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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? AB1 This is appropriate for all levels of chemistry. rev2023.5.1.43405. Error results and analysi, The first procedure (Part 1) used heat to dehydrate the 4 hydrates and sucrose. 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. cup' method. When you would go to mass the anhydrous salt, some of the mass would be missing as it would be in the air. The actual percent is ____. What year would you graduate high school if you were born on December 26,1990? Who makes the plaid blue coat Jesse stone wears in Sea Change? 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. Use caution when heating the crucible and cover. Heating maybe required to provide the required activation energy. Save the residue and perform your calculations. Sulphate. As a result the actual 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. Has the Melford Hall manuscript poem "Whoso terms love a fire" been attributed to any poetDonne, Roe, or other? Add highlights, virtual manipulatives, and more. the main. Purpose: To observe the difference between chemical and physical changes. Introduction: 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. Do you have pictures of Gracie Thompson from the movie Gracie's choice. If the results of your calculations suggest that you have some water left in the residue, reheat your sample for an additional 5 minutes, allow it to cool down and weigh it again. To find the expected error in the answer, $\Delta X$, assuming no error in the molecular masses, we calculate: 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
When you have completed the experiment, dissolve all your heated residues in water, put all your solids and liquids in the waste crock. 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! For this step, you are just changing your grams of water to moles using factor labeling. B. Did Billy Graham speak to Marilyn Monroe about Jesus? 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). Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? This is written CuSO4 . Is Brooke shields related to willow shields? Added deionized water to the anhydrous copper sulfate, at which point it became hydrated again, and returned to its original blue coloration. 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. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. Empirical Formula of a Hydrate Chemistry Lab. Step 1: Find the moles of the Copper Sulfate anhydrate (white powder). What will be the effect, on the mass of the residue, of not heating the hydrate enough to drive off all the water of hydration in the hydrate. (8 points)
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. Write the goal of the lab or the question you tried to answer. The iron oxidation state was, Copper-Iron Stoichiometry
Find out the importance of drinking plenty of water and the adverse health effects of not getting enough water. Purpose and a brief description of what you did. > A C @ 6 bjbjWW 9n 5 5 r. Heat for 5 minutes using a single-cone blue flame. Lab Question: How can lichen indicate the quality of its environment? 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. Hydrate Lab. 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). Lab Report Removed crucible from burner, placed on mesh pad, and allowed to return to room temperature. The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. Will this likely lead to a higher or lower value of \(x\) than the actual value. The introduction to this lab introduces students to h. Eat, Sleep, Exercise & Hydrate: The Importance of Taking Care of Yourself! A hot crucible looks like a cold one, avoid direct contact with the crucible, clay triangle and ring stand until you are sure they are cooled. 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). 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. Includes teacher instructions, sample calculations, and a key to the conclusion questions. How many moles of water (x) do you think are in this hydrate? What does that x value tell you? Measured mass of crucible with anhydrous copper sulfate: 37.3005g . 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. Platform provided by Digication, Inc. Follow the directions below to complete the lab. Record the mass of the crucible, cover and sample. Building on previous knowledge of ions and formulas from Part One & Two are included in the Exit Ticket and the Homework. No. Observations on structure, texture , wetness, etc. This error is almost completely determined by the error in $W_e$. The mass was reduced to 7.58 g. What is the formula of the hydrate? Procedure Weigh out approximately 5g of copper sulfate pentahydrate. has a mass of 4.31 g before heating. Lab Report
