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. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. All rights reserved. Sulphate, Calcium Sulphate, Barium Sulphate and also Silver Which observations, experiences, or lesson materials helped you form your hypothesis? How many moles of water (x) do you think are in this hydrate? The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate.
Download Free PDF View PDF Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. 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. 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). 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 weight after cooling of the evap dish is constant. 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water of hydration in a hydrate. Then use that information to write the formula of the hydrate. Ferrous or iron(II) compounds can easily be oxidised to ferric * Salt
Stack Exchange network consists of 181 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. Heat the blue copper(II) sulfate until it has turned . Through this the appropriate reaction had to be determined out of the two possibilities. This worksheet is a great follow-up to 42-Naming Hydrates. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. . This compound is not dissolved in water, the water is part of the formula and is a solid. has a mass of 4.31 g before heating. 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. Legal. Source: Royal Society of Chemistry. Introduction However, because the solutions were not mixed long and thoroughly enough, this made further deviations from what the data should have looked like. Heat for 5 minutes using a single-cone blue flame.
The lab has an introduction to help students understand why they are doing the lab. Heat the test tube and note any condensation that may appear at the mouth of the test tube as evidence of dehydration, note the color of the residue. Grace Timler * Hot plate
Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). Do you perhaps have any information about the nature of the .6% impurities in the original sample? If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? Some compounds like carbohydrates release water upon heating by decomposition of the compound rather than by loss of the water of hydration. Lab Report
Any time she touches the apparatus its under close supervision by myself. 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 * Matches
Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. completely anhydrous and will also absorb water from the air if 2. Lab Report
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. All metal sulphate are soluble in water, except barium 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. What does that x value tell you? 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? These compounds are not considered true hydrates as the hydration process is not reversible. Delsea Chemistry - Hydrate Lab Chemical Changes VS Physical Changes
$$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ In an evaporating dish, gently heat a small amount (0.3 - 0.5 g) of CoCl 2 6H 2O crystals until its color changes to violet then to blue. 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. Other compounds can spontaneously absorb water from the surrounding atmosphere, they are said to be hygroscopic. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis. The goal of this experiment was to determine the product of copper (II) sulfate with iron. This resource will come to you as a Google Doc. 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. The solvent was the dissolving substance and the solute was the substance being dissolved. Try a color-by-number activity. (Full Name)
A reversible reaction of hydrated copper(II) sulfate Firstly to clarify a chemical change is defined as a change resulting. Concepts covered include:Definition of a hydrateHow the chemical formulas of hydrates are written Nomenclature of hydratesHow to determine the formula of a hydrate with examleUses of hydrates, Students find the percent water, calculate percent error and using simple steps of 1-4 find empirical formula for copper(II) sulfate crystals. What should I follow, if two altimeters show different altitudes? 2. What did your group get as the formula of the hydrate? -Bunsen burner 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. Concentrations are based on how much solute is in a solvent, and is reported by the units of molarity. Write the goal of the lab or the question you tried to answer. Test tubes Label and place all samples at the same location in the room, well out of the way so they wont be spilled. Weigh the samples and record the masses as final masses.
