Mass of dish + anhydrous salt (after heating) 5. CHEM . What is lost from the CuSO4 in this process? Heat the compound gently Note the release of any steam from the beaker. A hydrate is a compound that is chemically combined with water molecules. based on the chemical formula. 3.) Explain why the experimentally determined empirical formula may not match the actual formula of Epsom salt (propose at least 2 ideas). This means we can exclude these three options from our prediction. As we altered the strength of the flame from low to high without increasing the amount of time to wait until all the water can evaporate, there could have possibly been some water left in the beaker with magnesium sulfate that did not evaporate to completion. Included are labs on the following. The mass of water evaporated is obtained by subtracting the mass of the . waters of hydration released as water vapor, leaving solid white anhydrous CuSO, Equation 1 (heating copper (II) sulfate pentahydrate), CuSO5HO (s, blue)heatCuSO (s, white)+5HO (g), 3 steps to determining percent water in unknown hydrate, 1. Measure out 2 to 3 g of the magnesium sulfate in the crucible. Show your work, include units, and write your answers in the blanks on the right. 1.) Each type of hydrate traps water in its own unique way, but heating a hydrate will release the By doing this, it figured out that the . 3. Mass of hydrate 4. The reaction for the decomposition is as follows: In this part of the lab you will repeat the same procedure performed for the salt of known formula with a salt for which you do not know the hydrate formula. To calculate the molar mass, we added up each element's atomic mass for each part of the substance. How? Continue heating gently until the salt turns completely light grey. , as the hydrate appeared to be white due to the colorless magnesium.Thus, this knowledge of specific colors of ions led us to confidently conclude that the anhydrate was undoubtedly magnesium sulfate. The water in a hydrate is bound loosely, and so is relatively easily removed by heating. 1) The process you will execute in this lab is similar to _____, which a separation process that exploits differences in _____ between . (process and specific method used here). Mass of water. Copper suifate pentahydrate is used to determine the percent composition of water in a lab. . Unfamiliar with hydrates, we were first oblivious to how one could experimentally come up with a correct formula. Then, they heat the, experimentally. Hydrate Lab Answers Detailed calculations shown Accurate data recorded (5 0.3) Correct calculation for water lost Q1 - . Less moles of magnesium sulfate in the beaker would have then increased the ratio as the number of water moles would have been divided by a smaller value. Furthermore, this lab illustrated a new term for the group - hydrate. But as soon as we used previous knowledge of stoichiometry by using molar masses and numbers of moles, we were easily capable of depicting a reasonable empirical formula for the hydrate. crucible and contents and record the result in trial 1 of the observation table. From the calculation, you can clearly see that the units of g/mol in the numerator and denominator cancel out. Then, the experimental ratio of water to magnesium sulfate being 6.63 to 1 with about 6% error strongly supports our hypothesis to a deeper level. : an American History, 3.4.1.7 Lab - Research a Hardware Upgrade, BUS 225 Module One Assignment: Critical Thinking Kimberly-Clark Decision, The Deep Dive Answers - jdjbcBS JSb vjbszbv, Lessons from Antiquity Activities US Government, CWV-101 T3 Consequences of the Fall Contemporary Response Worksheet 100%, Piling Larang Akademik 12 Q1 Mod4 Pagsulat Ng Memorandum Adyenda at Katitikan ng Pulong ver3, 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. 3676 S 232 HL 100 . Empty the anhydrous salt onto a large watch glass. ring stand 1.000 g - 0.6390 g = 0.3610 g. 2. Calculate mass of water in hydrate sample. 