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. Record the appearance of the hydrate before it is heated. The electronic scales (quite cheap) were an obvious first candidate for a source of error. 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. Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. Period 3 Write the chemical formula of the hydrated form of your unknown sample. Follow the directions below to complete the lab. * 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. 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. . 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. Hydrates Lab Report Final - Chemistry Exp: Explore And Evaluate Bonding Ammonium sulphide. For this step, you are just changing your grams of water to moles using factor labeling. Do you perhaps have any information about the nature of the .6% impurities in the original sample? Hydrate Lab 4 fun activities! 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. Did you heat the dish before weighing it to find the tare? The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. Use MathJax to format equations. Name: Kamaal Thomas |Date: January 4, 2011 | |Graded Assignment Test tubes Little or no prior knowledge of finding empirical formula necessary. Percent Composition of a Hydrate Lab - Chemistry Classes / Ronald NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. 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. Materials: We would call this copper sulfate pentahydrate. 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. Added deionized water to the anhydrous copper sulfate, at which point it became hydrated again, and returned to its original blue coloration. -Pre soaked popsicle, Graded Assignment You will be able to edit the document to your needs and share it with your students. Which is very close to the actual error you find. The anhydrous salt could have been exposed to air prior to measurement, and reabsorbed some moisture, thus disrupting measurements. 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. Record the mass and place the solute into a 50 mL volumetric flask. At that time, the copper sulfate had turned a yellowish-white. It only takes a minute to sign up. In this experiment, the percentage by mass of sulfate in an unknown sulfate salt will be determined by gravimetric analysis. 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. 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. Why did DOS-based Windows require HIMEM.SYS to boot? anyhydrous salt, which forms one half of the experiment, may not be Iron (III) chloride. This resource will come to you as a Google Doc. We tested the different reactions of each chemical compound that we used with the flame. What does that x value tell you? The copper sulfate is dissolved in 100ml of water that is distilled and contained in . You will be able to easily integrated it into your Learning Management System. T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. 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! Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. Through this the appropriate reaction had to be determined out of the two possibilities. When you would go to mass the anhydrous salt, some of the mass would be missing as it would be in the air. Water is trapped in an ionic jail and can only escape using heat! 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. Making statements based on opinion; back them up with references or personal experience. What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six? Be sure that the flame will be close enough to the triangle to engulf the entire crucible. Return the evaporating dish with the hydrate to the wire gauze. 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. If the correct formula of copper sulfate is CuSO4.5H20, determine your percent error. This is a student-centered, active learning lesson without lecture or notetaking! 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. It is soluble. I give . Does a password policy with a restriction of repeated characters increase security? Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. 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. left exposed for any length of time. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis. 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. For sulphate salts, all are soluble except Lead Introduction to Formulas (FREE) Why purchase my version of this lab? 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. Center the crucibles cover and let it cool down to room temperature. Label and place all samples at the same location in the room, well out of the way so they wont be spilled. 5,7% of error in a Hydrated Crystal lab, is it too high? How to apply a texture to a bezier curve? To achieve this, a known mass of hydrated salt was heated, evaporating the water (essentially distillation). For each of the chemical compounds below, place a. Copper Sulfate Lab Report - 773 Words | Bartleby Interpreting non-statistically significant results: Do we have "no evidence" or "insufficient evidence" to reject the null? Score * Evaporating dish In this lab students will heat a hydrate and from their collected data, calculate their percent error, and calculate the number of moles water in the hydrategiving them the final formula for the hydrate. clip art, assessment, writing prompt, art activity, answer key, printables, no prep needed. Question: Name Formula of Hydrates Lab Report Data and Calculations: Copper (II) sulfate hydrate Trial 1 Trial 2 19.244 20.546 24.504 27.689 Mass of crucible and cover (6) Mass of crucible, cover, sample before heating is) Mass crucible, cover, sample after heating (8) Mass of hydrate() 22.606 25.111 Mass of anhydrous solide Mass of water driven off (e) Moles of water Period: 5 Minutes in set-up time! completely anhydrous and will also absorb water from the air if 1. The goal of this experiment was to determine the product of copper (II) sulfate with iron. Chemical Reaction Lab Report This means part of the copper (II) sulfate would be turned into a gas, sulfur dioxide. ; (NH4)2S. It contains a brief introduction to hydrates and then describes the series of calculations that are done to determine the ratio of the moles of water to anhydrate salt. 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. 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.
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