Use MathJax to format equations. However, immediately after the first heating, It can be clearly seen that the heated copper sulfate has now transformed into a grainy and whitish-gray form. Try a color-by-number activity. The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. Use this picture to get the mass of the hydrate (blue powder). Water, the most common chemical on earth, can be found in the atmosphere as water vapor. Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. You will be able to easily integrated it into your Learning Management System. In this lab, the five general types of chemical reactions were conducted and observations. Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. Copper Sulfate's Water of Hydration Lab Copper Sulfate's Water of Hydration Lab: Enrichment Activity Purpose - To observe the effect of removing the "water of hydration" from hydrated copper(II) sulfate. Measured mass of crucible again: 36.1571g, Measured mass of (hydrous) copper sulfate: 2.1614g, Measured mass of crucible with (hydrous) copper sulfate: 38.3189g, Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. * Salt Instead, as seen calibration results, more of each was used. Honors Chemistry - You do not need to write three paragraphs for this conclusion. 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! > A C @ 6 bjbjWW 9n 5 5 r. (3 points) Paragraph #2: What did you learn? Placed crucible on mesh pad using tongs (from this point, the crucible was handled solely with tongs until the experiment concluded), and allowed to cool to room temperature. This was the same for all five trials. Wt after: 8.22g 5 H 2 O 6. The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. At that time, the copper sulfate had turned a yellowish-white. Once dissolved, fill the rest of the volumetric . 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. cup' method. 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. Asking for help, clarification, or responding to other answers. 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 Introduction to Formulas (FREE) What did you learn? 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. The second procedure called for us to heat a number of other hydrates and test their vapors for any evidence of acid just as we had done in the previous experimental procedure. My percent error is _____. (8 points) Empirical Formula of a Hydrate Chemistry Lab. $$\Delta X=\frac{\sqrt{(\Delta W_0)^2 W_e^2+(\Delta W_e)^2 W_0^2}}{W_e^2}\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{3}$$. * Evaporating dish What will be the effect, on the mass of the residue, of not heating the hydrate enough to drive off all the water of hydration in the hydrate. X is a specific whole number value. When heated gently, the red burgundy \(\ce{CoCl2*6H2O}\) will decomposes into the violet \(\ce{CoCl2*2H2O}\) then to the blue anhydrous \(\ce{CoCl2}\). The actual percent is ____. Covering the fundamental properties, thermodynamics and behavior of hydrates in multiphase systems, this reference explains the basics before advancing to more practical applications, the latest developments and models. Did Billy Graham speak to Marilyn Monroe about Jesus? Common examples of minerals that exist as hydrates are gypsum (\(\ce{CaSO4*2H2O}\)), Borax (\(\ce{Na3B4O7*10H2O}\)) and Epsom salts (\(\ce{MgSO4*7H2O}\)). 2. Then use that information to write the formula of the hydrate. The lab has an introduction to help students understand why they are doing the lab. with an unknown hydrate to determine the mass percent of water lost and solve for the formula and name of the unknown hydrate. Copyright 2023. You can check for this by looking for the telltale brown/black color of copper oxide. The actual (true) value is 5, so the formula would be CuSO4 5H2O. When hydrates are heated, the water is released from the compound as water vapor. This worksheet is a great follow-up to 42-Naming Hydrates. When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. Grace Timler Where's my experimental error coming from? Through the use of a vacuum filtration system the mass of Cu was, Flame Test Lab Report In this lab, the student will determine the percentage of water in the hydrate by comparing the mass of the hydrate to the mass of the anhydrous salt. A. Will this likely lead to a higher or lower value of \(x\) than the actual value. A hot crucible looks like a cold one, avoid direct contact with the crucible, clay triangle and ring stand until you are sure they are cooled. 8.22/(63.5+32+64) = 0.0515mol anhydrous copper sulphate. They are very math intensive, and very conceptual in nature. 10/3/12 Save the residue and perform your calculations. Record the mass and place the solute into a 50 mL volumetric flask. Answer the questions below. 1. Download the preview file to get a look! After heating, the mass of the anhydrous compound is found to be 3.22 g. Determine the formula of the hydrate and then write out the name of the hydrate. MIP Model with relaxed integer constraints takes longer to solve than normal model, why? You did what I thought of doing but didn't get around to do. ), 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 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. What are the qualities of an accurate map? The number you found for the water replaced the x in the formula CuSO, The actual (true) value is 5, so the formula would be CuSO. 