Then I re-weighed. There is an example problem included. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. I give . Observations on structure, texture , wetness, etc. 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. Quizzes with auto-grading, and real-time student data. anyhydrous salt, which forms one half of the experiment, may not be 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. * Copper II sulfate
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 best answers are voted up and rise to the top, Not the answer you're looking for? Includes teacher instructions, sample calculations, and a key to the conclusion questions. 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. Previous to an exposure to heat via the stove, it can be seen that the copper sulfate bear the natural form and colour of a bright blue crystal. Score Is Brooke shields related to willow shields? 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. 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. It should be brief (aim for ten words or less) and describe the main point of the experiment or investigation. By comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. { "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 MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Gravimetric_Analysis_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Reaction_Stoichiometry_and_the_Formation_of_a_Metal_Ion_Complex_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Evaluating_the_Cost-Effectiveness_of_Antacids_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Vitamin_C_Analysis_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11A:_The_Molecular_Weight_of_Carbon_Dioxide_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11B:_The_Dumas_Method_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Calorimetry_and_Hess\'s_Law_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Measuring_Manganese_Concentration_Using_Spectrophotometry_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14A:_Atomic_Emission_Spectra_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14B:_Atomic_Emissions_Spectra_-_Pizza_Box_Version_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Using_Periodic_Properties_to_Identify_Group_2A_Cations_and_Group_7A_Anions_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Qualitative_Analysis_of_Everyday_Chemicals_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_VSEPR_Theory_and_Shapes_of_Molecules_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Introduction_to_the_Structures_and_Isomerism_of_Simple_Organic_Molecules-_Description_and_Modeling_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Chem_10_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_11_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_12_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_9_Experiments : "property get [Map 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. Students will perform an experiment to find the hydrate formula. In this experiment, the percentage by mass of sulfate in an unknown sulfate salt will be determined by gravimetric analysis. Hydrated Copper (II) Sulphate Experiment Report Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. We would call this copper sulfate pentahydrate. 5: Properties of Hydrates (Experiment) - Chemistry LibreTexts Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. Place the crucible, hydrated copper sulfate, and lid on/in your clay triangle. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. 10/3/12
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 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. present. 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. If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Hydrate Lab. However, some spontaneously lose water upon standing in the atmosphere, they are said to be efflorescent. 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. Two sources of error include _____. At that time, the copper sulfate had turned a yellowish-white. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. Then use that information to write the formula of the hydrate. When heated gently, the red burgundy \(\ce{CoCl2*6H2O}\) will decomposes into the violet \(\ce{CoCl2*2H2O}\) then to the blue anhydrous \(\ce{CoCl2}\). There are some possible sources of experimental error for this lab Connect and share knowledge within a single location that is structured and easy to search. My percent error is _____. First, it is so easy to set upnot much prep at all. cup' method. 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. The number you found for the water replaced the x in the formula CuSO4 xH2O. Heating on the other hand would introduce heat change and thus a Add highlights, virtual manipulatives, and more. (8 points)
Copyright 2023 StudeerSnel B.V., Keizersgracht 424, 1016 GC Amsterdam, KVK: 56829787, BTW: NL852321363B01, The purpose of this experiment was to explore and evaluate the bonding properti, the percentage of water is various hydrates, (3) Determine if dehydrati, versible change, and (4) Determine the mathematical relat. 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}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. . 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. | |
Name: Kamaal Thomas |Date: January 4, 2011 | |Graded Assignment
* Alka-Seltzer tablet
Chemistry Experiment # _____ Percent of Water in Copper II Sulfate Pentahydrate Name_____ Section_____Date_____ Name(s) of Lab Partner(s) . Little or no prior knowledge of finding empirical formula necessary. You will be able to edit the document to your needs and share it with your students. 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. Excellent layout. Why purchase my version of this lab? Lab Report 1 Student exploration Graphing Skills SE Key Gizmos Explore Learning. 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. Finding the formula of hydrated copper(II) sulfate Embedded hyperlinks in a thesis or research paper. Explain what may have happened. Mathematics was used to explore wate, servation of mass and the reversibility properties in question. Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? 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 . * Lead II nitrate
Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride. > A C @ 6 bjbjWW 9n 5 5 r. To achieve this, a known mass of hydrated salt was heated, evaporating the water (essentially distillation). Period: 5 Write the chemical formula of the hydrated form of your unknown sample. 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. To determine the mass of the water, subtract the anhydrate from the hydrate and put it in the proper space above. What will be the effect, on the mass of the residue, of overheating the hydrate so that the compound decomposes. All metal sulphate are soluble in water, except barium TPT empowers educators to teach at their best. 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.
