7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. Your name and the names of any lab partners. 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. Heat the content of the crucible with its cover slightly open to allow the water of hydration to escape, first gently (about 10 minutes), then strongly (about 5 minutes). ALL of the Chemistry Labs you need for a WHOLE year!! Source: Royal Society of Chemistry. Send me a message, I'd love to hear from you! Answer: * Salt Students chew bubble gum to remove sugar instead of removing water from a hydrate. 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%. I give you teacher set up instructions, a key, and sample calculations. Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. Rinse the crucible and its cover with distilled water. This lesson presumes a basic understanding of how to name and write the formulas for binary ionic compounds. 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. Quizzes with auto-grading, and real-time student data. completely anhydrous and will also absorb water from the air if A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Lab Report Sulphate. So assuming that 26 degrees is not warm enough to cause partial loss of water of crystallisation, that suggests that at best my hydrate is only 98.36% pure, not 99.5 as it says on the bottle (typo corrected above). Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. Or the hydrate, as supplied, could be a little wet. Other hygroscopic substances, such as solid \(\ce{NaOH}\), absorb so much water from the atmosphere that they dissolve in this water, these substances are said to be deliquescent. clip art, assessment, writing prompt, art activity, answer key, printables, no prep needed. Center the crucibles cover and let it cool down to room temperature. Chemical Reaction Lab Report 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. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. 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. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Eventually, a linear equation that showed the relationship between absorbance and. $$\Delta X=\frac{\sqrt{(\Delta W_0)^2 W_e^2+(\Delta W_e)^2 W_0^2}}{W_e^2}\left(\frac{M_{CuSO_4}}{M_{H_2O}}\right) \tag{3}$$. Iron (III) chloride. Solutions were made up of two parts, the solute and the solvent. - CLICK HERE **--------------------------------------------If you like what you see, check out the rest of my store and be sure, This hydrate lab activity is perfect for chemistry teachers without a lab room! Materials: 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. The date the lab was performed or the date the report was submitted. You will be able to easily integrated it into your Learning Management System. Follow the directions below to complete the lab. 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. Note from Mr. Cook: Use the virtual lab and watch the video I put on the homepage! (Full Name) Observations on structure, texture , wetness, etc. The purpose of the flame test lab was to further study the process of electron excitation. Sulphate, Calcium Sulphate, Barium Sulphate and also Silver * Cornstarch My percent error is _____. 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. Problem #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Why do men's bikes have high bars where you can hit your testicles while women's bikes have the bar much lower? The name of this compound is "copper sulfate pentahydrate". Naming and Formulas: Simple Ionic and Covalent Compounds (3 points) 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. What can this chemical be? The error you find falls within the worst-case expected error due to impurity and potentially adhered water. In this lab, the five general types of chemical reactions were conducted and observations. * Water the main. Lab 1: Determining the Empirical Formula of a Compound, Lab 2: Determine the Percentage of Water in a Hydrate, Lab 16: Gravimetric Determination of a Precipitate, Lab 14a: Separation and Analysis of Cations, Lab 18: Separation by Liquid Chromatography, Lab 6a: Standardizing a Solution of Sodium Hydroxide, Lab 33: Determination of Calcium Carbonate Content of and Anti-Acid Pill, Lab 28: Molecular Interaction in Ethanol and Acetone, Obtained crucible and lid (henceforth, the two are considered to be together unless mentioned otherwise), inspected them, and measured their mass: 36.1574g, Obtained equipment, set up ring stand, Bunsen Burner, clay triangle, and mesh pad. What is wrong with reporter Susan Raff's arm on WFSB news? What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six? Abstract: This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. Heated crucible with hydrated copper sulfate for 3 minutes, before increasing heat, and heating it for 5 more minutes. This means, This lesson plan assists elementary students in understanding why it is important to drink plenty of water. Is this a true hydrate? If a CHEM 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. Some compounds may possess some of the properties of hydrates without being true hydrates. Pending marking your answer as accepted, my grateful thanks in the meantime for your detailed analysis. Note the color of the dissolved residue. In this section you will observe the changes in the physical properties of compounds, including wetness, color, structure, texture and mass. Percent error **hint set up the table with percent composition for water** Percent error = actual % experimental % X 100 = ____ % actual %. 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. 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. 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. \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\]. 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. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. sulphate, calcium sulphate and lead sulphate. A minor scale definition: am I missing something? Find out the importance of drinking plenty of water and the adverse health effects of not getting enough water. * Hot plate 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. 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. Heat for 5 minutes using a single-cone blue flame. 4 fun activities! Measure out between 1 and 4 grams of copper sulfate hydrate that you have crushed into the crucible. 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. 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). A chemical reaction is when substances (reactants) change into other substances (products). Happy teaching and have an, Students find the Empirical Formula of Epsom Salt. Chemical Changes VS Physical Changes 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. 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. 