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. Lab Report 1 October 3, 2017 The electronic scales (quite cheap) were an obvious first candidate for a source of error. sulphate, calcium sulphate and lead sulphate. * Watch glass Lab Report Second, the results are great! 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. It is generally possible to remove the water of hydration by heating the hydrate. In the Hydrate lab at first, a sample of approximately 0.1000 grams of copper (II) sulfate pentahydrate was heated for the purpose to cause a chemical reaction that would remove all of the water molecules in order to determine the number of moles of water in the inorganic $X$ is the desired answer. Score 1 A student is given a cobalt (II) chloride hydrate. So thats 4.81/18 = 0.267mol water, and Some chemicals, when exposed to water in the atmosphere, will reversibly either adsorb it onto their surface or include it in their structure forming a complex in which water generally bonds with the cation in ionic substances. Pre-made digital activities. After one hour, note any change in the physical appearance of each sample. Follow the directions below to complete the lab. I havent investigated that yet, but I plan to weigh a sample before and after leaving in a warm airing cupboard overnight. * Vinegar As a result the actual Purpose: 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. 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. 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. Hydrates generally contain water in stoichiometric amounts; hydrates formulae are represented using the formula of the anhydrous (non-water) component of the complex followed by a dot then the water (\(\ce{H2O}\)) preceded by a number corresponding to the ratio of \(\ce{H2O}\) moles per mole of the anhydrous component present. Bunsen Burner or Hot PlateComplete Lesson: PPT, Warm-up, Exit Ticket, Lab PaperStudents: drive off water of hydration calculate percent water use percent water and given elemental percentages to find formulaLab 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 Qui, This is a great lab to introduce or reinforce percent composition and empirical formulas. However, some spontaneously lose water upon standing in the atmosphere, they are said to be efflorescent. 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. 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Download Free PDF View PDF For example, because for Trial 1 there was not exactly 2 mL of Copper Sulfate and 8 mL of distilled water, the concentration of the solution definitely could not be 0.080M. Making statements based on opinion; back them up with references or personal experience. Who makes the plaid blue coat Jesse stone wears in Sea Change? Did you heat the dish before weighing it to find the tare? The solvent was the dissolving substance and the solute was the substance being dissolved. Solutions were made up of two parts, the solute and the solvent. Hydrated copper sulfate (CuSO 4), hydrated ferrous sulfate, hydrated cobalt sulfate, sucrose, epson salt, 4 test tubes, . present. You'll be surprised at how much older kids like to color!This Science color-by-numbers activity includes 18 questions covering writing a formula from the name of an acid, hydroxide or hydrate or naming the compound from a chemical formula. Calculate your % error: "absolute value of . 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. When it is all white the water has been removed and the anhydrate is left. Mass a dry watch glass Add a small scoop of blue hydrate Mass the watch glass and hydrate Heat the hydrate on hot plate until all blue is gone Allow watch glass to cool Mass the watch glass and anhydrate . 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. Coloring pages - Water facts, how it helps the brain, how it helps the body, ideas on drinking more water. Chemical Changes VS Physical Changes 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. 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. Ignited Bunsen Burner, and heated crucible for 12 minutes. Why don't we use the 7805 for car phone chargers? To find the expected error in the answer, $\Delta X$, assuming no error in the molecular masses, we calculate: The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. Let's face it, percent composition and empirical formulas are not the most exciting concepts to teach in chemistry. In this lab and unknown hydrate will be heated two separate times over a Bunsen burner to remove as much water from the substance as possible, before and after heating the crucible the masses will be calculated and recorded for future reference. Lab Report Hydrates Lab Report introduction the purpose of this experiment was to explore and evaluate the bonding properties and characteristics of hydrates. Answer: Can copper-plating be reversed? Lab Question: How can lichen indicate the quality of its environment? Find out the importance of drinking plenty of water and the adverse health effects of not getting enough water. * Cup This is appropriate for all levels of chemistry. The residue obtained after heating, called the anhydrous compound, will have a different structure and texture and may have a different color than the hydrate. 