To participate in this lab it is, that there was no release of acidic vapors during the separating of the water and compound bonds. 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. PDF Chemistry Honors Lab - NJCTL Also, to see the color of each reaction determining the amount of energy released using our color scale. 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. : an American History (Eric Foner), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Biological Science (Freeman Scott; Quillin Kim; Allison Lizabeth), The definition of a hydrate is a chemical that contai, ), hydrated ferrous sulfate, hydrated cobalt sulfate, sucrose, epson salt, 4 test tubes, test, Seidel's Guide to Physical examination (043), Educational Psychology and Development of Children Adolescents (D094), Language Arts Instruction and Intervention (C365), Health Assessment Of Individuals Across The Lifespan (NUR 3065L), Introduction To Project Management Software (CSBU539), PHIL ethics and social responsibility (PHIL 1404), Professional Application in Service Learning I (LDR-461), Advanced Anatomy & Physiology for Health Professions (NUR 4904), Principles Of Environmental Science (ENV 100), Operating Systems 2 (proctored course) (CS 3307), Comparative Programming Languages (CS 4402), Business Core Capstone: An Integrated Application (D083), A&p exam 3 - Study guide for exam 3, Dr. Cummings, Fall 2016, BMGT 364 Planning the SWOT Analysis of Silver Airways, Lesson 13 Paleoseismology Case Studies; Induced Seismicity, Skill Blood Admin - Active Learning Template, Philippine Politics and Governance W1 _ Grade 11/12 Modules SY. In this lab, the five general types of chemical reactions were conducted and observations. I started with the hydrate, heated it in the evap dish over a flame (using a gas cooker ring) until it had all turned greyish white, then allowed it to cool and weighed again. Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. This mass was taken before the substance was heated. which is stored for some time will have iron(III) sulphate A substance is classified as efflorescent if its mass decreases by 0.005 g or more; and it is classified as hygroscopic if its mass increases by 0.005 g or more. 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. 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. The actual (true) value is 5, so the formula would be CuSO4 5H2O. 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). Answer: Can copper-plating be reversed? 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. Ammonium sulphide. Purpose: To observe the difference between chemical and physical changes. temperature change caused by the reaction is hard to measure. dissolved is another. 6. * Ammonium hydroxide
Will this likely lead to a higher or lower value of \(x\) than the actual value? ), Not all of the water may have evaporated during heating (Also unlikely, for the same reason as the one above. How do you feel in the morning when you wake up? Purpose: The Composition of a Hydrate Lab - Teach Basic Percent Composition! 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). Center the crucibles cover and let it cool down to room temperature. Students should know how to name ionic compounds (39-Naming Ionic Compounds) and how to convert from grams to moles (60-Mole Convers, Students learn about hydrates - the ionic compounds with water physically associated with them! Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. Percent Composition of a Hydrate Lab - Chemistry Classes / Ronald Record the values as initial masses of containers and samples. Use MathJax to format equations. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. Materials: Tests tubes (small or medium size), watch glasses, crucible* and cover*, crucible tongs, clay triangle. This lesson also covers the benefits of daily exercise an, Naming and Formulas: Polyatomic Ion Compounds and Hydrates Lesson Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). Solutions were made up of two parts, the solute and the solvent. This will result in the precipitation of . The copper sulfate moles should be the smaller. Is it safe to publish research papers in cooperation with Russian academics? Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. . * Phenolphthalein
Accessibility StatementFor more information contact us atinfo@libretexts.org. Im teaching chemistry to a home-ed 15 year old. Record the mass and place the solute into a 50 mL volumetric flask. Source: Royal Society of Chemistry. This lab will go in your lab book. 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. (Qualitative Analysis). AB1 Percent error = |Actual - Theoreticall * 100 Theoretical 2. Other compounds can spontaneously absorb water from the surrounding atmosphere, they are said to be hygroscopic. Determining the Empirical Formula of a Hydrate Lab 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. left exposed for any length of time. Determining the Water Percentage Within Copper Sulfate - WritingBros so with this last source of error you edited in (the 0.02 g) my estimate of $\Delta W_e=0.1$g actually seems quite realistic. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). 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. Period 3 The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. 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? 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. 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 Materials: When you have finished, submit this assignment to your teacher by the due date for full credit. Use caution when heating the crucible and cover. 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. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Measure the mass of the empty crucible using the balance. Score October 3, 2017 1. Return the evaporating dish with the hydrate to the wire gauze. ), 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.
Leanna Roacher Tulsa Oklahoma,
Where Does Richard M Daley Live Now,
Iep Goals For Autism Preschool,
Swindon Health Centre Islington Street,
Articles C
