copper sulfate hydrate lab sources of error
3rd period A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. 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. > A C @ 6 bjbjWW 9n 5 5 r. 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. 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. Solutions: Nitric Acid (6M) * Phenolphthalein 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! Students will perform an experiment to find the hydrate formula. Concentrations are based on how much solute is in a solvent, and is reported by the units of molarity. This is appropriate for all levels of chemistry. 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 means, This lesson plan assists elementary students in understanding why it is important to drink plenty of water. 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. Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. Why do men's bikes have high bars where you can hit your testicles while women's bikes have the bar much lower? Use MathJax to format equations. 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? Wt after: 8.22g This error is almost completely determined by the error in $W_e$. So iron(II) sulphate Chemistry Naming & Formulas: Polyatomic Ions & Hydrates Guided Inquiry Lesson, Composition of a Hydrate Chemical Formula Lab, Naming & Writing Chemical Formulas: Acids & Hydrates |Distance Learning, Naming & Writing Chemical Formulas-LESSONS BUNDLE, Drink more water- hydrating, refreshing, natural. Students chew bubble gum to remove sugar instead of removing water from a hydrate. Period: 5 The goal of this experiment was to determine the product of copper (II) sulfate with iron. Data can be collected and most of it analyzed in a single 45-50 class period. $$\Delta X=\frac{\sqrt{(\Delta W_0)^2 W_e^2+(\Delta W_e)^2 W_0^2}}{W_e^2}\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{3}$$. The number you found for the water replaced the x in the formula CuSO4 xH2O. Paragraph #1: Purpose and a brief description of what you did. This mass was taken after the substance was heated. It is soluble. The purpose of the flame test lab was to further study the process of electron excitation. Explain. This was the same for all five trials. However, some spontaneously lose water upon standing in the atmosphere, they are said to be efflorescent. ALL of the Chemistry Labs you need for a WHOLE year!! 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. We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. 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 . Weigh the samples and record the masses as final masses. Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. 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. My background is a PhD in organic chemistry, so Im familiar with hazard assessment, and all the lab work I do with my student is something Ive done myself already. TPT empowers educators to teach at their best. * Milk October 3, 2017 The actual percent is ____. This is a great lab to introduce or reinforce percent composition and empirical formulas. After one hour, note any change in the physical appearance of each sample. Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride. Chemical Changes VS Physical Changes When hydrates are heated, the water is released from the compound as water vapor. Heating on the other hand would introduce heat change and thus a 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. It should be brief (aim for ten words or less) and describe the main point of the experiment or investigation. Period 3 Set the crucible with its cover slightly open on a clay triangle and heat strongly for at least 10 minutes. 2021-22, PDF Mark K Nclex Study Guide: Outline format for 2021 NCLEX exam. 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. When you have finished, submit this assignment to your teacher by the due date for full credit. Hydrates generally contain water in stoichiometric amounts; hydrates formulae are represented using the formula of the anhydrous (non-water) component of the complex followed by a dot then the water (\(\ce{H2O}\)) preceded by a number corresponding to the ratio of \(\ce{H2O}\) moles per mole of the anhydrous component present. Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. I give you teacher set up instructions, a key, and sample calculations. 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. First, a pre-weighed sample of the unknown sulfate salt will be dissolved in water. 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. Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. O. When heated gently, the red burgundy \(\ce{CoCl2*6H2O}\) will decomposes into the violet \(\ce{CoCl2*2H2O}\) then to the blue anhydrous \(\ce{CoCl2}\). Answer: Can copper-plating be reversed? Is it safe to publish research papers in cooperation with Russian academics? In this section you will observe the changes in the physical properties of compounds, including wetness, color, structure, texture and mass. Excellent layout. Grace Timler Measure the mass of the empty crucible using the balance. I havent investigated that yet, but I plan to weigh a sample before and after leaving in a warm airing cupboard overnight. Materials: * Cornstarch 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). What is wrong with reporter Susan Raff's arm on WFSB news? Purpose: To observe the difference between chemical and physical changes. You will be able to easily integrated it into your Learning Management System. Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. * Alka-Seltzer tablet Our first constant mass was 28.3208gand the average mass turned out to be 28.3222g. Also, to see the color of each reaction determining the amount of energy released using our color scale. Measure out between 1 and 4 grams of copper sulfate hydrate that you have crushed into the crucible. Which is very close to the actual error you find. Measured mass of crucible again: 36.1571g, Measured mass of (hydrous) copper sulfate: 2.1614g, Measured mass of crucible with (hydrous) copper sulfate: 38.3189g, Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. Introduction to Formulas (FREE) Lab Report This mass was taken before the substance was heated. You will find that most students will obtain the expected results pretty much dead on, and the students love the very low percent erro, Students get to discover the formula of a hydrate with real world experimental techniques in this lab! Heating maybe required to provide the required activation energy. Conclusion The mass percent of water in copper sulfate pentahydrate is _______. 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. Improving the copy in the close modal and post notices - 2023 edition, New blog post from our CEO Prashanth: Community is the future of AI. They are very math intensive, and very conceptual in nature. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. 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. $X$ is the desired answer. Lab Report 1 1. Lab Report Do you perhaps have any information about the nature of the .6% impurities in the original sample? For each of the chemical compounds below, place a. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. Use this tool to record your data and then watch all the necessary calculations and analysis completed in seconds!This resource accompanies the lab handout/procedure here. Happy teaching and have an, Students find the Empirical Formula of Epsom Salt. The mass was reduced to 7.58 g. What is the formula of the hydrate? (MgSO 4 XH 2 O). What does that x value tell you? 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. Lab written for Hotplate or Bunsen burner.Students: Observe water leaving compound as steam Heat to constant mass Calculate percent water Re-hydrate the anhydrous compoundLab Contains: Student Lab Sh, This lab is a great way for your students to investigate what a hydrate is and how its formula is determined. This lab will go in your lab book. 7. 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 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. To determine the mass of the water, subtract the anhydrate from the hydrate and put it in the proper space above. For a compound to be a true hydrate, it has to show all properties of true hydrates, including evolution of water upon heating, solubility of its anhydrous residue in water and reversibility in the color of the residue back to the color of the hydrate when dissolved in water. Student exploration Graphing Skills SE Key Gizmos Explore Learning. 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. Problem #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Percent error = |Actual - Theoreticall * 100 Theoretical 2. 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. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Your lab report must contain the following information: has a mass of 4.31 g before heating. copper (II) sulfate hydrate. Error results and analysi, The first procedure (Part 1) used heat to dehydrate the 4 hydrates and sucrose. 1. 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. MathJax reference. You did what I thought of doing but didn't get around to do. higher temperature change to the system. 2. Once dissolved, fill the rest of the volumetric . 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. Texas Chemistry Standards (TEKS) This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! 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. If a CHEM Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? Embedded hyperlinks in a thesis or research paper. In this lab, the five general types of chemical reactions were conducted and observations. B. Your name and the names of any lab partners. Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved. Use a minimum of 2 g. This will help to reduce errors due to small lab balance inaccuracies. (8 points) Try to avoid and popping or . Center the crucibles cover and let it cool down to room temperature. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. 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. Naming and Formulas: Simple Ionic and Covalent Compounds 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. which works out to: When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. This resource will come to you as a Google Doc. So if I look at the calculation process you have the following equation to get from known quantities to the answer: $$X=\left(\frac{W_0}{W_e}-1\right)\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{1}$$. 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. 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). 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! Weigh and record the mass of the cooled crucible with its cover and content (anhydrous residue). Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). Why purchase my version of this lab? When this anhydrous compound is dissolved in water it will go back to the original red burgundy color. Calculate the change in mass for each sample. Water is trapped in an ionic jail and can only escape using heat! Iron (III) chloride. Platform provided by Digication, Inc. 