Wt after: 8.22g Set the crucible with its cover slightly open on a clay triangle and heat strongly for at least 10 minutes. The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. Lab reports are due week of September 29 October 3, 2014. Copper/Iron Stoichiometry Grace Timler AB1 October 3, 2017 Abstract The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8.001 grams of copper (II) sulfate, CuSO4, and 2.0153 grams of iron powder, Fe.
B. The mass was reduced to 7.58 g. What is the formula of the hydrate? 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. . To learn more, see our tips on writing great answers. 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. - 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! The equation for the decomposition of copper (II) sulfate is CuSO4 (aq) ==> SO2(g) + CuO(s). 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. The water present in the latter case is called water of hydration or water of crystallization. Why don't we use the 7805 for car phone chargers? Write the chemical formula of the hydrated form of your unknown sample. Moles of water per mole of \(\ce{CoCl2}\): What color would you expect to see when this student dissolves the blue residue in water at the end of the experiment? * Watch glass
February 29, 2016 ** Interested in my other Chemistry Resources?? How many moles of water (x) do you think are in this hydrate? Easel assessment included with this lesson plan.CDC HEALTH STANDARD SEVEN: Students will demonstrate the ability to practice health enhancing behaviors and to avoid or re, 9 worksheets to practice naming and writing formulas for ionic and covalent compounds, including acids and hydrates. The reason why this is a source of error is because as time passed between the measurements, the copper sulfate hydrate sample absorbed humidity (water) from the atmosphere and therefore increased its mass. Pour the used nitric acid in the waste container provided. anyhydrous salt, which forms one half of the experiment, may not be 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? The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . Students chew bubble gum to remove sugar instead of removing water from a hydrate. I havent investigated that yet, but I plan to weigh a sample before and after leaving in a warm airing cupboard overnight. Measure the mass of the empty crucible using the balance.
In this section you will try to determine through the testing of a series of compounds, which ones are true hydrates. rev2023.5.1.43405. 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. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. 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. As a result the actual 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 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. or iron(III) compounds, when exposed to air. I weighed out some of the hydrate into another dry dish, flattened it out as much as possible within the confines of the dish to expose as much surface area as possible, and left it in the airing cupboard for 24h at 26 degrees Celsius. Weigh out approximately 3 grams of copper(II) sulfate pentahydrate into a clean, dry large ignition tube (25 x 200 mm). 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. At that time, the copper sulfate had turned a yellowish-white. Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. The date the lab was performed or the date the report was submitted. For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. These errors made the absorbance values measured by the SpectroVis off from what it should have been. The name of this compound is "copper sulfate pentahydrate". In this part, pea-, sized samples (1-3g) were place separately in test tubes and heated for approxim, Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Educational Research: Competencies for Analysis and Applications (Gay L. R.; Mills Geoffrey E.; Airasian Peter W.), Brunner and Suddarth's Textbook of Medical-Surgical Nursing (Janice L. Hinkle; Kerry H. Cheever), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Civilization and its Discontents (Sigmund Freud), Business Law: Text and Cases (Kenneth W. Clarkson; Roger LeRoy Miller; Frank B. When it is all white the water has been removed and the anhydrate is left. The difference between 5.00 and 5.16 is a weight error of about 200mg, and I was really careful, so this seems unlikely. 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). 2. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. This means, This lesson plan assists elementary students in understanding why it is important to drink plenty of water. 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. Will this likely lead to a higher or lower value of \(x\) than the actual value. Do you perhaps have any information about the nature of the .6% impurities in the original sample? { "01:_Using_Excel_for_Graphical_Analysis_of_Data_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_The_Densities_of_Solutions_and_Solids_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Paper_Chromatography-_Separation_and_Identification_of_Five_Metal_Cations_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Inorganic_Nomenclature_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Properties_of_Hydrates_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Types_of_Chemical_Reactions__(Experiment)" : "property get [Map 