Answer: _____ c) Calculate the mole ratio of water to salt in the hydrate, round to the nearest whole number. Mark Bailliecoordinated the modifications ofthis activity for implementation in a 15 week fall course, with the help of Elena Lisitsyna and Karie Sanford. connected to the rest of the formula with a raised dot, formula for copper (II) sulfate pentahydrate, how do we remove the waters of hydration from a compound? iron ring Determine the number of moles of water, x, per mole of anhydrous salt and write the chemical formula of the hydrate sample. when we heat blue CuSO5HO, what happens? The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . Why do hydrates form? Thus, at the end, we learned that there are countless numbers of applications of stoichiometry in chemistry. Experiment 605: Hydrates . 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. Use the dropper to add a very little water to the anhydrous copper (II) sulfate. 8. 5. Your Lab Reports are individual assignments, but you're welcome to communicate with your group and discuss the results. This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. Copper suifate pentahydrate is used to determine the percent composition of water in a lab. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Percent Water in a Hydrate_Virtual Lab.docx. By multiplying the mass of the anhydrate, which is magnesium sulfate in the experiment, with its molar mass, the number of moles present at the end can be determined. However, there must be a few sources of errors that affected the data. Your Teammates have to be able to see and hear you. Record this figure as "Epsom salt, original (hydrated) mass" in Data Table 1. Complete your Lab Report and submit it via Google Classroom. 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. The pentahydrate is 100% isolable only in temperatures lower than 30 C. 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. Record the mass. 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. View WS More Hydrate Lab Practice Answer Key.pdf from CHEM 151 at Leeward Community College. Iron (III) sulfate has a purple tint to it, and has a crystalline structure. All students MUST be in constant contact with their teams vie Zoom Breakout Rooms. 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. Show how you determined your answer. Mass of water. Tuck the Sterno can beneath the wire stand that is included. If not, repeat the heating/cooling/weighing process until two successive weighing have the same mass. The identity of the mysterious substance was magnesium sulfate. Because the number of moles of water was lower than what it could have been originally, the ratio of water to anhydrate was 6:63:1 rather than 7:1. c. Change in the strength of the heat while maintaining the same amount of time to heat. how are the waters of hydration included in the chemical formula? Each type of hydrate traps water in its own unique way, but heating a hydrate will release the The number of water moles can also be known by repeating the same procedure, but with the molar mass of water instead. A 5.0 g sample of a hydrate of BaC12 was heated, and only 4.3 g of the anhydrous salt remained. Empty the anhydrous salt onto a large watch glass. mass lost after second heating could be 3.0662g-1.8040g = 1.2622g. hydrate lab procedure. Second, it will also determine the molar ration of water to inorganic salt in, Epsom salt. 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%. Describe the magnesium sulfate hydrate before heating, How many moles of copper (II) sulfate (CuSO. 2. Calculate mass of hydrate heated 2. Chemistry: Lab - Formula of a Hydrate . : an American History (Eric Foner), Biological Science (Freeman Scott; Quillin Kim; Allison Lizabeth), Psychology (David G. Myers; C. Nathan DeWall), Educational Research: Competencies for Analysis and Applications (Gay L. R.; Mills Geoffrey E.; Airasian Peter W.), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Brunner and Suddarth's Textbook of Medical-Surgical Nursing (Janice L. Hinkle; Kerry H. Cheever), The Methodology of the Social Sciences (Max Weber), Business Law: Text and Cases (Kenneth W. Clarkson; Roger LeRoy Miller; Frank B. FEATURESGuided notes that have students listening to you instead of writing notes.Opt to use slides for all students and guid, Chemistry Unit 10--The Mole Concept Bundle, This bundle contains the Unit 9--Chemical Reactions resources, one download. 9. 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. 