For this step, you are just changing your grams of water to moles using factor labeling. * Evaporating dish The best answers are voted up and rise to the top, Not the answer you're looking for? For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. : an American History (Eric Foner), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. 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The difference between 5.00 and 5.16 is a weight error of about 200mg, and I was really careful, so this seems unlikely. Copper sulfate and potassium iodide precipitate, EXAMPLE HYDRATECUPRIC SULFATE PENTAHYDRATE The coefficient of 5, Copper SourcesUses n Copper cookware n Copper pipes, Characterization of the Heparan Sulfate and Chondroitin Sulfate, Percent of Change Percent of Increase Percent of, Percent Composition What is Percent Composition The percent, Percent Proportion Equation Percent of Change Percent of, Empirical molecular percent composition Percent Composition Percent by, Percent Vpoet potu percent Vypotaj spamti koko percent. Also this lab was used as an opportunity to improve the ability to write lab reports and make data tables, and to provide experience with unfamiliar lab equipment. Paragraph #1: Purpose and a brief description of what you did. Score Interpreting non-statistically significant results: Do we have "no evidence" or "insufficient evidence" to reject the null? Who makes the plaid blue coat Jesse stone wears in Sea Change? But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. 2. $$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ Hypothesis (answer in a complete sentence in lab book). Making statements based on opinion; back them up with references or personal experience. Hydrated Copper (II) Sulphate Experiment Report This mass was taken before the substance was heated. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos Record the mass of the crucible, cover and sample. These compounds are not considered true hydrates as the hydration process is not reversible. Distilled, Precipitation Reactions This lesson also covers the benefits of daily exercise an, Naming and Formulas: Polyatomic Ion Compounds and Hydrates Lesson anyhydrous salt, which forms one half of the experiment, may not be 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. 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. 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. 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. Copyright 2023. In this section you will try to determine through the testing of a series of compounds, which ones are true hydrates. You should then decide if the compound is hygroscopic, efflorescent or neither using the change in the mass of the substance. 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? We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. For Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions, describe what happened in each well. Happy teaching and have an, Students find the Empirical Formula of Epsom Salt. If the correct formula of copper sulfate is CuSO4.5H20, determine your percent error. 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. 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! cup' method. . All rights reserved. -Bunsen burner Which observations, experiences, or lesson materials helped you form your hypothesis? Error results and analysi, The first procedure (Part 1) used heat to dehydrate the 4 hydrates and sucrose. What did your group get as the formula of the hydrate? Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. To subscribe to this RSS feed, copy and paste this URL into your RSS reader. When dissolved in water, the anhydrous compound will have a color similar to that of the original hydrate even if it had changed color going from the hydrate to the anhydrous compound. 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. Percent Composition of a Hydrate Lab - Chemistry Classes / Ronald 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? 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 Hydrate Lab. Chemical Changes VS Physical Changes copper (II) sulfate hydrate. Follow the directions below to complete the lab. 5,7% of error in a Hydrated Crystal lab, is it too high? Hydrate Teaching Resources | TPT A reversible reaction of hydrated copper(II) sulfate 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. Be sure that the flame will be close enough to the triangle to engulf the entire crucible. Do you perhaps have any information about the nature of the .6% impurities in the original sample? Students will perform an experiment to find the hydrate formula. - 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! Wt before: 13.030.9836 = 12.82g hydrate Some compounds like carbohydrates release water upon heating by decomposition of the compound rather than by loss of the water of hydration. Because this kind of reaction is usually not spontaneous. Use a minimum of 2 g. This will help to reduce errors due to small lab balance inaccuracies. The Homework includes all ionic compound possibilities: binary, ternary, multivalent cations, acids, and hydrates. Do Eric benet and Lisa bonet have a child together? dissolved is another. From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid (the formula of the anhydrous solid will be provided), the number of moles of water and moles of the anhydrous solid are calculated as shown below (\ref{4}, \ref{5}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. 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. By comparing the mass lost to the mass of anhydrous salt left behind, we can calculate the percentage of water within the hydrated salt. 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. 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. This is appropriate for all levels of chemistry. Problem #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Percent error **hint set up the table with percent composition for water** Percent error = actual % experimental % X 100 = ____ % actual %. The results for the heating, Title: Title of lab/experiment. Great for practice or assessment in your chemistry or physical science classroom. When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. TPT empowers educators to teach at their best. 