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. Using crucible tongs, clean a porcelain crucible and its cover using concentrated nitric acid (6 M). The number you found for the water replaced the x in the formula CuSO, The actual (true) value is 5, so the formula would be CuSO. Thanks for contributing an answer to Chemistry Stack Exchange! when does coordination become the distinctive task of management why? Building on previous knowledge of ions and formulas from Part One & Two are included in the Exit Ticket and the Homework. Materials: 3. The Homework includes all ionic compound possibilities: binary, ternary, multivalent cations, acids, and hydrates. Chemistry Experiment # _____ Percent of Water in Copper II Sulfate Pentahydrate Name_____ Section_____Date_____ Name(s) of Lab Partner(s) . Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). All metal sulphate are soluble in water, except barium (3 points) Label and place all samples at the same location in the room, well out of the way so they wont be spilled. Purpose and a brief description of what you did. (Qualitative Analysis). Pre-made digital activities. Wt before: 13.030.9836 = 12.82g hydrate Return the evaporating dish with the hydrate to the wire gauze. Rinse the crucible and its cover with distilled water. Another possibility would be to get more accurate equipment, to replicate the experiment within a dehumidified environment, and/or perform the experiment using a larger crucible (to reduce the possibility that spatter from the hydrated salt could leave the crucible). Abstract: Minutes in set-up time! This worksheet is a great follow-up to 42-Naming Hydrates. Honors Chemistry - You do not need to write three paragraphs for this conclusion. Which observations, experiences, or lesson materials helped you form your hypothesis? The weight after cooling of the evap dish is constant. The equation for the decomposition of copper (II) sulfate is CuSO4 (aq) ==> SO2(g) + CuO(s). * Salt I love this lab for several reasons. Experimental data may be collected with other students in introductory chemistry labs. Little or no prior knowledge of finding empirical formula necessary. However, I understand that sharing information required for a lab report or unknown submission (including but not limited to word processing or spreadsheet files, calculations, graphs, conclusions and additional problems at the end of the lab report) with other students is, evaporating dish, Bunsen burner, wood splint, test tubes, micro spatula, dropper, mortar and pestle, test tube holder, safety goggles, lab apron. Who makes the plaid blue coat Jesse stone wears in Sea Change? Your teacher's name. * Evaporating dish 1 A student is given a cobalt (II) chloride hydrate. Eventually, a linear equation that showed the relationship between absorbance and. Ammonium sulphide. 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. 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. 4 fun activities! Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. 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. 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. Water adheres to the dish when the dish is at room temperature. Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. -Pre soaked popsicle, Graded Assignment You should then decide if the compound is hygroscopic, efflorescent or neither using the change in the mass of the substance. Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. Introduction 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 Mathematics was used to explore wate, servation of mass and the reversibility properties in question. The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. Hydrate: A compound that contains the water molecule. Also, suggest some reasons why your number might be off from the true number. Record the appearance of the hydrate before it is heated. Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. Sulphate. Copper/Iron Stoichiometry Safety: Patel clip art, assessment, writing prompt, art activity, answer key, printables, no prep needed. At that time, the copper sulfate had turned a yellowish-white. If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? 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. Follow the directions below to complete the lab. +1. What can this chemical be? Write the chemical formula of the hydrated form of your unknown sample. On an analytical balance, weigh a pea-sized sample of each of the compounds below on separate clean and dry watch glasses. 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! I can also customize anything you', Looking for an engaging way for your students to review nomenclature for acids, bases and hydrates? (Full Name) There was no sign of $\ce{CuO}$ after the heating. anyhydrous salt, which forms one half of the experiment, may not be * Cup Use crucible tongs when cleaning the crucible with concentrated nitric acid. 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. Which are the best resorts for conference venues in Jim Corbett? Assumed water content: 42.6841.98 = 0.7g (!!!). * Matches |Score | Rounded to the nearest integer, the ratio is 1:5. 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. Remember the hydrate is in the crucible so you need to subtract the mass of the crucible to get the mass of just the hydrate. Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. Copper Sulfate's Water of Hydration Lab: Enrichment Activity. A chemical reaction is when substances (reactants) change into other substances (products). For this step, you are just changing your grams of water to moles using factor labeling. Minutes in set up time. Gently heat the hydrate by moving the burner back and forth around the dish. Then use that information to write the formula of the hydrate.
