the complex formed when hydrated copper (II) sulfate is reacted with oxine is Cu (C 9 H 6 ON) 2 with 351.85g/mole formula weight. Procedure Weigh out approximately 5g of copper sulfate pentahydrate. Follow the directions below to complete the lab. For example, Glucose is C6H12O6; it's empirical formula is CH2O. In contrast, an anhydrate does not contain water, and has had all . Percent Composition of Water in Hydrated Copper (II) Sulfate Ruth Zhang Lab Partner: Serge-Erik Douge Instructor: Mrs. Fran Jimnez Date of Activity: February 13, 2019 Introduction Percent composition is used to determine how much of an element is in a compound, by mass. Mass of hydrated copper(II) sulfate copied from yesterday's data sheet:_____ 2. The ratio of water mol ecules to the anhydrous salt is constant. Determine the mass of Copper II Sulfate Anhydrate Using the mass of the beaker and the mass of the beaker with copper II anhydrate, determine the mass of the copper II sulfate anhydrate. Percent composition is determined by dividing the molar mass of a part by the molar mass of the whole compound. _____g CuSO 4 Determine the mass of water lost from Hydrate. The goal of this lab was to see if the mass of copper would be same after going through a series of chemical reactions. Its blue crystals look and feel dry, but each mole of the anhydrous salt is actually bonded to five moles of water. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. 2. Lab #9: Composition of a Copper Sulfate Hydrate Lab Hydrate Photo Before The hydrate was a deep blue color and very crystalline. In this experiment iodometric titration is done using an unknown concentration of copper (II) sulfate in a 100ml volumetric flask (A43). The compound's formula is CuSO 4. copper (II) sulphate heptahydrate. z H 2 O. Now place the mini crucible filled with 2.00 g of Copper (II) Sulfate hydrate on top of the clay triangle. We assumed that all the water had evaporated after the third cooling. Conclusion: In this lab, we were trying to determine the empirical hydrates of copper (II) Sulfate Hydrate and of Magnesium Sulfate. When all the water has been evaporated from a hydrate it is known as an anhydrous compound. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. The initial moles of copper is 0.03152 mol, and the final moles of copper is 0.1457 mol. The mass of the empty crucible was found using the scale. This is appropriate for all levels of chemistry. Now take the two separate hydrates back to your lab station. a) Determine the value of x in the formula of the compound b) Chem 11. (e) mass of copper Average % copper content (f) % copper content 12B Exercise Copper(II) sulfate forms a hydrate which contains 36.1% by mass water. 5 H 2 O. Then we measured the mass again. First, a hot plate is turned on and heated to 70C, in the meantime, 0.3g of Cu x (SO 4) y . The initial mass of copper was 2.003 grams. INCLUDE UNITS EVERY STEP AND keep dp when + or - AND keep sig fig when x or ./. Hydrate Lab. Overview: Epsom salt (aka magnesium sulfate) is a combination of MgSO 4 and H 2 O. When referring to an unknown hydrate, you should use the notation described above. Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. I won't go into too much detail about hydrates and anhydrous compounds.. #color(green)("Point a)")# So, you start with a certain mass of the hydrate. Record the mass and place the solute into a 50 mL volumetric flask. One example of a hydrate is copper (II) sulfate pentahydrate. The accepted value is about #36.075%# , so I would say that your results are not ideal, but that they should fall within the accepted range. z H 2 O is collected and poured into a 250ml beaker, then, 100ml of distilled water is added to dissolve Cu x (SO 4) y . Today we will analyze a pure salt of copper(II) - maybe it's copper(II) nitrate, or copper(II) acetate, or copper(II) chloride, and so on. In order to do this, we measured the mass of the copper,put the copper sulfate in a crucible and burned off the water. Its blue crystals look and feel dry, but each mole of the anhydrous salt is actually bonded to five moles of water. Copper sulfate solutions may serve as an antiseptic and as a source for depositing copper on metals. Very toxic to aquatic life with long effects. The name of this compound is "copper sulfate pentahydrate". Allow the test tube and its contents to cool. Hold it over the flame with a test tube holder and heat it for a few minutes with the mouth of the tube slightly below the base of the tube. Molecular Weight. 5. The symptoms of poisoning include diarrhea, headache and injury to vital organs. Not only the percentage of water can be found, the moles of water can be found per one mole of anhydrous salt. The mass of water is found by weighing before and after heating. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Do this by placing the empty crucible on the balance then pressing tare, then measure out 2.00 g of Copper (II) Sulfate hydrate, and put it in the mini crucible. 4. Make sure that the tube is clamped near the bung as shown. The compound's formula is CuSO4 . This lab will go in your lab book. 3. CID 23978 (Copper) CID 962 (Water) I. Hydrate test A. Component Compounds. A hydrate is an ionic compound that has a definite amount of water molecules attached to its crystalline structure. In order to do this, we measured the mass of the copper,put the copper sulfate in a crucible and burned off the water. According to the equation the mole ratio between copper sulfate and water is 1: x. Heat the hydrated copper (II) sulfate for 10 minutes. We systematically heated and cooled the copper sulfate three times, massing after each cooling. SAFETY Nom Chimique : Cuivre(II) sulfate-5-hydrate No.