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. However, because the solutions were not mixed long and thoroughly enough, this made further deviations from what the data should have looked like. Your teacher's name. The date the lab was performed or the date the report was submitted. Purposive Communication Module 2, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. Chemistry Experiment # _____ Percent of Water in Copper II Sulfate Pentahydrate Name_____ Section_____Date_____ Name(s) of Lab Partner(s) . This worksheet is a great follow-up to 42-Naming Hydrates. Record the mass and place the solute into a 50 mL volumetric flask. $X$ is the desired answer. Record the values as initial masses of containers and samples. Try a color-by-number activity. Did you heat the dish before weighing it to find the tare? In this experiment, the percentage by mass of sulfate in an unknown sulfate salt will be determined by gravimetric analysis. Data can be collected and most of it analyzed in a single 45-50 class period. A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. Platform provided by Digication, Inc. 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. If a CHEM Student exploration Graphing Skills SE Key Gizmos Explore Learning. My percent error is _____. 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. Has the Melford Hall manuscript poem "Whoso terms love a fire" been attributed to any poetDonne, Roe, or other? To determine the mass of the water, subtract the anhydrate from the hydrate and put it in the proper space above. The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. In this section we will demonstrate the dehydration and re-hydration of cobalt (II) chloride hexahydrate. left exposed for any length of time. Experiment_605_Hydrates_1_2_1 - Chemistry LibreTexts PDF Experiment 4 Hydrates and Anhydrous Salts In this section you will observe the changes in the physical properties of compounds, including wetness, color, structure, texture and mass. Three different versions! 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 At that time, the copper sulfate had turned a yellowish-white. 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. Hydrate: A compound that contains the water molecule. No. As such, there is always the possibility of inaccuracies with measurement, perception of measurement, inaccuracies of equipment, and other such errors. * Candle Gently heat the hydrate by moving the burner back and forth around the dish. Introduction to Formulas (FREE) 10/4/17 * Cup | | Add highlights, virtual manipulatives, and more. Minutes in set up time. How to force Unity Editor/TestRunner to run at full speed when in background? At that time, the copper sulfate had turned a yellowish-white. Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. Copper Sulfate's Water of Hydration Lab: Enrichment Activity. 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). Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. Lab Report Is Brooke shields related to willow shields? 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. Ms. Macielag's Thursday Lab Class (Honors), Building and Identifying All Organic Compounds, Lab Book: Setting Up Graphing Reference Sections, Naming and Writing Formulas (without Formula Mass). Explain what may have happened. Includes teacher instructions, sample calculations, and a key to the conclusion questions. which works out to: Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. 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. 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). Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field 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. Safety: Patel Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. 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. 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. Water adheres to the dish when the dish is at room temperature. (MgSO 4 XH 2 O). (Full Name) Percent error = |Actual - Theoreticall * 100 Theoretical 2. Lab Question: How can lichen indicate the quality of its environment? Water, the most common chemical on earth, can be found in the atmosphere as water vapor. Follow the directions below to complete the lab. The actual value of moles of water per copper sulfate is 5 moles and the percent composition of water in copper sulfate pentahydrate is 36.1% Variables: Independent Variable: Mass of crucible, cover and hydrated sample in grams Dependent Variable: Mass of water evolved in grams Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. \[ \underbrace{\ce{CuSO4*5H2O (s)}}_{\text{Deep Blue}} \ce{->[\Delta]} \underbrace{ \ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{+ 5 H2O (g)} \label{1}\], \[ \underbrace{\ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{->[\ce{H2O (l)} ]} \underbrace{ \ce{CuSO4 (aq)}}_{\text{Deep Blue}} \label{2}\]. I have a porcelain evaporating dish to contain the hydrate during heating, electronic scales that will weigh to 300g in increments of 10mg, and commercially bought copper sulphate that is allegedly 99.5% pure. 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). Weigh the samples and record the masses as final masses. Ive now heated the dish over a hot blue natural gas flame for ten minutes. So iron(II) sulphate The technique for this lab is based on actual geochemical analysis techniq. * Ammonium hydroxide 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. Then I re-weighed. ). The lab has an introduction to help students understand why they are doing 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. Your name and the names of any lab partners. 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. Skip to main content Skip to navigation Mast navigation Register Sign In Search our site All All Resources Articles A. This will result in the precipitation of . This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. 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}). The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. Purpose: 6. -Pre soaked popsicle, Graded Assignment Determining the Empirical Formula of a Hydrate Lab 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. 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. 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. Students chew bubble gum to remove sugar instead of removing water from a hydrate. with an unknown hydrate to determine the mass percent of water lost and solve for the formula and name of the unknown hydrate. 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