4. The change from hydrate to anhydrous salt is accompanied by a . percent water in a hydrate lab answers. Answer: _____ b) Calculate the number of moles of water in the hydrate sample that were driven off by heating? Final mass ofAnhydrousCuSO4(without water), Moles of CuSO4in the anhydrous mass (mass / 159.5), Ratio between moles of water /moles of anhydrous copper sulfate, Final mass ofAnhydrousMgSO4(without water), Moles of MgSO4in the anhydrous mass (mass / 120), Ratio between moles of water /moles of anhydrous Magnesium sulfate, THIS DATA TABLE IS NOT FOR 2020-2021 STUDENTS, Data Table Lab #1 with triple beam balance, Mass after heating (First time) beaker + glass rod + CuSO45H2O, Mass after heating (Second time) beaker + glass rod + CuSO45H2O, (Mass of beaker + glass rod + CuSO45H2O Mass after heating (Second time), Data Table Lab #2 with triple beam balance, Mass after heating (First time) beaker + glass rod + mGSO4, Mass after heating (Second time) beaker + glass rod + mGSO4, Final mass ofAnhydrous MgSO4(without water-Lowest number you got), Moles of MgSO4in the anhydrous mass (mass / 159.5), (Mass of beaker + glass rod + MgSO45H2O Mass after heating (Second time), I am text block. Calculating amount of water in hydrate. Heat. Why Do Organism Look Like the Way They Do. Experiment 605: Hydrates . We believe our hydrate was magnesium sulfate, because the unknown hydrate was more closely related in physical appearance to that of magnesium sulfate, compared to the the three other options. represents the ratio. Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? 1. Balance Setup the ring stand with iron ring and ring. ("n" in SrCl2nH2O) Hydrates are ionic compounds that contain water molecules as part of their crystal structure. Calculate the percent by mass of water by dividing the mass of H 2 O in 1 mole of the hydrate by the molar mass of the hydrate and multiplying by 100%. Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO 4 x H 2 O, where x represents the ratio. Identity of the Hydrate:MgSO47H2O Magnesium heptahydrate, % Error = | (actual value - experimental value) / actual value | x 100%, = | (6.63 - 7.00) / (6.63) | x 100% = 5.58% Error. Write the formula of the one you chose. (MgSO4XH2O).Use a minimum of 2 g. This will help to reduce errors due to small lab balance inaccuracies. xH2O). Lone Star College System, Woodlands. Be sure your beaker and glass rod does not have any crack, and that that they are clean and dry. This, report requires students to directly apply their understanding of Empirical Formula and, procedure. The procedure is clearly defined so that there is no question about the proper way to safely perform the. Rubber hose Thus, at the end, we learned that there are countless numbers of applications of stoichiometry in chemistry. Some sources of deviation of the data may include: a. When hydrates are heated, the water is released from the compound as water vapor. Want to include, experiment that correlates with Stoichiometry? The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate ( 2.12.3 ): mH 2O = mHydrate mAnhydrous Solid. ? water lost by the hydrate. how are the waters of hydration included in the chemical formula? Equation 2 (percent water in a hydrate) The ratios of other three substances were incongruous to each other. Quizzes with auto-grading, and real-time student data. Finally, this is for balancing the chemical equation of the decomposition of a hydrate. = 0.08158 mol / 0.009273 mol = 8.80 mol H, = 0.08158 mol / 0.009125 mol = 8.94 mol H, = 0.08158 mol / 0.006120 mol = 13.3 mol H, | (actual value - experimental value) / actual value | x 100%, From this lab, we are able to conclude that our prediction was strongly supported in both terms. The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. Before this, we had heard of this scientific word briefly in textbooks and in class, but we were never sure of its exact definition. how do you know when crucible has cooled to room temperature? water of hydration pre lab answers. and from their collected data, calculate their, for several reasons. This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. You can use a metallic spatula this time. Repeat steps 4 and 5 until a consistent mass is obtained. This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. The hydrate contains water as a. Integral part of the crystalline structure. After comparing experimentally acquired ratios to the factual ratios for each substance, we determined that the ratios of magnesium sulfate was the closest one out of all four. + lose uoa. Record this value in your data table with the maximum available precision. To determine what percent by mass of a hydrate is water, first determine the mass of water in one mole of hydrate. While heating, be ready to adjust the height or Why do hydrates form? Virtual Lab: Hydrates. Iron (III) sulfate has a purple tint to it, and has a crystalline structure. b. Heat the hydrate for 5 to 10 minutes and allow for cooling. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . While these do not have teacher directions, most labs are fairly self-explanatory and have materials lists provided. Ut elit telctus nec ullamcorper matti, A2 Transition Elements Complexes and Equilibria, LAB #1 Preparation of a standard solution, AS Amount of Substance # 6 More complex calculations, AS Enthalpy Change of a Displacement Reaction, AS Enthalpy Change of Combustion of Fuels, ELECTROCHEMISTRY Exercises 1 Oxidation numbers, AS Volumetric Analysis 1-Preparation of a standard solution of NaOH, AS- Finding the molar mass of a volatile liquid, AS Experimental Determination of the Gas Constant, AS Qualitative Analysis Ions Recognition, IGCSE CH 2 Mixtures-Separation Methods Vocabulary, Matter Notes #3 Pure Substances and Mixtures, IGCSE BONDING DRY LAB Bears and Penguins, Precipitation Reactions Testing for Ions, Empirical and Molecular Formula Exercises, Rates of Reaction Lab #2 AlkaSeltzer + H2O, The Air Up There Making Space Breathable, Determine the percent of water present in a hydrated copper (II) sulfate (CuSO, Epson Salt (Magnesium Sulfate Sample (Around 5.0 g). then what do you do? for the imperialist) and position the flame under the crucible so that the inside blue Mass of evaporating dish 2. The change, mass observed allows them to calculate the amount of, COMPOSITION EMPIRICAL FORMULA Multiple Choice Grade 11 Chemistry (13 PG), This product contains 13 pages of chemistry multiple choice WITH ANSWERS on calculating the mass, data or mass data, determining the molecular formula of, 12 font, times new roman, without text boxes and condensed into the least amount of space possible. Minutes, written for Hotplate or Bunsen burner.Students: Observe, leaving compound as steam Heat to constant mass Calculate, the anhydrous compoundLab Contains: Student, , students heat epsom salt to drive off the, the crystal lattice. Calculate mass of hydrate heated 2. (0.3610 g /1.000 g) (100) = 36.10%. During exercise, hydrating with water only can dilute the body's sodium levels, according to Natalie Allen, R.D., clinical assistant professor of biomedical sciences at Missouri State University, with expertise in sports dietetics. The following data were obtained when a sample of barium chloride hydrate was analyzed: Mass of empty test tube 18.42 g. Mass of test tube and hydrate (before heating) 20.75 g % water = . . 7. What is bound to the copper (II) ion in copper sulfate? Honors Chemistry Worksheet - Hydrates ANSWER KEY. Simple! The moles of water and inorganic salt in Epson salt were separately calculated and. How many moles of water did you have in your original sample? Required Pre-Lab Video: ZamJ713 channel on YouTube: "Quarter 3 Chemistry Lab - Percent Water in a Hydrate" QUESTIONS: Refer to the information from the pre-lab video to answer the questions below. Masses are measured beforeheating to determine the mass of theoriginal sample (the hydrate)andafterheating to determine the mass of copper (II) sulfate (CuSO4) anhydrous. Record any qualitative observations (i. spattering, spilling, smoke). We are given the following data in the trial 1 , Before Heating : Mass of Dry crucible and cover = 40.11 g Mass of crucib, Lab 5 Data Sheet: Percent Water in a Hydrate Name: British lue Date: 10.0% 2020 Instructor Time & Day of lecture online DATA TABLE Sample Identification Number Before Heating Trial 1 Trial 2 Trial 3 Mass of Dry Crucible and Cover a 40.11a b Mass of Crucible, Cover, and Hydrate 40:91009 Mass of Hydrate ba After Heating a Mass of Crucible, Cover, and Dry Solid 41.4809 e Mass of Anhydrous Compound da f Mass of Water in Hydrate Sample Trial 1 Trial 2 Trial 3 Calculate the percent of water in the Hydrate Sample Trial 1 Answer: Show calculations: Trial 2 Answer: Show calculations: Lab Contains: Student Lab Sheet Student Lab Make-up Sheet for Absent Students Student Lab Sheet with Answers in Italics Lab Quiz - Use as exit ticket, next day warm-up or quiz Lab Quiz Answer Key Teaching Tips and Set-up Directions. In contrast, an anhydrate does not contain water, and has had all . how should crucible FIRST be arranged on ring? This is a oneperiod lab where you will be working in your Kitchen Chemistry Lab while connected with your group via Zoom Breakout Rooms. Trial Anwwer Show calculations! 