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? (However, this is not likely to be the sole cause of the inaccuracies within this experiment, though it may contribute to it. Ive compared its readings at weights of about 2, about 20, and about 50g, with another similar model, and they agree to within 10mg (one digit in the final decimal place) at all weights. So now the final thing left to do is estimate how big $\Delta W_0$ and $\Delta W_e$ are. The lesson tutorial and the previous, reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. the main. Do Eric benet and Lisa bonet have a child together? A student trying to determine if a white solid is a true hydrate heats the sample and finds that there is evolution of water, that the residue obtained is soluble in water and that the solution is colorless. You will find that most students will obtain the expected results pretty much dead on, and the students love the very low percent erro, Students get to discover the formula of a hydrate with real world experimental techniques in this lab! The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate . It should be brief (aim for ten words or less) and describe the main point of the experiment or investigation. has a mass of 4.31 g before heating. By clicking Post Your Answer, you agree to our terms of service, privacy policy and cookie policy. TPT empowers educators to teach at their best. Your name and the names of any lab partners. anyhydrous salt, which forms one half of the experiment, may not be Lab Report It only takes a minute to sign up. Explain. Any time she touches the apparatus its under close supervision by myself. * Hot plate Improving the copy in the close modal and post notices - 2023 edition, New blog post from our CEO Prashanth: Community is the future of AI. 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. Does a password policy with a restriction of repeated characters increase security? B. What is "water of hydration" and how does it affect me (you)? (Qualitative Analysis). Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. Remember the hydrate is in the crucible so you need to subtract the mass of the crucible to get the mass of just the hydrate. I could perhaps have not heated the hydrate enough, and not driven off all the water but then Id have less than 5, not more, waters per mol. No. Mathematics was used to explore wate, servation of mass and the reversibility properties in question. 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 Copper Sulfate's Water of Hydration Lab: Enrichment Activity. Embedded hyperlinks in a thesis or research paper. The mass was reduced to 7.58 g. What is the formula of the hydrate? If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? Label and place all samples at the same location in the room, well out of the way so they wont be spilled. * Alka-Seltzer tablet 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. Rinse the crucible and its cover with distilled water. 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. | | What's even better is that you get credit from TpT every time you leave a constructive comment. 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. Why purchase my version of this lab? 4 fun activities! Send me a message, I'd love to hear from you! Then reheat the solution to dryness. You might also like these related lessons! In other words, the chemical equation BaCl2 + 2H2O (s) BaCl2 + 2H2O (g), labeled as 5.3 in the original lab report, is best used to describe the transition which took place during this portion of the lab. 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. Also this lab was used as an opportunity to improve the ability to write lab reports and make data tables, and to provide experience with unfamiliar lab equipment. So you will get 1 copper sulfate and your amount of water should be larger than 1 when you divide by the smallest. 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. C.7.A: The student is expected to name ionic compounds containing main gr, 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. So if I look at the calculation process you have the following equation to get from known quantities to the answer: $$X=\left(\frac{W_0}{W_e}-1\right)\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{1}$$. Some compounds like carbohydrates release water upon heating by decomposition of the compound rather than by loss of the water of hydration. Heating maybe required to provide the required activation energy. Materials: T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. These compounds are not considered true hydrates as the hydration process is not reversible. * Ammonium hydroxide ). Because this kind of reaction is usually not spontaneous. Which observations, experiences, or lesson materials helped you form your hypothesis? Heat for 5 minutes using a single-cone blue flame. Use this picture to get the mass of the anhydrate (white powder). Be sure that the flame will be close enough to the triangle to engulf the entire crucible. 