-Index : 029-023-00-4 Numro d'Enregistrement REACH : 01-2119520566-40 1.2. Then we measured the mass again. I want to determine the chemical formula for a hydrate. Thus, copper sulfate is . Measured mass of crucible with anhydrous copper sulfate: 37.3005g Once dissolved, fill the rest of the volumetric . The mass of the hydrated salt was 2.90 grams so therefore, the percentage by mass of water in the hydrated copper(II) sulfate compound was determined to be 37.2 percent. The mass of the substance was found using the tare function on the scale. Mass of anhydrous copper(II) sulfate (copied from yesterday's data sheet):_____ 3. Then use that information to write the formula of the hydrate. Data can be collected and most of it analyzed in a single 45-50 class period. After calculating the empirical formula of the copper (II) sulfate hydrate, analyze this data using percent composition. Causes skin irritation, causes serious eye irritation. copper (II) sulfate.Break up any large crystals before placing them in the crucible. Heat can be used to dehydrate a hydrated salt causing the H 2 O molecules to Chemical Name CAS Number 1DPH 54 CERCLA RQ 734 CAA 112(2) TQ Copper (II) Sulfate, 5-hydrate 7758-99-8 No No No No No California Prop 65: No California Proposition 65 ingredients Suppose that you heated a sample of hydrated ionic compound in a test tube. This would cause there to be a . Copper sulfate without water is named "anhydrous copper sulfate" and written just "CuSO4 ". INCLUDE UNITS EVERY STEP AND keep dp when + or - AND keep sig fig when x or ./. Percent error= In the lab, it is possible to get a higher percentage of water than 36.0% by losing some anhydrous salt perhaps by spilling or being stuck on the spatula. Its blue crystals look and feel dry, but each mole of the anhydrous salt is actually bonded to five moles of water. Based on your data, determine the molecular formula of CuSO4 xH2O. A hydrate of copper (II) sulfate with formula CuSO4.xH2O has a molar mass of 250.0 g/mol. 4. CuSO4.xH20 CuSO4 + xH2O. Compare the results observed when testing the liquid from the hydrate and distilled water with the cobalt chloride paper and the anhydrous salt by completing the table below. At that time, the copper sulfate had turned a yellowish-white. Determine the mass of the covered crucible and crystals to the nearest 0.01 g, and record the mass in your data table. 5 H2O. The molar mass of anhydrous copper sulfate is 159.6g. N.O.S. One example of a hydrate is copper (II) sulfate pentahydrate. The ratio is 1 mole copper (II) sulfate to 5 moles water. Set up the bunsen burner with a ring stand above and a triangle . . Materials needed: hot plates or burners with stands (pipe triangle or similar), crucibles or evaporating dishes, CuSO4-5H2O (fine crystals or powder). CAS 7758-99-8 Copper (II) Sulfate Pentahydrate 100 % Percentages are by weight SECTION 4 : First aid measures . 3. The first procedure consists of analyzing copper ion in hydrated copper sulfate. Conclusion. Using the mass of the copper II sulfate hydrate and the mass of the copper II Set up the apparatus as shown (but without water in the receiving tube - this is to be collected during the experiment), placing about 5 g of powdered hydrated copper(II) sulfate in the test tube. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. An anhydrous salt is a hydrate that lost its water. This information is used to find x in the formula CuSO 4 .xH 2 O, using mole calculations. After all of the chemical reactions have finished, the final mass of copper was 6.85 grams. The name of this compound is "copper sulfate pentahydrate". hydrate - a salt that includes water in its formula. anhydrous salt. Data: sources Protect from heat Additional information (precautions): Move product containers away from fire or keep cool with water . In order to determine this, we put both copper (II) Sulfate Hydrate and Magnesium Sulfate under extreme heat, to evaporate the excess water. When heated, the crystals "melt" at a much lower temperature than the ionic compound Na2SO4 normally does. Determine the mass of Copper II Sulfate Anhydrate Using the mass of the beaker and the mass of the beaker with copper II anhydrate, determine the mass of the copper II sulfate anhydrate. Nom du produit : Copper(II) sulfate pentahydrate FDS-nombre : 000000020682 Type de produit : Substance Remarques : SDS conformment l'Art. So the practical involved taking hydrated copper sulphate, heating it to drive off the water, weighing before and after, and thus calculating the number of water molecules of crystallisation, based on the respective molecular weights of the anhydrous salt and water. Testable Prediction: Our unknown hydrate may be a hydrate of copper (II) sulfate, magnesium sulfate, iron (III) chloride, or iron (III) nitrate. Unfortunately, that was not the case in this lab, and the final mass of copper exceeded the initial mass by 4.841g. We found that there were 3 moles of water to one mole of salt and hydrate. 1. Had a very dark and bold color. Do this determination. Since copper (II) sulfate is usually a bright blue due to Cu2+ presence, we can exclude that option .