1. Now, you try: calculate the percent of water in borax, Na2B4O7.10H2O. crucible & cover I give you teacher set up instructions, has an introduction to help students understand why they are doing the, from copper (II) sulfate pentahydrate by heating and determine the empirical formula. What percentage of water is found in CuSOp5H20? That's a problem, because sodium helps the body maintain fluid balance by ensuring that the right amount of fluid . this experiment.Materials needed:Copper(II) sulfate pentahydratecruciblehot plate or bunsen burner setupcrucible tongswaterLab also includes assessment questions from the NYS Regents Examination. weighing boat. This concluded that 75% of the substance was copper (II) sulfate while 25% was water. Question: Lab 5 Data Sheet: Percent Water in a Hydrate Name: British lue Date: 10.0% 2020 Instructor Time & Day of lecture online DATA TABLE Sample Identification Number Before Heating Trial 1 Trial 2 Trial 3 Mass of Dry Crucible and Cover a 40.11a b Mass of Crucible, Cover, and Hydrate 40:91009 Mass of Hydrate ba After Heating a Mass of Crucible, Cover, and Dry Solid Re-hydrate the anhydrous compound. when we heat blue CuSO5HO, what happens? Includes teacher instructions, sample calculations, and, key to the conclusion questions. CuSO5HO (s, blue)heatCuSO (s, white)+5HO (g) 3 steps to determining percent water in unknown hydrate. From the data the students can determine the experimental percentage of, list of six hydrated names that are provided, the students will write the formulas for those hydrates, calculate the theoretical percentage of, each, and determine which of the six hydrates is the identity of the unknown, Experiment for Stoichiometry! The number of moles of water in a hydrate was determined by taking the mass of the water released and dividing it by the molar mass of water. However, as we dehydrated the hydrate and discovered that a hydrate is made of some anhydrate and water with a certain ratio, we soon realized what a hydrate actually was. The change from hydrate to anhydrous salt is accompanied by a change in color: Record the mass. As 6.63:1 is relatively close to 7:1, the expected ratio for this substance, we can thus conclude that the unknown hydrate is magnesium sulfate heptahydrate, MgSO. Second, it will also determine the molar ration of water to inorganic salt in Epsom salt. In order to determine the formula of the hydrate, [\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)], the number of moles of water per mole of anhydrous solid (\(x\)) will be calculated by dividing the number of moles of water by the number of moles of the anhydrous solid (Equation \ref{6}). Answer the questions below. Once the beaker is cool, measure the mass of the beaker, the anhydrous salt and the glass rod. a) If the sample was heated to constant weight after reheating, what is the minimum mass that the sample can have after the second weighing? dish. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. 6. Place the crucible in the clay triangle. Subtract the mass of the metal dish plus Epsom salt from the mass of the empty aluminum. First, this experiment is focusing on how to determine the water content of a hydrate by heating. Answer: Show Calculations. Students will be determining the number of, procedure goes along with the corresponding, involves the heating of an unknown hydrated sample (magnesium sulfate heptahydrate). iron ring Log in, How to calculate the empirical formula of a hydrate. The identity of the mysterious substance was magnesium sulfate. 1.7: Experiment 6 - Hydration of Salt is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. T T , t _' l K K K K K 2 2 2 &. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. Design an experiment to accurately determine the empirical formula of a given hydrate. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. Dehydration of an Inorganic Salt Hydrate Student Name: Hojin Song Date: March 26 th, 2023 Purpose First, this experiment is focusing on how to determine the water content of a hydrate by heating. Legal. 1. chemical reaction changing Copper Sulfate pentaHydrate (CuSO4 . 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. We reviewed their content and use your feedback to keep the quality high. remove the burner in case of excess spattering. Water is a very polar molecule which tends to be attracted to . Take the mass of the If not enough heat is applied, some water will remain attached to the copper sulfate producing a low calculated mass percent water for the hydrate. An insufficient amount of time for waiting until all water of the hydrate evaporated. Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO. Describe the changes you can observe during the heating process. White monohydrate form is available at 110C, while the anhydrous form can be isolated near 250C. So the correct chemical formula is S r c l 2.2 waters for the next 1 37.2% water or 100 g of the compound gives us 32.7 g water Which will convert to moles water by dividing by its smaller mass, the remaining percentage is 62.8. If we had either heated the beaker with a strong flame from the beginning or increased the amount of time of heating, the number of moles of water during calculation could have been larger. 5. 9. how long should you heat the crucible at an angle? Course Hero is not sponsored or endorsed by any college or university. By the addition of water to the anhydrous salt. Then, the experimental ratio of water to magnesium sulfate being 6.63 to 1 with about 6% error strongly supports our hypothesis to a deeper level. . Step 3: Think about your result. Describe what happens in your lab notebook. If too much heat is applied, the anhydrous copper (II) sulfate (CuSO4), which has a grayish white color, decomposition starts at 250 degrees, while complete decomposition occurs around 600 degrees. lab hydrate ratio of epsom salt answer key. 7H2O) is a heptahydrate of magnesium sulfate:within one mole of magnesium sulfate heptahydrate are seven moles of water. Then allow it to cool and weigh it. By knowing that ions such as Cu2+and Fe3+have their designated colors, we were able to eliminate three options for the anhydrate, FeCl3, Fe(No3)3, and CuSO4, as the hydrate appeared to be white due to the colorless magnesium.Thus, this knowledge of specific colors of ions led us to confidently conclude that the anhydrate was undoubtedly magnesium sulfate. As 6.63:1 is relatively close to 7:1, the expected ratio for this substance, we can thus conclude that the unknown hydrate is magnesium sulfate heptahydrate, MgSO47H2O. A hydrate is a chemical compound, generally ionic, that has weakly bonded to it a specific number of water molecules per formula unit. Mass of anhydrous salt Calculations - Remember to show all of your work. Calculate the value of " n ", the number of moles of water molecules present per mole of CuSO 4 and Epson Salts. The light blue trihydrate non-isolable form can be obtained around 30C. Calculate the Average % of Water in the Hydrate Samples. What errors would this cause in the calculation of the percent of water in the hydrate? Hydrate Math The percent of water in a hydrate can be determined in a manner similar to determining the percent composition of a compound. Carry out actions from the step 2 to step 4 again for aluminum dishes with numbers 2 and 3. Data can be collected and most of it analyzed, single 45-50 class period. Bunsen burner Describe the magnesium sulfate hydrate before heating, How many moles of copper (II) sulfate (CuSO. How can original hydrates be regenerated? 90.10 Mass of Hydrate. The accepted values for the percent of water in the following hydrates are as follows: BaCl, 2 H,0 - 14.8%, ZnSO, 7H,0 - 43.9% MgSO, 7H,0 - 51.2%, MgCl, 6 H,O=53.2% Fe(NO), 9 H,0 = 40.1% Based on your calculations above, which of the hydrates listed was your unknown? View Notes - hydrate-lab-answers from CHEM 113 at Brigham Young University. This is a Premium document. magnesium sulfate hydrate lab answers. cone is just below the crucible. Thus, MgSO 4 may also be prepared with 1 mole of determine the percent water in an unknown hydrate, solid ionic compound that contains weakly bound water molecules in its crystalline structure, the weakly bound water molecules in a hydrate. If the compound turn yellow, remove it from the hot plate and place it on a ceramic pad (DO NOT PLACE THE HOT BEAKER ON THE COOL TABLE, IT CAN SHATTER) Allow the beaker and its contents to cool completely. The reaction for the decomposition is as follows: CuSO4 5H2O (s)= => SO2(g) + CuO (s) + 5H2O. This Chemistry experiment illustrates the Law of Definite Proportions and reinforces the concept of Composition Stoichiometry. Become Premium to read the whole document. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Why purchase my version of this. If you found this article useful, please . Furthermore, in order to determine the exact name of the hydrate, we must find out the ratio between the anhydrate and water that are associated with the hydrate. Describes the process of calculating the percent of water in a hydrate. To calculate the percent composition, we took the mass of each part of the substance and divided it by the total mass. We could have not gotten rid of the water in the hydrate to begin with as 15 minutes of heating was perhaps too short. This phenomenon could have deviated the ratio by causing a loss in the amount of water and anhydrate. An additional challenge is that both the hydrate and anhydrous salt are white.Finally, unless you frequently stir the crystals they will combine and harden, possibly trapping water inside To prevent stir continuously. Once the numbers of moles of two substances are known, the ratio can be computed by dividing them. Thus, the ratio between water and magnesium sulfate will be close to being 7:1. at a slight angle with its cover slightly ajar. Be specific. Mass of dish + hydrate 3. In this lab, we learned how to apply stoichiometry in a new way to determine a formula of a hydrate. Percent of water in hydrate (theoretical) Moles of water. Your LAB SETUP should be a sketch of the picture on the right. Lab: Determining the Composition of a HydrateFor students in Grades 8-12.INTRODUCTION:Hydrates are ionic compounds that have a number of water molecules attached as part of their structure. Calculate mass of hydrate heated 2. Examine the formula for the hydrate: CuSO, The actual mass percent of water in the hydrated copper (II) sulfate compound should have been, In the experiment involving hydrated copper sulfate, overheating causes a. You will watch the video (link provided) and obtain the data from the video. What can transform a hydrate into an anhydrous salt? KEY. 1. View WS More Hydrate Lab Practice Answer Key.pdf from CHEM 151 at Leeward Community College. Predict how experimental factors will impact the accuracy and precision of results. 1. Ratios vary in different hydrates but are specific for any given hydrate. Describe the way the anhydrous compound looks like. After obtaining the data from the video and filling out your data table, you will then perform the necessary calculations to determine the mass, video shows the heating of an unknown hydrated sample. Keep in mind, that you have to use your own data and no two reports can be exactly the same. 2. Answer 2) A hydrate that . Purpose: Determine the percent of water present in a hydrated copper (II) sulfate (CuSO 4 n H 2 O) and Epson Salts. The exact definition of a hydrate - any substance that contains some amount of water molecules in its structures - was illustrated in a precise way in this experiment. Calculate the mass of water lost from . For example, Glucose is C6H12O6; it's empirical formula is CH2O. Use the balance to weigh the metal dish with the number 1 label and record the weight in Data, 3. If clumps are formed, just continue stirring and heating until you see. Spatula Nearly half of the mass of the hydrate is composed of water molecules within the . This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Magnesium sulfate, the only left option, is white in appearance which makes it a possible identification for our hydrate. The resources include:Chemistry Unit 10--The Mole Concept Notes & Worksheets PacketChemistry Mole Quiz/PreactivityCounting by Weighing, ActivityMole Concept Quiz IMole Concept Quiz II, I have compiled all of the labs I use for my Chemistry I class into one document. According to a smaller ratio compared to the expected ratio, more water was probably lost during this occurrence, which lowered the number of water moles. By using both quantitative and qualitative approaches, we can successfully predict the identity of the hydrate and its structure consisting of anhydrate and water. the ratio was determined by dividing the moles of water by the moles of inorganic salt. Two forms of this, included for student differentiation. The number of water moles can also be known by repeating the same procedure, but with the molar mass of water instead. The water is present in a definite and consistent ratio. copper (II) sulfate hydrate Mark Bailliecoordinated the modifications ofthis activity for implementation in a 15 week fall course, with the help of Elena Lisitsyna and Karie Sanford. Light the burner with a flame that is approximately 3 to 4 cm high (1 to 2 inches Chemistry: Lab - Formula of a Hydrate . This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Use the dropper to add a very little water to the anhydrous copper (II) sulfate. Hence the percentage composition of water in CuSO4.5H2O is 36.08 %. The water is chemically combined with the salt in a definite ratio.