They are very math intensive, and very conceptual in nature. This document includes the pre-lab, procedure, data table, and analysis questions. Safety: When heating a substance in a test tube, be sure the open end of the test tube points away from yourself. Observations on structure, texture , wetness, etc. Explain. Solutions: Nitric Acid (6M) This means part of the copper (II) sulfate would be turned into a gas, sulfur dioxide. 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. The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. 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. Measured mass of crucible with anhydrous copper sulfate: 37.3005g. 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. If a chemical reaction occurred, write a balanced equation for it. Chemical Changes VS Physical Changes In the Hydrate lab at first, a sample of approximately 0.1000 grams of copper (II) sulfate pentahydrate was heated for the purpose to cause a chemical reaction that would remove all of the water molecules in order to determine the number of moles of water in the inorganic 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. ; (NH4)2S. Hydrated Copper (II) Sulphate Experiment Report Place the crucible on the triangle and ring stand over the bunsen burner and heat until it turns white. 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. You might also like these related lessons! ), Human error is always in effect, given that the laboratory does not function under ideal conditions. 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. Will this likely lead to a higher or lower value of \(x\) than the actual value? A chemical reaction is when substances (reactants) change into other substances (products). A reversible reaction of hydrated copper(II) sulfate Heating maybe required to provide the required activation energy. present. If a CHEM Have you ever wondered why you get a lot of headaches, your muscle doesnt function as well and your immune system is low? 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. 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). Introduction Piece of paper, NaCl (sodium chloride), water, 6 M HCL (hydrochloric acid), 0.1 M AgNO3 (silver nitrate), Mg ribbon, 6 M HCL (hydrochloric acid), CuSO4 5 H2O, 0.50g iron fillings, 0.50g of powdered sulfur, magnet, copper sulfate solution, zinc metal Do Eric benet and Lisa bonet have a child together? Weigh the crucible with its cover to the nearest 0.001 g. Making sure to handle the crucible and its cover with clean tongs, add about 1 g (weighed to the nearest 0.001 g) of the unknown hydrate. * Evaporating dish . Explain what may have happened. When you have completed the experiment, dissolve all your heated residues in water, put all your solids and liquids in the waste crock. 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. Water, the most common chemical on earth, can be found in the atmosphere as water vapor. Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). * Cup temperature change caused by the reaction is hard to measure. 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. * Iodine 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! ). \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\]. Who makes the plaid blue coat Jesse stone wears in Sea Change? This mass was taken after the substance was heated. ), During heating, some of the hydrous salt may have spattered, thus removing a portion of the hydrous salt from the crucible (A more likely source of error, considering that this would result in a greater difference between the two ratios, and percentages. You did what I thought of doing but didn't get around to do. The mass was reduced to 7.58 g. What is the formula of the hydrate? (3 points) Calculate your % error: "absolute value of . Students chew bubble gum to remove sugar instead of removing water from a hydrate. 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. Also, to see the color of each reaction determining the amount of energy released using our color scale. MathJax reference. The error you find falls within the worst-case expected error due to impurity and potentially adhered water. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. By clicking Post Your Answer, you agree to our terms of service, privacy policy and cookie policy. I havent investigated that yet, but I plan to weigh a sample before and after leaving in a warm airing cupboard overnight. How did it compare to the actual (it is given to you in step 3 of the calculations)? Paragraph #3: An error and how to fix it. 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. : an American History (Eric Foner), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Biological Science (Freeman Scott; Quillin Kim; Allison Lizabeth), The definition of a hydrate is a chemical that contai, ), hydrated ferrous sulfate, hydrated cobalt sulfate, sucrose, epson salt, 4 test tubes, test, Seidel's Guide to Physical examination (043), Educational Psychology and Development of Children Adolescents (D094), Language Arts Instruction and Intervention (C365), Health Assessment Of Individuals Across The Lifespan (NUR 3065L), Introduction To Project Management Software (CSBU539), PHIL ethics and social responsibility (PHIL 1404), Professional Application in Service Learning I (LDR-461), Advanced Anatomy & Physiology for Health Professions (NUR 4904), Principles Of Environmental Science (ENV 100), Operating Systems 2 (proctored course) (CS 3307), Comparative Programming Languages (CS 4402), Business Core Capstone: An Integrated Application (D083), A&p exam 3 - Study guide for exam 3, Dr. Cummings, Fall 2016, BMGT 364 Planning the SWOT Analysis of Silver Airways, Lesson 13 Paleoseismology Case Studies; Induced Seismicity, Skill Blood Admin - Active Learning Template, Philippine Politics and Governance W1 _ Grade 11/12 Modules SY. In this section you will observe the changes in the physical properties of compounds, including wetness, color, structure, texture and mass. higher temperature change to the system. 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. Place the crucible, hydrated copper sulfate, and lid on/in your clay triangle. The following steps are followed: Approximately 3g hydrated copper sulfate is weighed to the closest milligram. We tested the different reactions of each chemical compound that we used with the flame. Lab Report The Composition of a Hydrate Lab - Teach Basic Percent Composition! Assumed water content: 42.6841.98 = 0.7g (!!!). Source: Royal Society of Chemistry. Eventually, a linear equation that showed the relationship between absorbance and. Note the color of the dissolved residue. Rinse the crucible and its cover with distilled water. Why do men's bikes have high bars where you can hit your testicles while women's bikes have the bar much lower? 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. Once students have answered, they use the colo, Fully editable slide presentationHave you ever wondered why you get a lot of headaches, your muscle doesn't function as well and your immune system is low. 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}). Ive now heated the dish over a hot blue natural gas flame for ten minutes. Period 3 There are some possible sources of experimental error for this lab Lab Report ), Not all of the water may have evaporated during heating (Also unlikely, for the same reason as the one above. Why don't we use the 7805 for car phone chargers? Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. This lesson also covers the benefits of daily exercise an, Naming and Formulas: Polyatomic Ion Compounds and Hydrates Lesson We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. What does that x value tell you? The results for the heating, Title: Title of lab/experiment. 