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MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Hydrate", "authorname:smu", "showtoc:no", "license:ccbync" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FAncillary_Materials%2FLaboratory_Experiments%2FWet_Lab_Experiments%2FGeneral_Chemistry_Labs%2FOnline_Chemistry_Lab_Manual%2FChem_11_Experiments%2F05%253A_Properties_of_Hydrates_(Experiment), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 6: Types of Chemical Reactions (Experiment), Formula of a Hydrate (\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)), Part A: Reversibility of hydration (optional, by Instructor), Part B: Hygroscopic and Efflorescent Solids, Part D: Determination of the formula of a hydrate, Pre-laboratory Assignment: Properties of Hydrates, Part A: Reversibility of Hydration (Optional), Identification of hydrates in a group of compounds, Investigation of the properties of hydrates, Determination of the number moles of water of hydration in a hydrate. +1. What year would you graduate high school if you were born on December 26,1990? I can also customize anything you've already purchased.Check out some of my other work!Atomic StructureIonic CompoundsNomenclatureGeneral ChemistryScientific Method, End your nomenclature unit with a lab! Building on previous knowledge of ions and formulas from Part One & Two are included in the Exit Ticket and the Homework. Lab Report
* Water
If a CHEM Follow the directions below to complete the lab. Then I re-weighed. 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. copper (II) sulfate hydrate. The electronic scales (quite cheap) were an obvious first candidate for a source of error. How to apply a texture to a bezier curve? This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. A chemical reaction is when substances (reactants) change into other substances (products). 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. sulphate, calcium sulphate and lead sulphate. Kieran Sidebotham Instead you are to complete the three problems below in your lab book using what you learned from the lab. 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. Ignited Bunsen Burner, and heated crucible for 12 minutes. However, because the solutions were not mixed long and thoroughly enough, this made further deviations from what the data should have looked like. * Milk
Experimental data may be collected with other students in introductory chemistry labs. Rounding out with new case study examples, this new edition gives engineers an im, This PowerPoint is intended to introduce high school students formulas of hydrates. The actual (true) value is 5, so the formula would be CuSO4 5H2O. Materials: Crucible and lid (or use aluminum foil if you don't trust children to drop the lids), electronic balances, bunsen burners, tongs, strikers, clay triangles, ring stand and ring. Using crucible tongs, clean a porcelain crucible and its cover using concentrated nitric acid (6 M). \[ \underbrace{\ce{CuSO4*5H2O (s)}}_{\text{Deep Blue}} \ce{->[\Delta]} \underbrace{ \ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{+ 5 H2O (g)} \label{1}\], \[ \underbrace{\ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{->[\ce{H2O (l)} ]} \underbrace{ \ce{CuSO4 (aq)}}_{\text{Deep Blue}} \label{2}\]. Learn more about Stack Overflow the company, and our products. Heating maybe required to provide the required activation energy. 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). Paragraph #1: Purpose and a brief description of what you did. Have you ever wondered why you get a lot of headaches, your muscle doesnt function as well and your immune system is low? Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! Texas Chemistry Standards (TEKS) Another possibility would be to get more accurate equipment, to replicate the experiment within a dehumidified environment, and/or perform the experiment using a larger crucible (to reduce the possibility that spatter from the hydrated salt could leave the crucible). The copper sulfate is dissolved in 100ml of water that is distilled and contained in . This will result in the precipitation of . If the correct formula of copper sulfate is CuSO4.5H20, determine your percent error. T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. Updated sections include a new hydrate toolbox, updated correlations and computer methods. After one hour, note any change in the physical appearance of each sample. ALL of the Chemistry Labs you need for a WHOLE year!! If a chemical reaction occurred, write a balanced equation for it. That is how I taught it during my first years of teaching, and even though I have a lab room now, I still love and use this activity! However, this lab allows them to apply what they've learned about percent composition, hydrates, and empirical formulas in a real world example! Distilled, Precipitation Reactions clip art, assessment, writing prompt, art activity, answer key, printables, no prep needed. (Full Name)
$0.08$ g. Now plugging in the numbers in Eq.$(3)$ I find $\Delta X=0.14$ mol water per mol copper sulphate. 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. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. Calculate the change in mass for each sample. A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. * Iodine
Also, to see the color of each reaction determining the amount of energy released using our color scale. This lab will go in your lab book. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. As such, there is always the possibility of inaccuracies with measurement, perception of measurement, inaccuracies of equipment, and other such errors. Through this the appropriate reaction had to be determined out of the two possibilities. All rights reserved.