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? 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. $$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ This worksheet is a great follow-up to 42-Naming Hydrates. Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). Where's my experimental error coming from? A 'chemical' source of error is that the Also as I was calculating the empirical formula, I wasn't quite sure the figures were correct so I might have miscalculated. 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 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. Your lab report must contain the following information: Abstract Record the exact mass of the dish with the hydrate to the nearest 0.01 gram. Weigh and record the mass of the cooled crucible with its cover and content (anhydrous residue). Ammonium sulphide. You will be able to edit the document to your needs and share it with your students. This compound is not dissolved in water, the water is part of the formula and is a solid. Purpose: 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. Have you ever wondered why you get a lot of headaches, your muscle doesnt function as well and your immune system is low? The purpose of this bundle is to offer a worksheet to cover every type of naming.Goes Well With My Other Nomenclature Worksheets.NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? Chemistry Honors When hydrates are heated, the water is released from the compound as water vapor. Some chemicals, when exposed to water in the atmosphere, will reversibly either adsorb it onto their surface or include it in their structure forming a complex in which water generally bonds with the cation in ionic substances. 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. The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. 8.22/(63.5+32+64) = 0.0515mol anhydrous copper sulphate. 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. The goal of this experiment was to determine the product of copper (II) sulfate with iron. Did Billy Graham speak to Marilyn Monroe about Jesus? 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 Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. 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. Academic Chemistry - Three paragraph conclusion. The anhydrous salt could have been exposed to air prior to measurement, and reabsorbed some moisture, thus disrupting measurements. Second, the results are great! 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? We tested the different reactions of each chemical compound that we used with the flame. ** Interested in my other Chemistry Resources?? A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. Calculate the change in mass for each sample. Three different versions! Instead, as seen calibration results, more of each was used. Write the chemical formula of the hydrated form of your unknown sample. Minutes in set up time. Hypothesis (answer in a complete sentence in lab book). This was the same for all five trials. I give . Materials: Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. Do Eric benet and Lisa bonet have a child together? 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. rev2023.5.1.43405. This resource will come to you as a Google Doc. Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. 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. The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. Hydrate Lab. In this section you will try to determine through the testing of a series of compounds, which ones are true hydrates. T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. What is "water of hydration" and how does it affect me (you)? 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. Ferrous or iron(II) compounds can easily be oxidised to ferric Label and place all samples at the same location in the room, well out of the way so they wont be spilled. Pre-made digital activities. Pour the used nitric acid in the waste container provided. 3. Explain. Hydrate: A compound that contains the water molecule. Hypothesis: If dyed lichen is exposed to certain chemicals, than color will color the solution. The water is present in a definite and consistent ratio. I love this lab for several reasons. Record the mass and place the solute into a 50 mL volumetric flask. * Watch glass Procedure Weigh out approximately 5g of copper sulfate pentahydrate. How did it compare to the actual (it is given to you in step 3 of the calculations)? Coloring pages - Water facts, how it helps the brain, how it helps the body, ideas on drinking more water. Copper sulphate ; CuSO4.5H2O (NB The 5H2O is the water of hydration held in the crystal ; like you hold a tennis ball in your hand). Using crucible tongs, clean a porcelain crucible and its cover using concentrated nitric acid (6 M). The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. A. 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. Be sure to subtract out the crucible before putting it into the proper space above. This lab will go in your lab book. When you would go to mass the anhydrous salt, some of the mass would be missing as it would be in the air. Some compounds like carbohydrates release water upon heating by decomposition of the compound rather than by loss of the water of hydration. 1 A student is given a cobalt (II) chloride hydrate. So now the final thing left to do is estimate how big $\Delta W_0$ and $\Delta W_e$ are. Lab Report 1 Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. 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). 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. Skip to main content Skip to navigation Mast navigation Register Sign In Search our site All All Resources Articles Students will perform an experiment to find the hydrate formula. What did your group get as the formula of the hydrate? ; (NH4)2S. * Iodine If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? * Milk 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. The weight after cooling of the evap dish is constant. When you have finished, submit this assignment to your teacher by the due date for full credit. Purpose and a brief description of what you did. Bunsen Burner or Hot PlateComplete Lesson: PPT, Warm-up, Exit Ticket, Lab PaperStudents: drive off water of hydration calculate percent water use percent water and given elemental percentages to find formulaLab Contains: Student Lab Sheet Student Lab Make-up Sheet for Absent Students Student Lab Sheet with Answers in Italics Lab Quiz - Use as exit ticket, next day warm-up or quiz Lab Qui, This is a great lab to introduce or reinforce percent composition and empirical formulas. Distilled, Precipitation Reactions Firstly to clarify a chemical change is defined as a change resulting. |Score | 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.