copper sulfate hydrate lab sources of error

October 3, 2017 There is an example problem included. Materials: Tests tubes (small or medium size), watch glasses, crucible* and cover*, crucible tongs, clay triangle. Adding EV Charger (100A) in secondary panel (100A) fed off main (200A). Solved Post-Lab Questions 1. If the correct formula of - Chegg Determined mass of anhydrous salt by subtracting the mass of the crucible and lid, from the mass of the crucible, lid, and anhydrous salt: 1.1434g, Determined mass of the water lost by subtracting the mass of the anhydrous salt, from the hydrous salt: 1.018g. Also as I was calculating the empirical formula, I wasn't quite sure the figures were correct so I might have miscalculated. So you will get 1 copper sulfate and your amount of water should be larger than 1 when you divide by the smallest. Heating will shift the equation of dehydration below to the right since it is an endothermic reaction. Im teaching chemistry to a home-ed 15 year old. Piece of paper, NaCl (sodium chloride), water, 6 M HCL (hydrochloric acid), 0.1 M AgNO3 (silver nitrate), Mg ribbon, 6 M HCL (hydrochloric acid), CuSO4 5 H2O, 0.50g iron fillings, 0.50g of powdered sulfur, magnet, copper sulfate solution, zinc metal The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. When you get this mass remember it includes the mass of the crucible so you need to subtract the mass of the crucible from the total mass. For example, if a given amount of hydrated copper(II) sulfate gave off 0.060 mole of H 2 O and left behind 0.012 mole of anhydrous copper(II) sulfate, CuSO 4, then the ratio of H 2 O to CuSO 4 is 5:1, and the formula would be written as CuSO 4 5H 2 O. Cross), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Psychology (David G. Myers; C. Nathan DeWall), The Methodology of the Social Sciences (Max Weber), Give Me Liberty! Do Eric benet and Lisa bonet have a child together? Introduction Determining which hydrate of calcium chloride I have? It is generally possible to remove the water of hydration by heating the hydrate. * Pipet This compound is not dissolved in water, the water is part of the formula and is a solid. ). Hydrate: A compound that contains the water molecule. Lab Report Solved Name Formula of Hydrates Lab Report Data and - Chegg Finding the formula of hydrated copper(II) sulfate | Experiment | RSC Education In this experiment students will measure the mass of hydrated copper(II) sulfate before and after heating and use mole calculations to find the formula. I weighed out some of the hydrate into another dry dish, flattened it out as much as possible within the confines of the dish to expose as much surface area as possible, and left it in the airing cupboard for 24h at 26 degrees Celsius. Download the preview file to get a look! 10/4/17 Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved. The focus of this lesson is defining hydrates, the lab procedure of dehydrating a hydrate, doing percent of hydration and percent error calculations and naming hydrates. Is Brooke shields related to willow shields? Texas Chemistry Standards (TEKS) The actual percent is ____. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. All rights reserved. ), Human error is always in effect, given that the laboratory does not function under ideal conditions. Explain what may have happened. . Paragraph #3: An error and how to fix it. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. Follow the directions below to complete the lab. * Salt The actual value of moles of water per copper sulfate is 5 moles and the percent composition of water in copper sulfate pentahydrate is 36.1% Variables: Independent Variable: Mass of crucible, cover and hydrated sample in grams Dependent Variable: Mass of water evolved in grams The mass was reduced to 7.58 g. What is the formula of the hydrate? The introduction to this lab introduces students to h. Eat, Sleep, Exercise & Hydrate: The Importance of Taking Care of Yourself! A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. Firstly to clarify a chemical change is defined as a change resulting. The reason why this is a source of error is because as time passed between the measurements, the copper sulfate hydrate sample absorbed humidity (water) from the atmosphere and therefore increased its mass. Occasionally we do some practical work, since I believe very strongly that physical science learning should have some real lab work to bring it alive, and also to teach things like observational skills and attention to detail. When you have finished, submit this assignment to your teacher by the due date for full credit. 2. Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. What did your group get as the formula of the hydrate? Skip to main content Skip to navigation Mast navigation Register Sign In Search our site All All Resources Articles Pour the used nitric acid in the waste container provided. What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six? Le Chateliers principle predicts that an addition of heat to an endothermic reaction (heat is a reactant) will shift the reaction to the right (product side). Be sure to subtract out the crucible before putting it into the proper space above. Who makes the plaid blue coat Jesse stone wears in Sea Change? temperature change caused by the reaction is hard to measure. 1.7: Experiment 6 - Hydration of Salt - Chemistry LibreTexts The weight after cooling of the evap dish is constant. In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. Given that the mass of the hydrated salt is known, it is also given that the mass lost is equivalent to the mass of the water. The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. Answer: Weigh and record the mass of the cooled crucible with its cover and content (anhydrous residue). Percent error **hint set up the table with percent composition for water** Percent error = actual % experimental % X 100 = ____ % actual %. heat loss to the surroundings if you using the simple 'insulated What does that x value tell you? -Pre soaked popsicle, Graded Assignment AB1 (8 points) Is there any known 80-bit collision attack? Added deionized water to the anhydrous copper sulfate, at which point it became hydrated again, and returned to its original blue coloration. Safety: When heating a substance in a test tube, be sure the open end of the test tube points away from yourself. Mass of crucible, cover and solid hydrate: Mass of crucible, cover and anhydrous solid: Formula of anhydrous solid (from Instructor): Moles of \(\ce{H2O}\) present in the hydrate: Ratio of moles \(\ce{H2O}\):Anhydrous solid = \(x\): Formula of hydrate [\(\text{Anhydrous solid}\ce{*}x\ce{H2O}\)]: Did the compound(s) that appeared wet in section B lose or gain water? Lab Report Period: 5 \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\]. The salt is magnesium sulfate - MgSO 4 and, the same as Copper sulfate, it exists as a hydrate, but in this case we will find the amount of water surrounding the compound. Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! Copper sulfate and potassium iodide precipitate, EXAMPLE HYDRATECUPRIC SULFATE PENTAHYDRATE The coefficient of 5, Copper SourcesUses n Copper cookware n Copper pipes, Characterization of the Heparan Sulfate and Chondroitin Sulfate, Percent of Change Percent of Increase Percent of, Percent Composition What is Percent Composition The percent, Percent Proportion Equation Percent of Change Percent of, Empirical molecular percent composition Percent Composition Percent by, Percent Vpoet potu percent Vypotaj spamti koko percent. * Paper towel A. Calculate your % error: "absolute value of . What did your group get as the formula of the hydrate? How do you feel in the morning when you wake up? In this section we will demonstrate the dehydration and re-hydration of cobalt (II) chloride hexahydrate. 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. Measured mass of crucible with anhydrous copper sulfate: 37.3005g. Grace Timler Your name and the names of any lab partners. Lab 1: Determining the Empirical Formula of a Compound, Lab 2: Determine the Percentage of Water in a Hydrate, Lab 16: Gravimetric Determination of a Precipitate, Lab 14a: Separation and Analysis of Cations, Lab 18: Separation by Liquid Chromatography, Lab 6a: Standardizing a Solution of Sodium Hydroxide, Lab 33: Determination of Calcium Carbonate Content of and Anti-Acid Pill, Lab 28: Molecular Interaction in Ethanol and Acetone, Obtained crucible and lid (henceforth, the two are considered to be together unless mentioned otherwise), inspected them, and measured their mass: 36.1574g, Obtained equipment, set up ring stand, Bunsen Burner, clay triangle, and mesh pad. Solutions were made up of two parts, the solute and the solvent. Error results and analysi, The first procedure (Part 1) used heat to dehydrate the 4 hydrates and sucrose. Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). What is wrong with reporter Susan Raff's arm on WFSB news? If the results of your calculations suggest that you have some water left in the residue, reheat your sample for an additional 5 minutes, allow it to cool down and weigh it again. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. Try to avoid and popping or . Hydrate Lab Hydrate Lab. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . How did it compare to the actual (it is given to you in step 3 of the calculations)? PDF Experiment 4 Hydrates and Anhydrous Salts This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Which observations, experiences, or lesson materials helped you form your hypothesis? What is "water of hydration" and how does it affect me (you)? Record the values as initial masses of containers and samples. This worksheet is a great follow-up to 42-Naming Hydrates. Send me a message, I'd love to hear from you! 2. Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. Chemistry Experiment # _____ Percent of Water in Copper II Sulfate Pentahydrate Name_____ Section_____Date_____ Name(s) of Lab Partner(s) . For this step, you are just changing your grams of water to moles using factor labeling. (3 points) When hydrates are heated, the water is released from the compound as water vapor. Hydrates Lab Report Final - Chemistry Exp: Explore And Evaluate Bonding To subscribe to this RSS feed, copy and paste this URL into your RSS reader. Naming and Formulas: Simple Ionic and Covalent Compounds Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. Chem 1A 04 Lab 3 Hydrate Report - Studocu You will be able to edit the document to your needs and share it with your students. * Water The solvent was the dissolving substance and the solute was the substance being dissolved. This lab will go in your lab book. Purposive Communication Module 2, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1. Still working on that - I'm going to leave a sample fresh from the bottle in a warm cupboard overnight tonight, and see if it gets any lighter. Once students have answered, they use the colo, Fully editable slide presentationHave you ever wondered why you get a lot of headaches, your muscle doesn't function as well and your immune system is low. Data can be collected and most of it analyzed in a single 45-50 class period. sulphate, calcium sulphate and lead sulphate. You did what I thought of doing but didn't get around to do. Copper/Iron Stoichiometry 7: Gravimetric Analysis (Experiment) - Chemistry LibreTexts * Evaporating dish Moles of water per mole of \(\ce{CoCl2}\): What color would you expect to see when this student dissolves the blue residue in water at the end of the experiment? This resource will come to you as a Google Doc. Be sure to subtract out the crucible before putting it into the proper space above. Use MathJax to format equations. Minutes in set-up time! Chemistry Naming & Formulas: Polyatomic Ions & Hydrates Guided Inquiry Lesson, Composition of a Hydrate Chemical Formula Lab, Naming & Writing Chemical Formulas: Acids & Hydrates |Distance Learning, Naming & Writing Chemical Formulas-LESSONS BUNDLE, Drink more water- hydrating, refreshing, natural. * Matches Other compounds can spontaneously absorb water from the surrounding atmosphere, they are said to be hygroscopic. There are a couple sources of error during the experiment, one would be the fact that we aren't entirely sure that the water had completely evaporated from the Copper (II) Sulfate and the Magnesium Sulfate. Ignited Bunsen Burner, and heated crucible for 12 minutes. The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. ), During heating, some of the hydrous salt may have spattered, thus removing a portion of the hydrous salt from the crucible (A more likely source of error, considering that this would result in a greater difference between the two ratios, and percentages. when does coordination become the distinctive task of management why? Lab written for Hotplate or Bunsen burner.Students: Observe water leaving compound as steam Heat to constant mass Calculate percent water Re-hydrate the anhydrous compoundLab Contains: Student Lab Sh, This lab is a great way for your students to investigate what a hydrate is and how its formula is determined. We would call this copper sulfate pentahydrate. He weighs a clean and dry crucible with its cover and records a mass of 18.456 g. He then weighs the sample in the crucible and cover and obtains a mass of 19.566 g. He heats the sample, allows it to cool to room temperature and reweighs it to obtain a mass of 19.062 g. In the process, the samples color changed from red- burgundy to blue. Introduction: * Copper II sulfate xH2O(s)) Before heating Run 1 Run 2 Mass of crucible 27.29 g 27.51 g Mass of crucible + hydrate 28.56 g 30.00 g Mass of hydratea 1.27 For a compound to be a true hydrate, it has to show all properties of true hydrates, including evolution of water upon heating, solubility of its anhydrous residue in water and reversibility in the color of the residue back to the color of the hydrate when dissolved in water. I give . When heated gently, the red burgundy \(\ce{CoCl2*6H2O}\) will decomposes into the violet \(\ce{CoCl2*2H2O}\) then to the blue anhydrous \(\ce{CoCl2}\). Calculated the percentage of water in the hydrated salt: Determined amount of anhydrous salt by dividing the mass of the copper sulfide by the number of grams per mole, in 1 mole of copper sulfide: 0.01058mol, Determined amount of water lost, by dividing the mass of the water lost during heating, by the number of grams per mole in 1 mole of water: 0.0565mol. This lesson presumes a basic understanding of how to name and write the formulas for binary ionic compounds. Students dehydrate copper (II) sulfate pentahydrate in a crucible or evaporation dish and use their data to determine the % composition and the number of water molecules per formula unit of copper (II) sulfate. Why purchase my version of this lab? Happy teaching and have an, Students find the Empirical Formula of Epsom Salt. has a mass of 4.31 g before heating. - CLICK HERE **--------------------------------------------If you like what you see, check out the rest of my store and be sure, This hydrate lab activity is perfect for chemistry teachers without a lab room! It contains a brief introduction to hydrates and then describes the series of calculations that are done to determine the ratio of the moles of water to anhydrate salt. Record the exact mass of the dish with the hydrate to the nearest 0.01 gram. 