4 fun activities! Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). 1. Paragraph #2: What did you learn? temperature change caused by the reaction is hard to measure. Answer the questions below. Lab 1: Determining the Empirical Formula of a Compound, Lab 2: Determine the Percentage of Water in a Hydrate, Lab 16: Gravimetric Determination of a Precipitate, Lab 14a: Separation and Analysis of Cations, Lab 18: Separation by Liquid Chromatography, Lab 6a: Standardizing a Solution of Sodium Hydroxide, Lab 33: Determination of Calcium Carbonate Content of and Anti-Acid Pill, Lab 28: Molecular Interaction in Ethanol and Acetone, Obtained crucible and lid (henceforth, the two are considered to be together unless mentioned otherwise), inspected them, and measured their mass: 36.1574g, Obtained equipment, set up ring stand, Bunsen Burner, clay triangle, and mesh pad. Other compounds can spontaneously absorb water from the surrounding atmosphere, they are said to be hygroscopic. Label and place all samples at the same location in the room, well out of the way so they wont be spilled. Connect and share knowledge within a single location that is structured and easy to search. Try to avoid and popping or . Use caution when heating the crucible and cover. This lab will go in your lab book. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate . 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 actual percent is ____. What will be the effect, on the mass of the residue, of overheating the hydrate so that the compound decomposes. Coloring pages - Water facts, how it helps the brain, how it helps the body, ideas on drinking more water. This error is almost completely determined by the error in $W_e$. Water, the most common chemical on earth, can be found in the atmosphere as water vapor. Name: Kamaal Thomas |Date: January 4, 2011 | |Graded Assignment
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. Some hygroscopic substances, such as \(\ce{P2O5}\) and anhydrous \(\ce{CaCl2}\), are widely used to dry liquids and gases (see experiment on the Molecular Weight of \(\ce{CO2}\)); they are referred to as desiccants. What is "water of hydration" and how does it affect me (you)? This mass was taken before the substance was heated. 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. Materials:
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 water and moles of the anhydrous solid are calculated as shown below (\ref{4}, \ref{5}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. So thats 4.81/18 = 0.267mol water, and The copper sulfate moles should be the smaller. 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 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. Download the preview file to get a look! Water lost: 4.60g. I would go with a full fledged error propagation analysis on this one, because without systematic approach you might be guessing forever. 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? Even though it was close, the molarities of the five solutions were not exactly the ones that should have been used to carry out the lab. MathJax reference. They are very math intensive, and very conceptual in nature. Which is very close to the actual error you find. Use MathJax to format equations. The formula for hydrated copper sulfate is: Possible improvements that could be made to this experiment in the future could include increasing the sample size, to produce a more average measurement. To subscribe to this RSS feed, copy and paste this URL into your RSS reader. -Pre soaked popsicle, Graded Assignment (3 points) Empirical Formula of a Hydrate Chemistry Lab. 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. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. Pre-made digital activities. In an evaporating dish, gently heat a small amount (0.3 0.5 g) of \(\ce{CoCl2*6H2O}\) crystals until its color changes to violet then to blue. Three different versions! This is a student-centered, active learning lesson without lecture or notetaking! Copyright 2023. Also as I was calculating the empirical formula, I wasn't quite sure the figures were correct so I might have miscalculated. NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). A. * Pipet
Cool (approximately 10 minutes) and get the mass of the anhydrate (white compound). The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? Where's my experimental error coming from? This is written CuSO4 . Still working on that - I'm going to leave a sample fresh from the bottle in a warm cupboard overnight tonight, and see if it gets any lighter.
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