1.7: Experiment 6 - Hydration of Salt is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. Mass of anhydrous salt Calculations - Remember to show all of your work. percent by mass H 2 O = mass of water x 100% mass of hydrate. Measure the mass of the empty beaker with the glass rod inside. Show your work, include units, and write your answers in the blanks on the right. Section 1: Purpose and Summary . What is lost from the CuSO4 in this process? Calculate the percent error of your experiment. If the heating continued on for longer, more water could have evaporated to the air, leaving less amount of anhydrate left in the beaker. The, requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. Without water. By using both quantitative and qualitative approaches, we can successfully predict the identity of the hydrate and its structure consisting of anhydrate and water. A student performed the experiment correctly and the initial massing correctly, but forgot to mass the crucible cover after heating. You will find that most students will obtain the expected results pretty much dead on, and the students love the very low, error and using simple steps of 1-4 find empirical formula for copper(II) sulfate crystals. Hydrates are ionic compounds that contain water molecules as part of their crystal structure. Calculate mass of water in hydrate sample. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. T T , t _' l K K K K K 2 2 2 &. Second, the results are great! Answer 2) A hydrate that . Light the burner with a flame that is approximately 3 to 4 cm high (1 to 2 inches 2) Calculate the mass of water driven out of the hydrate. Become Premium to read the whole document. 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. weighing boat. What errors would this cause in the calculation of the percent of water in the hydrate? This lab is included in Teacher Friendly Chemistry . Nearly half of the mass of the hydrate is composed of water molecules within the . What is a hydrate? represents the ratio. Its experimental ratio was 6.63 to 1 and its expected ratio was 7:1. 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. remove the burner in case of excess spattering. Accessibility StatementFor more information contact us atinfo@libretexts.org. You have just come across an article on the topic water of hydration pre lab answers. = 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. From the data the students can determine the experimental percentage of, composition and empirical formulas. Add between 0.3 and 0.8 g of Epsom salt to the metal dish, then add the combined weight of. The change from hydrate to anhydrous salt is accompanied by a . at a slight angle with its cover slightly ajar. water lost by the hydrate. copper (II) sulfate hydrate From the calculation, you can clearly see that the units of g/mol in the numerator and denominator cancel out. Includes teacher instructions, sample calculations, and, key to the conclusion questions. Clean up lab area ( point will be deducted if area is not properly cleaned ), Copyright 2023 StudeerSnel B.V., Keizersgracht 424, 1016 GC Amsterdam, KVK: 56829787, BTW: NL852321363B01, incorporated into the solid. Then the larger number of moles of water divided by the smaller number of moles of anhydrate could have produced a higher ratio that is closer to 7:1 than what we got. From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid (the formula of the anhydrous solid will be provided), the number of moles of . Place the clay triangle over the ring to Thus, the ratio between water and magnesium sulfate will be close to being 7:1. 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. Elena Lisitsynacontributed to the creation and implementation of this page. ring stand 6. Then allow it to cool and weigh it. By the addition of water to the anhydrous salt. chemical reaction changing Copper Sulfate pentaHydrate (CuSO4 . To determine what percent by mass of a hydrate is water, first determine the mass of water in one mole of hydrate. Many of the "classic" chemistry experiments are included with, few that I've tweaked over the years.Labs-Thickness of Aluminum FoilDensity CubesDensity of PenniesConservation of MassMixture SeparationIdentifying Elements, Compounds, and MixturesDimensional Analy, Chemistry Lab Bundle 1: 31 Labs, 17 Inquiry, Quiz, Key, PPT, PDF/Word, (450PAGES) CHEMISTRY MULTIPLE CHOICE Grade 11 Chemistry all units WITH ANSWERS, Chemistry Curriculum Full Year Guided Notes Bundle. Subtract the mass of the metal dish plus Epsom salt from the mass of the empty aluminum. Describe the way the anhydrous compound looks like. Why Do Organism Look Like the Way They Do. From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid, the number of moles of water and moles of the anhydrous solid are calculated as shown below (\ref{4}, \ref{5}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. What percentage of water is found in CuSOp5H20? Now, you try: calculate the percent of water in borax, Na2B4O7.10H2O. The reaction for the decomposition is as follows: CuSO4 5H2O (s)= => SO2(g) + CuO (s) + 5H2O. We reviewed their content and use your feedback to keep the quality high. Heating time and temperature are critically important for this experiment. Hydrate Math The percent of water in a hydrate can be determined in a manner similar to determining the percent composition of a compound. Use the glass end to stir the compound. Sometimes the water is liberated in stages, with one or more lower hydrates being observed during the heating process. 