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. where $W_0$ is the start weight, $W_e$ the end weight and $M_i$ is the respective molecular mass. Will this likely lead to a higher or lower value of \(x\) than the actual value? Send me a message, I'd love to hear from you! Hows your energy level around mid-morning?This health trio bundle will give you and your students the much-needed information as to why eating breakfast, hydrating with the right liquids and sleeping well are important parts of keeping your body and well-being healthy. The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8.001 grams of copper (II) sulfate, CuSO4, and 2.0153 grams of iron powder, Fe. Weigh the samples and record the masses as final masses. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate . Solids: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride, Sodium sulfate hydrate, Iron (III) chloride, Potassium aluminum sulfate, Calcium chloride, Copper sulfate, Unknown. 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. NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? \[ \underbrace{\ce{CuSO4*5H2O (s)}}_{\text{Deep Blue}} \ce{->[\Delta]} \underbrace{ \ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{+ 5 H2O (g)} \label{1}\], \[ \underbrace{\ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{->[\ce{H2O (l)} ]} \underbrace{ \ce{CuSO4 (aq)}}_{\text{Deep Blue}} \label{2}\]. They are very math intensive, and very conceptual in nature. (However, this is not likely to be the sole cause of the inaccuracies within this experiment, though it may contribute to it. In this experiment, the percentage by mass of sulfate in an unknown sulfate salt will be determined by gravimetric analysis. 3. 1 A student is given a cobalt (II) chloride hydrate. Do you perhaps have any information about the nature of the .6% impurities in the original sample? DOC Copper Sulfate Lab - Montgomery Township School District Observations on structure, texture , wetness, etc. Through the use of a vacuum filtration system the mass of Cu was, Flame Test Lab Report The purpose of this lab was to have real life experience with using observations to determine whether or not a chemical or physical change had occurred. Purpose and a brief description of what you did. Why purchase my version of this lab? How to force Unity Editor/TestRunner to run at full speed when in background? Mathematics was used to explore wate, servation of mass and the reversibility properties in question. 5 H2O. This means that the formula for hydrated copper sulfate is: The goal of this experiment is to determine the percentage of water (by mass) in a hydrate, and to calculate the ratio of salt to water in a hydrated salt. Concentrations are based on how much solute is in a solvent, and is reported by the units of molarity. Minutes in set up time. CDC Health Standard 7, Naming Ionic and Covalent Compounds, Acids, and Hydrates, Acids, Bases and Hydrates Names and Formulas | Science Color By Numbers, Naming Compounds Bundle | Nomenclature | Science Color by Numbers, Chemistry Lab: Empirical Formula Hydrated Compound, PPT, WmUp, Ex Tic, Key, Lab, Chemistry Lab Bundle 1: 31 Labs, 17 Inquiry, Quiz, Key, PPT, PDF/Word, Copper (II) Sulfate Hydrate Lab - % composition, UNIT 9 - THE MOLE WORKSHEETS BUNDLE (#59-61), Chemistry Curriculum Full Year Guided Notes Bundle, Formula of Hydrate Lab - Data & Analysis GoogleSheet, Percent Composition, Empirical & Molecular Formulas, of Compounds & Hydrates, Chemistry Lab: Percent Water in a Hydrate. Then I re-weighed. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. If, like @brinnb suggests, an additional reduction in $W_e$ could be expected due to adhered water say that the error in $W_e$ is $0.1$ g you already get to $\Delta X=0.17$ mol water per mol copper sulphate. The name of this compound is "copper sulfate pentahydrate". Hypothesis (answer in a complete sentence in lab book). Record the mass of the crucible, cover and sample. Excellent layout. Gently heat the hydrate by moving the burner back and forth around the dish. Through this the appropriate reaction had to be determined out of the two possibilities. In this part, pea-, sized samples (1-3g) were place separately in test tubes and heated for approxim, Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Educational Research: Competencies for Analysis and Applications (Gay L. R.; Mills Geoffrey E.; Airasian Peter W.), Brunner and Suddarth's Textbook of Medical-Surgical Nursing (Janice L. Hinkle; Kerry H. Cheever), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Civilization and its Discontents (Sigmund Freud), Business Law: Text and Cases (Kenneth W. Clarkson; Roger LeRoy Miller; Frank B. Iron (III) chloride. Explain. Purpose: To observe the difference between chemical and physical changes. However, I understand that sharing information required for a lab report or unknown submission (including but not limited to word processing or spreadsheet files, calculations, graphs, conclusions and additional problems at the end of the lab report) with other students is, evaporating dish, Bunsen burner, wood splint, test tubes, micro spatula, dropper, mortar and pestle, test tube holder, safety goggles, lab apron. MathJax reference. Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). How to apply a texture to a bezier curve? By comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Do you have pictures of Gracie Thompson from the movie Gracie's choice. Heat the content of the crucible with its cover slightly open to allow the water of hydration to escape, first gently (about 10 minutes), then strongly (about 5 minutes). To determine the mass of the water, subtract the anhydrate from the hydrate and put it in the proper space above. No trace of black, and indeed we dissolved the anhydrous salt in water (for growing some seed crystals later), and there was no insoluble residue. 10/3/12 This document includes the pre-lab, procedure, data table, and analysis questions. -Bunsen burner It only takes a minute to sign up. Its weight before cooling was 0.02g (on my scales) less than its empty weight cold. The results for the heating, Title: Title of lab/experiment. The date the lab was performed or the date the report was submitted. 2021-22, PDF Mark K Nclex Study Guide: Outline format for 2021 NCLEX exam. The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. If a chemical reaction occurred, write a balanced equation for it. PDF Experiment 1 Hydrates Period 3 $$\Delta X=\frac{\sqrt{(\Delta W_0)^2 W_e^2+(\Delta W_e)^2 W_0^2}}{W_e^2}\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{3}$$. You will be able to easily integrated it into your Learning Management System. Place the crucible, hydrated copper sulfate, and lid on/in your clay triangle. Heat for 5 minutes using a single-cone blue flame. Given that water has a much lower boiling point than copper sulfate, I hypothesize thatwe can heat it to remove the water, and then calculate the mass that was lost, based on measurements made before and after the water was evaporated. Record the appearance of the hydrate before it is heated. Tina Jones Heent Interview Completed Shadow Health 1, Test Bank Varcarolis Essentials of Psychiatric Mental Health Nursing 3e 2017, 1-2 Module One Activity Project topic exploration, (Ybaez, Alcy B.) Chemical Changes VS Physical Changes * Candle However, because the solutions were not mixed long and thoroughly enough, this made further deviations from what the data should have looked like. Cool (approximately 10 minutes) and get the mass of the anhydrate (white compound). B. ** Interested in my other Chemistry Resources?? The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid. Paragraph #2: What did you learn? Previous to an exposure to heat via the stove, it can be seen that the copper sulfate bear the natural form and colour of a bright blue crystal. Then use that information to write the formula of the hydrate. Hence 0.267/0.0515 = 5.18mol water per mol copper sulphate. Which is very close to the actual error you find. Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. Copper/Iron Stoichiometry Grace Timler AB1 October 3, 2017 Abstract The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8.001 grams of copper (II) sulfate, CuSO4, and 2.0153 grams of iron powder, Fe. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. The number you found for the water replaced the x in the formula CuSO4 xH2O. Make sure that the tube is clamped near the bung as shown. It is soluble. Rounded to the nearest integer, the ratio is 1:5. 8.22/(63.5+32+64) = 0.0515mol anhydrous copper sulphate. In this lab, the five general types of chemical reactions were conducted and observations. 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. My background is a PhD in organic chemistry, so Im familiar with hazard assessment, and all the lab work I do with my student is something Ive done myself already. It should be brief (aim for ten words or less) and describe the main point of the experiment or investigation. 5 H 2 O 6. DOC Copper Sulfate's Water of Hydration Lab Digication ePortfolio :: General Chemistry (Alexander Antonopoulos