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. Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). The experiment was about creating solutions of standard molarity and measuring concentrations. Ignited Bunsen Burner, and heated crucible for 12 minutes. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis. However, this lab allows them to apply what they've learned about percent composition, hydrates, and empirical formulas in a real world example! Is there any known 80-bit collision attack? I love this lab for several reasons. 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. 3. It is soluble. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. 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. So thats 4.81/18 = 0.267mol water, and . Chem 1A 04 Lab 3 Hydrate Report - Studocu * Milk Empirical Formula of a Hydrate Chemistry Lab. 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! 10/3/12 This is probably a small effect. Determining the Empirical Formula of a Hydrate Lab As such, there is always the possibility of inaccuracies with measurement, perception of measurement, inaccuracies of equipment, and other such errors. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Write the chemical formula of the hydrated form of your unknown sample. Adding EV Charger (100A) in secondary panel (100A) fed off main (200A). Introduction to Formulas (FREE) Hence 0.267/0.0515 = 5.18mol water per mol copper sulphate. This resource will come to you as a Google Doc. 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. The best answers are voted up and rise to the top, Not the answer you're looking for? Try to avoid and popping or . 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. Hydrate Lab By heating a known mass of hydrated salt, evaporating the water (essentially distillation), and then comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. Then use that information to write the formula of the hydrate. October 3, 2017 Molarity is calculated by diving the number of moles in the solute by the volume (in liters) of the complete solution. 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. Hydrated copper sulphate is blue in color while anhydrous copper sulphate is white in color.CuSO4 is white, the pentahydrate crystal (CuSO4.5H2O) and the aquous solution (Cu2+ (aq) ions) are. Be sure to subtract out the crucible before putting it into the proper space above. 10/4/17 What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six? Answer: Can copper-plating be reversed? Purpose and a brief description of what you did. Sulphate, Calcium Sulphate, Barium Sulphate and also Silver No. To learn more, see our tips on writing great answers. Percent of Water in Copper Ii Sulfate Pentahydrate So iron(II) sulphate 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. Lab 2: Determine the Percentage of Water in a Hydrate: The goal of this experiment is to learn how to properly calculate the ratio of salt to water, in a hydrated salt, and to calculate the percentage of water (by mass) within a hydrated salt. After one hour, note any change in the physical appearance of each sample. Try a color-by-number activity. Error results and analysi, The first procedure (Part 1) used heat to dehydrate the 4 hydrates and sucrose. These compounds are not considered true hydrates as the hydration process is not reversible. I give you teacher set up instructions, a key, and sample calculations. Which is very close to the actual error you find. Your values correspond to a #38.169%# water percent composition for copper(II) sulfate pentahydrate. 1 A student is given a cobalt (II) chloride hydrate. Set the crucible with its cover slightly open on a clay triangle and heat strongly for at least 10 minutes. Using crucible tongs, clean a porcelain crucible and its cover using concentrated nitric acid (6 M). Pre-made digital activities. 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. $X$ is the desired answer. Heat the blue copper(II) sulfate until it has turned . When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. Ferrous or iron(II) compounds can easily be oxidised to ferric Answer the questions below. Download the preview file to get a look! (MgSO 4 XH 2 O). Honors Chemistry - You do not need to write three paragraphs for this conclusion. The iron oxidation state was, Copper-Iron Stoichiometry Note: This is an editable animated PowerPoint. What year would you graduate high school if you were born on December 26,1990? Copper Sulfate Pentahydrate Lab Report | ipl.org In this section we will determine the number of moles of water present per mole of anhydrous solid in a given hydrate. * Phenolphthalein Materials: It is generally possible to remove the water of hydration by heating the hydrate. has a mass of 4.31 g before heating. I was born December18,1963When would I graduate high school? 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. 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. So if I look at the calculation process you have the following equation to get from known quantities to the answer: $$X=\left(\frac{W_0}{W_e}-1\right)\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{1}$$. February 29, 2016 Hypothesis (answer in a complete sentence in lab book). Distilled, Precipitation Reactions When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. Also, suggest some reasons why your number might be off from the true number. I can also customize anything you', Looking for an engaging way for your students to review nomenclature for acids, bases and hydrates? Minutes in set up time. Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. Academic Chemistry - Three paragraph conclusion. $$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ This was determined by recording the absorbance values of five solutions of Copper Sulfate and distilled water of different molarities. (However, this is not likely to be the sole cause of the inaccuracies within this experiment, though it may contribute to it. Great for practice or assessment in your chemistry or physical science classroom. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. anyhydrous salt, which forms one half of the experiment, may not be 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). Im teaching chemistry to a home-ed 15 year old. Use this picture to get the mass of the anhydrate (white powder). * Candle Conclusion The mass percent of water in copper sulfate pentahydrate is _______. 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. 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. This is a great lab to introduce or reinforce percent composition and empirical formulas. For Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions, describe what happened in each well. Little or no prior knowledge of finding empirical formula necessary. Lab Report Weigh the samples and record the masses as final masses. 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! which works out to: 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. I give . 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. The purpose of this lab is to determine the relationship between moles of copper sulfate and moles of water in a hydrate. Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. The residue obtained after heating, called the anhydrous compound, will have a different structure and texture and may have a different color than the hydrate. Heating on the other hand would introduce heat change and thus a