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). We would call this copper sulfate pentahydrate. Platform provided by Digication, Inc. FEATURESGuided notes that have students listening to you instead of writing notes.Opt to use slides for all students and guid, This is the perfect companion to the popular chemistry lab: Determining the Formula of an Unknown Hydrate. Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). * Milk Data can be collected and most of it analyzed in a single 45-50 class period. Record the appearance of the hydrate before it is heated. I give . Also, to see the color of each reaction determining the amount of energy released using our color scale. What will be the effect, on the mass of the residue, of overheating the hydrate so that the compound decomposes. Do you have pictures of Gracie Thompson from the movie Gracie's choice. Determining which hydrate of calcium chloride I have? Part B: Hygroscopic and Efflorescent Solids Use this tool to record your data and then watch all the necessary calculations and analysis completed in seconds!This resource accompanies the lab handout/procedure here. . This means part of the copper (II) sulfate would be turned into a gas, sulfur dioxide. Its weight before cooling was 0.02g (on my scales) less than its empty weight cold. Will this likely lead to a higher or lower value of \(x\) than the actual value? This error is almost completely determined by the error in $W_e$. 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. This is a great lab to introduce or reinforce percent composition and empirical formulas. This page titled 5: Properties of Hydrates (Experiment) is shared under a CC BY-NC license and was authored, remixed, and/or curated by Santa Monica College. I have a porcelain evaporating dish to contain the hydrate during heating, electronic scales that will weigh to 300g in increments of 10mg, and commercially bought copper sulphate that is allegedly 99.5% pure. These errors made the absorbance values measured by the SpectroVis off from what it should have been. Return the evaporating dish with the hydrate to the wire gauze. - 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! Is Brooke shields related to willow shields? A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The anhydrous salt could have been exposed to air prior to measurement, and reabsorbed some moisture, thus disrupting measurements. Add highlights, virtual manipulatives, and more. * Lead II nitrate The goal of this experiment was to determine the product of copper (II) sulfate with iron. Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). Do you perhaps have any information about the nature of the .6% impurities in the original sample? $0.08$ g. Now plugging in the numbers in Eq.$(3)$ I find $\Delta X=0.14$ mol water per mol copper sulphate. For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. Why purchase my version of this lab? If a chemical reaction occurred, write a balanced equation for it. Hydrate Lab. In this lab students will heat a hydrate and from their collected data, calculate their percent error, and calculate the number of moles water in the hydrategiving them the final formula for the hydrate. This lab explored hydrates and the 4 objectives in a three procedure process through observation, experimentation, and mathematical methods to help prove whether dehydration of a hydrate is, Equipment and materials used in one or more procedure included: Hydrated copper sulfate, observation and experimentation. ALL of the Chemistry Labs you need for a WHOLE year!! $$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? What's the cheapest way to buy out a sibling's share of our parents house if I have no cash and want to pay less than the appraised value? The water is present in a definite and consistent ratio. In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. The copper sulfate moles should be the smaller. rev2023.5.1.43405. Use caution when heating the crucible and cover. * Cornstarch By comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. * Candle Be sure to subtract out the crucible before putting it into the proper space above. What can this chemical be? To participate in this lab it is, that there was no release of acidic vapors during the separating of the water and compound bonds. A minor scale definition: am I missing something? All rights reserved. Texas Chemistry Standards (TEKS) What did your group get as the formula of the hydrate? This is a student-centered, active learning lesson without lecture or notetaking! Try to avoid and popping or . The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride.
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