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. 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. From this lab, we are able to conclude that our prediction was strongly supported in both terms. Answer the questions below. To calculate the molar mass, we added up each element's atomic mass for each part of the substance. 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 Fundamental Chemistry 36. Calculate the percent water in the hydrate sample, using Equation 2, percent water, % = (mass of water lost, g/mass of hydrate heated, g) (100%), determine the mass of a hydrated salt sample and the mass of the residue after heating the sample; from these masses you will calculate the mass of water lost during heating and the percent water in the hydrate, crucible and cover, crucible tongs, Bunsen burner, ring stand and support ring, pipe-stem triangle, ceramic-centered wire gauze, microspatula, balance, preparing and weighing crucible; heating and weighing unknown hydrate. lab hydrate ratio of epsom salt answer key. The introduction to this, , students will experience the dehydration and re-hydration of, hydrated crystal, including doing the calculations involved. 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? Some sources of deviation of the data may include: a. Your LAB SETUP should be a sketch of the picture on the right. Course Hero is not sponsored or endorsed by any college or university. 1.000 g - 0.6390 g = 0.3610 g. 2. If you found this article useful, please . This phenomenon could have deviated the ratio by causing a loss in the amount of water and anhydrate. When hydrates are heated, the water is released from the compound as water vapor. 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. Mass of hydrate 4. This means we can exclude these three options from our prediction. Masses are measured beforeheating to determine the mass of theoriginal sample (the hydrate)andafterheating to determine the mass of copper (II) sulfate (CuSO4) anhydrous. Finally, this is for balancing the chemical equation of the decomposition of a hydrate. In this lab, we learned how to apply stoichiometry in a new way to determine a formula of a hydrate. Heat. The mass of water evaporated is obtained by subtracting the mass of the . Use the balance to weigh the metal dish with the number 1 label and record the weight in Data, 3. a) Calculate the mass percent of water in the hydrate? Most hydrates lose their water of hydration at temperatures slightly above 100 oC. the aluminum dish and Epsom salt to Data Table 1. Why purchase my version of this. then what do you do? 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. TPT empowers educators to teach at their best. 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. Data & Analysis. A 2.5 g sample of a hydrate of was heated, and only 1. . 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. Data can be collected and most of it analyzed, single 45-50 class period. These mu, compound. I ; O j CJ OJ QJ U56OJ QJ \] 56CJ OJ QJ \] j CJ OJ QJ CJ H*OJ QJ CJ H*OJ QJ 5>*CJ OJ QJ \5CJ OJ QJ \ CJ OJ QJ 6CJ OJ QJ ]:
m n * M N Z } ~ ( dh &. Be sure your beaker and glass rod does not have any crack, and that that they are clean and dry. 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. Write the formula of the one you chose. Once the beaker is cool, measure the mass of the beaker, the anhydrous salt and the glass rod. Two forms of this, included for student differentiation. For example, the ratio we got from an experiment for iron (III) nitrate was 13.3:1 while it should have been 9:1, according to the information from the resource. 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. This, report requires students to directly apply their understanding of Empirical Formula and, procedure. Before this, we had heard of this scientific word briefly in textbooks and in class, but we were never sure of its exact definition. CuSO5HO (s, blue)heatCuSO (s, white)+5HO (g) 3 steps to determining percent water in unknown hydrate. Predict how experimental factors will impact the accuracy and precision of results. If the mass is the same as the previous weighing, then the salt has been completely dehydrated. 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. Calculate the molar ratio of water to anhydrous solid to determine the hydrate's formula. Ans: 47.24 %. Carry out actions from the step 2 to step 4 again for aluminum dishes with numbers 2 and 3. 2.) Hence the percentage composition of water in CuSO4.5H2O is 36.08 %. 1.) Calculating amount of water in hydrate. This is a Premium document. Heat the contents again for a short time (3 minutes). magnesium sulfate hydrate lab answers. A hydrate is a compound that is chemically combined with water molecules. the ratio was determined by dividing the moles of water by the moles of inorganic salt. Experts are tested by Chegg as specialists in their subject area. Lab 09 - Percent of Water in a Hydrate Pre-Lab Questions Date: Name: - Section: Instructor: - Read the following laboratory experiment and answer the questions below. Use the information to answer the questions. 