TPT empowers educators to teach at their best. (8 points) Use this picture to get the mass of the anhydrate (white powder). Purposive Communication Module 2, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. As a result the actual I can also customize anything you', Looking for an engaging way for your students to review nomenclature for acids, bases and hydrates? So assuming that 26 degrees is not warm enough to cause partial loss of water of crystallisation, that suggests that at best my hydrate is only 98.36% pure, not 99.5 as it says on the bottle (typo corrected above). The error you find falls within the worst-case expected error due to impurity and potentially adhered water. 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%. 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. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis. Determining the Water Percentage Within Copper Sulfate - WritingBros $$\Delta X=\frac{\sqrt{(\Delta W_0)^2 W_e^2+(\Delta W_e)^2 W_0^2}}{W_e^2}\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{3}$$. This error is almost completely determined by the error in $W_e$. 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. Instead, as seen calibration results, more of each was used. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. Heating maybe required to provide the required activation energy. Mathematics was used to explore wate, servation of mass and the reversibility properties in question. Its weight before cooling was 0.02g (on my scales) less than its empty weight cold. Copper Sulfate's Water of Hydration Lab: Enrichment Activity. These errors made the absorbance values measured by the SpectroVis off from what it should have been. Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. Measured mass of crucible with anhydrous copper sulfate: 37.3005g. Will this likely lead to a higher or lower value of \(x\) than the actual value. Introduction - Hydrated Ionic Compounds, commonly called, "hydrates". Use crucible tongs when cleaning the crucible with concentrated nitric acid. . Period: 5 Follow the directions below to complete the lab. By comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. The Homework includes all ionic compound possibilities: binary, ternary, multivalent cations, acids, and hydrates. 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). PDF Chemistry Honors Lab - NJCTL 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. Save the residue and perform your calculations. 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. Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! Making statements based on opinion; back them up with references or personal experience. A. 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? * Alka-Seltzer tablet Why purchase my version of this lab? 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}). 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. The title says what you did. So thats 4.81/18 = 0.267mol water, and Do you perhaps have any information about the nature of the .6% impurities in the original sample? We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. Use the information collected in lab found below to fill in the blanks for the gram amounts above: Use this picture to get the mass of the empty crucible and fill it in above. 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. Learn more about Stack Overflow the company, and our products. * Salt Use MathJax to format equations. Name: Kamaal Thomas |Date: January 4, 2011 | |Graded Assignment 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. temperature change caused by the reaction is hard to measure. Second, the results are great! This lab will go in your lab book. Solved Post-Lab Questions 1. If the correct formula of - Chegg 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. Firstly to clarify a chemical change is defined as a change resulting. Do you have pictures of Gracie Thompson from the movie Gracie's choice. MIP Model with relaxed integer constraints takes longer to solve than normal model, why? Asking for help, clarification, or responding to other answers. 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. Heating on the other hand would introduce heat change and thus a In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. On an analytical balance, weigh a pea-sized sample of each of the compounds below on separate clean and dry watch glasses. We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. Introduction to Formulas (FREE) You will be able to edit the document to your needs and share it with your students. Measure out between 1 and 4 grams of copper sulfate hydrate that you have crushed into the crucible. If youve read this far, Im already grateful, but Id be even more so, if anyone could suggest where the difference between 5 and 5.18 is coming from. Measure the mass of the empty crucible using the balance. 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. Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride. This lesson presumes a basic understanding of how to name and write the formulas for binary ionic compounds. 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 anhydrous salt could have been exposed to air prior to measurement, and reabsorbed some moisture, thus disrupting measurements. The weight after cooling of the evap dish is constant. It should be brief (aim for ten words or less) and describe the main point of the experiment or investigation. 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. 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. (Full Name) which is stored for some time will have iron(III) sulphate Coloring pages - Water facts, how it helps the brain, how it helps the body, ideas on drinking more water. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from . Hydrates Lab Report introduction the purpose of this experiment was to explore and evaluate the bonding properties and characteristics of hydrates. Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). For Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions, describe what happened in each well. Kieran Sidebotham Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). 