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. ), Not all of the water may have evaporated during heating (Also unlikely, for the same reason as the one above. 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. 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. 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. At that time, the copper sulfate had turned a yellowish-white. 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. 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. Use a minimum of 2 g. This will help to reduce errors due to small lab balance inaccuracies. The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid. Our first constant mass was 28.3208gand the average mass turned out to be 28.3222g. Solids: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride, Sodium sulfate hydrate, Iron (III) chloride, Potassium aluminum sulfate, Calcium chloride, Copper sulfate, Unknown. Hydrate Lab Updated sections include a new hydrate toolbox, updated correlations and computer methods. However, this lab allows them to apply what they've learned about percent composition, hydrates, and empirical formulas in a real world example! 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%. Copper/Iron Stoichiometry Water, the most common chemical on earth, can be found in the atmosphere as water vapor. If a CHEM * Evaporating dish
The difference between 5.00 and 5.16 is a weight error of about 200mg, and I was really careful, so this seems unlikely. Your lab report must contain the following information: Lab Report
Chemistry Honors Data can be collected and most of it analyzed in a single 45-50 class period. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. sulphate, calcium sulphate and lead sulphate. When you would go to mass the anhydrous salt, some of the mass would be missing as it would be in the air. Solved Post-Lab Questions 1. If the correct formula of - Chegg 10/4/17 The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. No. 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. It is soluble. or iron(III) compounds, when exposed to air. So now the final thing left to do is estimate how big $\Delta W_0$ and $\Delta W_e$ are. Naming and Formulas: Simple Ionic and Covalent Compounds There was no sign of $\ce{CuO}$ after the heating. We would call this copper sulfate pentahydrate. In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. 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 purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Water is trapped in an ionic jail and can only escape using heat! Send me a message, I'd love to hear from you! Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. 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. The results for the heating, Title: Title of lab/experiment. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The date the lab was performed or the date the report was submitted. Platform provided by Digication, Inc. Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). Set the crucible with its cover slightly open on a clay triangle and heat strongly for at least 10 minutes. 1. rev2023.5.1.43405. 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. Great for practice or assessment in your chemistry or physical science classroom. Excellent layout. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Minutes in set-up time! The salt is magnesium sulfate - MgSO 4 and, the same as Copper sulfate, it exists as a hydrate, but in this case we will find the amount of water surrounding the compound. Building on previous knowledge of ions and formulas from Part One & Two are included in the Exit Ticket and the Homework. Accessibility StatementFor more information contact us atinfo@libretexts.org. The purpose of the flame test lab was to further study the process of electron excitation. You might also like these related lessons! higher temperature change to the system. This mass was taken before the substance was heated. MathJax reference. . They are very math intensive, and very conceptual in nature. 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.
. Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. 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. ). present. There are some possible sources of experimental error for this lab What does that x value tell you? Why do men's bikes have high bars where you can hit your testicles while women's bikes have the bar much lower? Note: This is an editable animated PowerPoint. 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! Disposed of salt within the proper receptacle, cleaned crucible, and returned all equipment to its point of origin. Name: Kamaal Thomas |Date: January 4, 2011 | |Graded Assignment
Use MathJax to format equations. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. Use this picture to get the mass of the hydrate (blue powder). The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate . Introduction: At that time, the copper sulfate had turned a yellowish-white. Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. 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. Wt after: 8.22g Follow the directions below to complete the lab. 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. I love this lab for several reasons. Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. Added deionized water to the anhydrous copper sulfate, at which point it became hydrated again, and returned to its original blue coloration. 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. B. Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. Im teaching chemistry to a home-ed 15 year old. cup' method. The Homework includes all ionic compound possibilities: binary, ternary, multivalent cations, acids, and hydrates. Paragraph #2: What did you learn? Try to avoid and popping or . Set up the apparatus as shown (but without water in the receiving tube - this is to be collected during the experiment), placing about 5 g of powdered hydrated copper(II) sulfate in the test tube. 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). 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. Determining the Empirical Formula of a Hydrate Lab 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. Some compounds may possess some of the properties of hydrates without being true hydrates. What's even better is that you get credit from TpT every time you leave a constructive comment. Cool (approximately 10 minutes) and get the mass of the anhydrate (white compound). X is a specific whole number value. Record the mass of the crucible, cover and sample. I give . Materials: The best answers are voted up and rise to the top, Not the answer you're looking for? Answer: * Cornstarch
What did you learn? The iron oxidation state was, Copper-Iron Stoichiometry
Weigh out approximately 3 grams of copper(II) sulfate pentahydrate into a clean, dry large ignition tube (25 x 200 mm). (3 points) Did Billy Graham speak to Marilyn Monroe about Jesus? Be sure to subtract out the crucible before putting it into the proper space above. heat loss to the surroundings if you using the simple 'insulated Be sure to subtract out the crucible before putting it into the proper space above. This is a great lab to introduce or reinforce percent composition and empirical formulas. Purpose and a brief description of what you did. Asking for help, clarification, or responding to other answers. The actual percent is ____. You can check for this by looking for the telltale brown/black color of copper oxide. 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. 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 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.
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