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). Measure and record the mass of a clean, dry, empty crucible. Students will be determining the number of, procedure goes along with the corresponding, involves the heating of an unknown hydrated sample (magnesium sulfate heptahydrate). 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 Step 3: Think about your result. To make sure that, each element has the equal number of atoms on both sides of the equation, coefficients were. The water in a hydrate is bound loosely, and so is relatively easily removed by heating. Add highlights, virtual manipulatives, and more. Pre-lab: (Show all work and necessary units) In a minimum of one (1) paragraph summarize . BOLD and Change the color of your answer to RED so the teacher could easily find them! The last idea we learned was how to apply the knowledge of colors of specific ions and solids. Log in, How to calculate the empirical formula of a hydrate. Record the final mass of the anhydrous salt in you lab notebook and do the calculations to show that the molar ratio of water to anhydrous salt really is 5:1. First, this experiment is focusing on how to determine the water content of a hydrate by heating. Want to include, experiment that correlates with Stoichiometry? ? The change from hydrate to anhydrous salt is accompanied by a change in color: 1. 120.3 g percentage of water in hydrate (from teacher) 51.2 % Processing Your Lab Data. 1. 3. Click edit button to change this text. Use matches or a lighter to start the Sterno can on fire. 3.) Spatula This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. 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}). Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO. 4. Key Term hydrate lab answers; This preview shows page 1 . Place your beaker with the sample and the rod on the hot plate. A hydrate is a chemical compound, generally ionic, that has weakly bonded to it a specific number of water molecules per formula unit. this experiment.Materials needed:Copper(II) sulfate pentahydratecruciblehot plate or bunsen burner setupcrucible tongswaterLab also includes assessment questions from the NYS Regents Examination. xH2O). This is a oneperiod lab where you will be working in your Kitchen Chemistry Lab while connected with your group via Zoom Breakout Rooms. Includes: title page, teacher guide, and two-page, an ionic jail and can only escape using heat! . Ratios vary in different hydrates but are specific for any given hydrate. 9H2O), 1.48g CuSO4x 1 mol CuSO4/ 159.61g mol-1CuSO4 = 0.009273 mol CuSO4, 1.47g H2O x 1 mol H2O / 18.02g mol-1H2O = 0.08158 mol H2O, number of moles H2O / number of moles CuSO4, = 0.08158 mol / 0.009273 mol = 8.80 mol H2O / 1 mol CuSO4 (3 significant figures), 1.48g MgSO4x 1 mol MgSO4/ 120.36g mol-1MgSO4= 0.01230 mol MgSO4, number of moles H2O / number of moles MgSO4, = 0.08158 mol / 0.01230 mol = 6.63 mol H2O / 1 mol MgSO4, 1.48g FeCl3x 1 mol FeCl3/ 162.20g mol-1FeCl3= 0.009125 mol FeCl3, number of moles H2O / number of moles FeCl3, = 0.08158 mol / 0.009125 mol = 8.94 mol H2O / 1 mol FeCl3, 1.48g Fe(NO3)3 x 1 mol Fe(NO3)3/ 241.86g mol-1Fe(NO3)3= 0.006120 mol Fe(NO3)3, number of moles H2O / number of moles Fe(NO3)3, = 0.08158 mol / 0.006120 mol = 13.3 mol H2O / 1 mol Fe(NO3)3. You will watch the video (link provided) and obtain the data from the video. 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? (process and specific method used here). how should crucible FIRST be arranged on ring? water of crystallization lab report. 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%. How can we experimentally determine the formula of an unknown hydrate, A? Answer: _____ b) Calculate the number of moles of water in the hydrate sample that were driven off by heating? , 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. Answer1) A hydrate is a solid ionic compound that contains specific number of water molecules in its crystal structure. dish. The hydrate was heated until all the water evaporated, and the mass of the remining anhydrous salt was measured. To calculate the percent composition, we took the mass of each part of the substance and divided it by the total mass. While these do not have teacher directions, most labs are fairly self-explanatory and have materials lists provided. Heat the compound gently Note the release of any steam from the beaker. Robert E. Belford(University of Arkansas Little Rock; Department of Chemistry) led the creation of this page for a 5 week summer course. crucible & cover Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Describe what happens in your lab notebook. Chem 1402: General Chemistry 1 Lab (Baillie), { "1.01:_Course_Information" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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