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. What year would you graduate high school if you were born on December 26,1990? PDF Experiment 1 Hydrates 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. First, a pre-weighed sample of the unknown sulfate salt will be dissolved in water. This was determined by recording the absorbance values of five solutions of Copper Sulfate and distilled water of different molarities. . Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. 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. Chemical Reaction Lab Report Send me a message, I'd love to hear from you! Which observations, experiences, or lesson materials helped you form your hypothesis? Two forms of this lab included for student differentiation. Heat the blue copper(II) sulfate until it has turned . Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. Record the appearance of the hydrate before it is heated. Embedded hyperlinks in a thesis or research paper. Includes teacher instructions, sample calculations, and a key to the conclusion questions. The difference between 5.00 and 5.16 is a weight error of about 200mg, and I was really careful, so this seems unlikely. Test tubes | | Chemical Changes VS Physical Changes Copper sulfate water of hydration lab and answer sheet and question Copper Sulfate Lab Report - 773 Words | Bartleby If a chemical reaction occurred, write a balanced equation for it. O. Try a color-by-number activity. The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. 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. CDC Health Standard 7, Naming Ionic and Covalent Compounds, Acids, and Hydrates, Acids, Bases and Hydrates Names and Formulas | Science Color By Numbers, Naming Compounds Bundle | Nomenclature | Science Color by Numbers, Chemistry Lab: Empirical Formula Hydrated Compound, PPT, WmUp, Ex Tic, Key, Lab, Chemistry Lab Bundle 1: 31 Labs, 17 Inquiry, Quiz, Key, PPT, PDF/Word, Copper (II) Sulfate Hydrate Lab - % composition, UNIT 9 - THE MOLE WORKSHEETS BUNDLE (#59-61), Chemistry Curriculum Full Year Guided Notes Bundle, Formula of Hydrate Lab - Data & Analysis GoogleSheet, Percent Composition, Empirical & Molecular Formulas, of Compounds & Hydrates, Chemistry Lab: Percent Water in a Hydrate. Use a minimum of 2 g. This will help to reduce errors due to small lab balance inaccuracies. Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. Molarity is calculated by diving the number of moles in the solute by the volume (in liters) of the complete solution. Delsea Chemistry - Hydrate Lab Percent error **hint set up the table with percent composition for water** Percent error = actual % experimental % X 100 = ____ % actual %. 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. Hydrate: A compound that contains the water molecule. This mass was taken before the substance was heated. In this experiment, the percentage by mass of sulfate in an unknown sulfate salt will be determined by gravimetric analysis. left exposed for any length of time. Other compounds can spontaneously absorb water from the surrounding atmosphere, they are said to be hygroscopic. I was born December18,1963When would I graduate high school? The purpose of this lab was to have real life experience with using observations to determine whether or not a chemical or physical change had occurred. Part B: Hygroscopic and Efflorescent Solids Anhydrate: The compound after the water molecule has been removed. Ive now heated the dish over a hot blue natural gas flame for ten minutes. 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. ; (NH4)2S. Little or no prior knowledge of finding empirical formula necessary. 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. Be sure that the flame will be close enough to the triangle to engulf the entire crucible. 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. Has the Melford Hall manuscript poem "Whoso terms love a fire" been attributed to any poetDonne, Roe, or other? Students chew bubble gum to remove sugar instead of removing water from a hydrate. Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. What did your group get as the formula of the hydrate? Return the evaporating dish with the hydrate to the wire gauze. 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. The goal of this experiment was to determine the product of copper (II) sulfate with iron. Then use that information to write the formula of the hydrate. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. ** Interested in my other Chemistry Resources?? completely anhydrous and will also absorb water from the air if A 'chemical' source of error is that the Great for Teachers:See if student data is on the right track with a few clicks or copy & paste.Check if calculations and conclusions made by students are right without needing manually doing the calculations.Provide s, This unit covers:1) Percentage Composition by Mass2) Finding Empirical Mass and Formulas3) Finding Molecular Mass and Formulas of Compounds4) Student Presentations Project, with rubric5) Finding Molecular Mass and Formulas of Hydrates6) Lab Activity: Determination of a Formula of a Hydrate7) Assessments and Check for Understandings8) Re-Teach PowerPoints, Over 15 practice problems on hydrate nomenclature, naming, and formula writing, complete with a full answer key.Goes Well With My Other Nomenclature Worksheets. * Iodine 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. 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. Data can be collected and most of it analyzed in a single 45-50 class period. The purpose of this bundle is to offer a worksheet to cover every type of naming.Goes Well With My Other Nomenclature Worksheets.NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? Is there any known 80-bit collision attack? What is wrong with reporter Susan Raff's arm on WFSB news? 1. 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. rev2023.5.1.43405. 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. : an American History (Eric Foner), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. 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