Conclusion The mass percent of water in copper sulfate pentahydrate is _______. Rounded to the nearest integer, the ratio is 1:5. Observations on structure, texture , wetness, etc. Your lab report must contain the following information: 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. 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. Ive now heated the dish over a hot blue natural gas flame for ten minutes. 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. 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 8.22/(63.5+32+64) = 0.0515mol anhydrous copper sulphate. This means part of the copper (II) sulfate would be turned into a gas, sulfur dioxide. The purpose of the flame test lab was to further study the process of electron excitation. 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. Interpreting non-statistically significant results: Do we have "no evidence" or "insufficient evidence" to reject the null? The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. rev2023.5.1.43405. Use this picture to get the mass of the hydrate (blue powder). This was the same for all five trials. Given the data presented above, findings showed the experimental percentage of water within the hydrated salt to be: 47.10%, The accepted percentage of water within hydrated copper sulfate is:36.07%, As such, the percent error within this measurement is30.57%, The experimental stoichiometric ratio between copper sulfate and water was found to be: 1:5.314, The accepted stoichiometric ratio between copper sulfate and water is: 1:5, The percent error within this measurement is 5.909%. There was no sign of $\ce{CuO}$ after the heating. The best answers are voted up and rise to the top, Not the answer you're looking for? 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. Introduction Naming and Formulas: Simple Ionic and Covalent Compounds Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. Place the crucible, hydrated copper sulfate, and lid on/in your clay triangle. has a mass of 4.31 g before heating. Let's face it, percent composition and empirical formulas are not the most exciting concepts to teach in chemistry. Download Free PDF View PDF * Hot plate Chemical Reaction Lab Report 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. . 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. Cool (approximately 10 minutes) and get the mass of the anhydrate (white compound). To participate in this lab it is, that there was no release of acidic vapors during the separating of the water and compound bonds. Ms. Macielag's Thursday Lab Class (Honors), Building and Identifying All Organic Compounds, Lab Book: Setting Up Graphing Reference Sections, Naming and Writing Formulas (without Formula Mass). -Bunsen burner Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. Chemistry Experiment # _____ Percent of Water in Copper II Sulfate Pentahydrate Name_____ Section_____Date_____ Name(s) of Lab Partner(s) . The weight after cooling of the evap dish is constant. Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. At that time, the copper sulfate had turned a yellowish-white. 2. We would call this copper sulfate pentahydrate. This is a student-centered, active learning lesson without lecture or notetaking! The solvent was the dissolving substance and the solute was the substance being dissolved. +1. Use MathJax to format equations. Hydrate Lab. Academic Chemistry - Three paragraph conclusion. Weigh the crucible with its cover to the nearest 0.001 g. Making sure to handle the crucible and its cover with clean tongs, add about 1 g (weighed to the nearest 0.001 g) of the unknown hydrate. Furthermore, the Copper Sulfate and the distilled water had to be thoroughly mixed up by shaking the test tubes. Happy teaching and have an, Students find the Empirical Formula of Epsom Salt. 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 . From this, we can calculate the ratio of salt to water (by calculating the molar and stoichiometric ratios), and the percentage of water (by mass) within the hydrated salt (by dividing the mass of the water, by the mass of the hydrated salt, then multiplying the resulting decimal by 100). Let the residue cool down (put the test tube in a beaker not on a plastic test tube rack) then try to dissolve in about 3 mL of water (about 1/3 of the small test tube), warming gently if necessary to dissolve the residue (dissolve only substances that have shown condensation). This lab will go in your lab book. Introduction to Formulas (FREE) You did what I thought of doing but didn't get around to do. 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. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Send me a message, I'd love to hear from you! Explain. 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). The goal of this experiment was to determine the product of copper (II) sulfate with iron. 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. 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. The iron oxidation state was, Copper-Iron Stoichiometry TPT empowers educators to teach at their best. This resource will come to you as a Google Doc. where $W_0$ is the start weight, $W_e$ the end weight and $M_i$ is the respective molecular mass. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. In this section you will observe the changes in the physical properties of compounds, including wetness, color, structure, texture and mass. In this section we will demonstrate the dehydration and re-hydration of cobalt (II) chloride hexahydrate. Lab Report 1 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 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. $X$ is the desired answer. Reasons to use this instead of removing water from a hydrateYou want to do a "trial run" of the lab before performing it with your studentsYou don't have a labYou don't have enough lab materials or che, In this lab, students will remove the water from copper (II) sulfate pentahydrate by heating and determine the empirical formula. Record the values as initial masses of containers and samples. This error is almost completely determined by the error in $W_e$. If a CHEM Gently heat the hydrate by moving the burner back and forth around the dish. Does a password policy with a restriction of repeated characters increase security? Hydrate: A compound that contains the water molecule. February 29, 2016 This is written CuSO4 . Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. * Ammonium hydroxide 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. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Quizzes with auto-grading, and real-time student data. When dissolved in water, the anhydrous compound will have a color similar to that of the original hydrate even if it had changed color going from the hydrate to the anhydrous compound. ** Interested in my other Chemistry Resources?? Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. Determining which hydrate of calcium chloride I have? left exposed for any length of time. In this lab, the five general types of chemical reactions were conducted and observations. Grace Timler Second, the results are great! The hydrate being, Nomenclature for Acids and Hydrates: Naming & Writing Formulas (Nomenclature) for Acids & Hydrates.In this lesson students are introduced to naming and writing formulas for acids and hydrates. Common examples of minerals that exist as hydrates are gypsum (\(\ce{CaSO4*2H2O}\)), Borax (\(\ce{Na3B4O7*10H2O}\)) and Epsom salts (\(\ce{MgSO4*7H2O}\)). 1. Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! Eventually, a linear equation that showed the relationship between absorbance and. 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. Which observations, experiences, or lesson materials helped you form your hypothesis? Experimental data may be collected with other students in introductory chemistry labs. \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\]. The results for the heating, Title: Title of lab/experiment. |Score | Then using the A, B symbols, this lab will be to determine the percent water in an unknown hydrate, determine the moles of water present in each mole of the unknown substance, and to use the molecular mass to find the empirical formula of a hydrate. All rights reserved. Add highlights, virtual manipulatives, and more. * Phenolphthalein Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. The equation for the decomposition of copper (II) sulfate is CuSO4 (aq) ==> SO2(g) + CuO(s). Its weight before cooling was 0.02g (on my scales) less than its empty weight cold. 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. Three different versions! Then use that information to write the formula of the hydrate. The water present in the latter case is called water of hydration or water of crystallization. Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). 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 This lab will go in your lab book. The date the lab was performed or the date the report was submitted. 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. So thats 4.81/18 = 0.267mol water, and Wt before: 13.030.9836 = 12.82g hydrate 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. * Iodine Heat the blue copper(II) sulfate until it has turned . To find the expected error in the answer, $\Delta X$, assuming no error in the molecular masses, we calculate: This worksheet is a great follow-up to 42-Naming Hydrates. First, a pre-weighed sample of the unknown sulfate salt will be dissolved in water. Will this likely lead to a higher or lower value of \(x\) than the actual value? Test tubes Water adheres to the dish when the dish is at room temperature. Some compounds may possess some of the properties of hydrates without being true hydrates. 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. 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. 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. In this lab, a SpectroVis was used to determine the concentration of an unknown substance. Have you ever wondered why you get a lot of headaches, your muscle doesnt function as well and your immune system is low? Paragraph #2: What did you learn? Heating will shift the equation of dehydration below to the right since it is an endothermic reaction. Copper Sulfate's Water of Hydration Lab: Enrichment Activity. Minutes in set-up time! Lab Report 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. Write the goal of the lab or the question you tried to answer. In this activity, I will construct an electroplating apparatus and observe the process of electroplating. Our first constant mass was 28.3208gand the average mass turned out to be 28.3222g. What does that x value tell you? Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). AB1 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! They are typically named by stating the name of the anhydrous component followed by the Greek prefix specifying the number of moles of water present then the word hydrate (example: \(\ce{MgSO4*7H2O}\): magnesium sulfate heptahydrate). The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. (Full Name) 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. (8 points) 5 H 2 O 6. Iron (III) chloride. Instead you are to complete the three problems below in your lab book using what you learned from the lab.
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