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. The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. Do you perhaps have any information about the nature of the .6% impurities in the original sample? Ive now heated the dish over a hot blue natural gas flame for ten minutes. So if I look at the calculation process you have the following equation to get from known quantities to the answer: $$X=\left(\frac{W_0}{W_e}-1\right)\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{1}$$. * Phenolphthalein
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. Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. * Matches
The technique for this lab is based on actual geochemical analysis techniq. $0.08$ g. Now plugging in the numbers in Eq.$(3)$ I find $\Delta X=0.14$ mol water per mol copper sulphate. For $\Delta W_0$ I think it is safe to say that this is only the inaccuracy of the scale, so perhaps $0.01$ g. For $\Delta W_e$ I would go for the worst case scenario: that all of the 0.6% impurity in the original copper sulfate has evaporated, meaning that the weight will be off by 0.6% times $W_0$ i.e. * Copper II sulfate
No. (3 points) 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. Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. This mass was taken after the substance was heated. 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). 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. 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. 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. Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? Students chew bubble gum to remove sugar instead of removing water from a hydrate. Abstract:
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. The mass was reduced to 7.58 g. What is the formula of the hydrate? The title says what you did. Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. 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. So the practical involved taking hydrated copper sulphate, heating it to drive off the water, weighing before and after, and thus calculating the number of water molecules of crystallisation, based on the respective molecular weights of the anhydrous salt and water. 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. In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. October 3, 2017 * Iodine
The error you find falls within the worst-case expected error due to impurity and potentially adhered water. Write the chemical formula of the hydrated form of your unknown sample. When hydrates are heated, the water is released from the compound as water vapor. * Hot plate
2021-22, PDF Mark K Nclex Study Guide: Outline format for 2021 NCLEX exam. cup' method. 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. * Evaporating dish
Conclusion The mass percent of water in copper sulfate pentahydrate is _______. A chemical reaction is when substances (reactants) change into other substances (products). Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. Water adheres to the dish when the dish is at room temperature. 4 fun activities! Cross), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Psychology (David G. Myers; C. Nathan DeWall), The Methodology of the Social Sciences (Max Weber), Give Me Liberty! Return the evaporating dish with the hydrate to the wire gauze. Find out the importance of drinking plenty of water and the adverse health effects of not getting enough water. The lesson tutorial and the previous, reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. 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. 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. To learn more, see our tips on writing great answers. I havent investigated that yet, but I plan to weigh a sample before and after leaving in a warm airing cupboard overnight. 1. +1. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis.
* Water
Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. 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. Introduction to Formulas (FREE) Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. 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. Paragraph #1: Purpose and a brief description of what you did. When heated gently, the red burgundy \(\ce{CoCl2*6H2O}\) will decomposes into the violet \(\ce{CoCl2*2H2O}\) then to the blue anhydrous \(\ce{CoCl2}\). 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. To find the expected error in the answer, $\Delta X$, assuming no error in the molecular masses, we calculate: Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. 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. Did Billy Graham speak to Marilyn Monroe about Jesus? Purpose: This error is almost completely determined by the error in $W_e$. What did you learn? > A C @ 6 bjbjWW 9n 5 5 r. Purpose and a brief description of what you did. When you would go to mass the anhydrous salt, some of the mass would be missing as it would be in the air. This lesson presumes a basic understanding of how to name and write the formulas for binary ionic compounds. 10/3/12
Our first constant mass was 28.3208gand the average mass turned out to be 28.3222g. Through the use of a vacuum filtration system the mass of Cu was, Flame Test Lab Report 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. T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. 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. In this section you will try to determine through the testing of a series of compounds, which ones are true hydrates. We would call this copper sulfate pentahydrate. 5 H 2 O 6. * Alka-Seltzer tablet
The purpose was to see the electron excitation of each reaction and the color that it emitted. 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. At that time, the copper sulfate had turned a yellowish-white. 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. Ammonium sulphide. Use caution when heating the crucible and cover. 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. Common examples of minerals that exist as hydrates are gypsum (\(\ce{CaSO4*2H2O}\)), Borax (\(\ce{Na3B4O7*10H2O}\)) and Epsom salts (\(\ce{MgSO4*7H2O}\)). 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. with an unknown hydrate to determine the mass percent of water lost and solve for the formula and name of the unknown hydrate. 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! This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. 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. 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. This was determined by recording the absorbance values of five solutions of Copper Sulfate and distilled water of different molarities. Place the crucible, hydrated copper sulfate, and lid on/in your clay triangle. Hows your energy level around mid-morning?This health trio bundle will give you and your students the much-needed information as to why eating breakfast, hydrating with the right liquids and sleeping well are important parts of keeping your body and well-being healthy. 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. 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). Interpreting non-statistically significant results: Do we have "no evidence" or "insufficient evidence" to reject the null? We would call this copper sulfate pentahydrate. However, immediately after the first heating, It can be clearly seen that the heated copper sulfate has now transformed into a grainy and whitish-gray form. 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? Why purchase my version of this lab? By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. This lab will go in your lab book. For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. However, because the solutions were not mixed long and thoroughly enough, this made further deviations from what the data should have looked like. This is a great lab to introduce or reinforce percent composition and empirical formulas. Hence 0.267/0.0515 = 5.18mol water per mol copper sulphate. Finding the formula of hydrated copper(II) sulfate | Experiment | RSC Education In this experiment students will measure the mass of hydrated copper(II) sulfate before and after heating and use mole calculations to find the formula. completely anhydrous and will also absorb water from the air if So iron(II) sulphate What is wrong with reporter Susan Raff's arm on WFSB news? 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. Includes teacher instructions, sample calculations, and a key to the conclusion questions. NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? Solutions were made up of two parts, the solute and the solvent. To achieve this, a known mass of hydrated salt was heated, evaporating the water (essentially distillation). O. Send me a message, I'd love to hear from you! I love this lab for several reasons. Each worksheet has a full preview available. Answer the questions below. These errors made the absorbance values measured by the SpectroVis off from what it should have been. Did you heat the dish before weighing it to find the tare? Tina Jones Heent Interview Completed Shadow Health 1, Test Bank Varcarolis Essentials of Psychiatric Mental Health Nursing 3e 2017, 1-2 Module One Activity Project topic exploration, (Ybaez, Alcy B.) What is "water of hydration" and how does it affect me (you)? 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. 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. I give you teacher set up instructions, a key, and sample calculations. Measured mass of crucible with anhydrous copper sulfate: 37.3005g Mathematics was used to explore wate, servation of mass and the reversibility properties in question. X is a specific whole number value. { "01:_Using_Excel_for_Graphical_Analysis_of_Data_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