This worksheet is a great follow-up to 42-Naming Hydrates. The purpose was to see the electron excitation of each reaction and the color that it emitted. 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. sulphate, calcium sulphate and lead sulphate. 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. 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. Abstract Hydrated copper sulfate (CuSO 4), hydrated ferrous sulfate, hydrated cobalt sulfate, sucrose, epson salt, 4 test tubes, . Any anhydrous compound from a hydrate generally has the following properties: Most hydrates are stable at room temperature. Paragraph #1: Purpose and a brief description of what you did. October 3, 2017 7H2O) Ratio (water to anhydrate): 7 to 1 3.) I weighed out some of the hydrate into another dry dish, flattened it out as much as possible within the confines of the dish to expose as much surface area as possible, and left it in the airing cupboard for 24h at 26 degrees Celsius. If the null hypothesis is never really true, is there a point to using a statistical test without a priori power analysis? Examine your moles of anhydrate and moles of water that you just calculated, divide each by the smaller mole amount. Is there any known 80-bit collision attack? (MgSO 4 XH 2 O). 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. What are the qualities of an accurate map? Instead you are to complete the three problems below in your lab book using what you learned from the lab. Molarity is calculated by diving the number of moles in the solute by the volume (in liters) of the complete solution. What is wrong with reporter Susan Raff's arm on WFSB news? Introduction - Hydrated Ionic Compounds, commonly called, "hydrates". The actual (true) value is 5, so the formula would be CuSO4 5H2O. (Unlikely, considering that the ratios between the two, both stoichiometric and percent water content, would be smaller in such an instance. At that time, the copper sulfate had turned a yellowish-white. Ignited Bunsen Burner, and heated crucible for 12 minutes. Next, an excess of aqueous barium chloride is added to the aqueous solution of the unknown salt. This lab will go in your lab book. If a chemical reaction occurred, write a balanced equation for it. This lab explored hydrates and the 4 objectives in a three procedure process through observation, experimentation, and mathematical methods to help prove whether dehydration of a hydrate is, Equipment and materials used in one or more procedure included: Hydrated copper sulfate, observation and experimentation. 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. 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. Measure the mass of the empty crucible using the balance. Use this picture to get the mass of the hydrate (blue powder). Skip to main content Skip to navigation Mast navigation Register Sign In Search our site All All Resources Articles T, Concepts:This worksheet teaches students how to determine the number of water molecules in a hydrate. A. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. You can check for this by looking for the telltale brown/black color of copper oxide. 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! What should I follow, if two altimeters show different altitudes? Academic Chemistry - Three paragraph conclusion. Heating will shift the equation of dehydration below to the right since it is an endothermic reaction. How to force Unity Editor/TestRunner to run at full speed when in background? 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 Asking for help, clarification, or responding to other answers. I give you teacher set up instructions, a key, and sample calculations. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. 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). The title says what you did. Distilled, Precipitation Reactions 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. Be sure to subtract out the crucible before putting it into the proper space above.
Safety: Patel A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six? 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? 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. Set up the apparatus as shown (but without water in the receiving tube - this is to be collected during the experiment), placing about 5 g of powdered hydrated copper(II) sulfate in the test tube. Make sure that the tube is clamped near the bung as shown. * Hot plate
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. * Salt
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. The lab has an introduction to help students understand why they are doing the lab. anyhydrous salt, which forms one half of the experiment, may not be Water adheres to the dish when the dish is at room temperature. What is "water of hydration" and how does it affect me (you)? How did it compare to the actual (it is given to you in step 3 of the calculations)? This means part of the copper (II) sulfate would be turned into a gas, sulfur dioxide. 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. 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. 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. Great for practice or assessment in your chemistry or physical science classroom. Weigh and record the mass of the cooled crucible with its cover and content (anhydrous residue). . The best answers are voted up and rise to the top, Not the answer you're looking for? However, immediately after the first heating, It can be clearly seen that the heated copper sulfate has now transformed into a grainy and whitish-gray form. When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. completely anhydrous and will also absorb water from the air if 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. Or the hydrate, as supplied, could be a little wet. The equation for the decomposition of copper (II) sulfate is CuSO4 (aq) ==> SO2(g) + CuO(s). How did it compare to the actual (it is given to you in step 3 of the calculations)? 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. NomenclaturePossible Uses- Worksheet- Activity- Homework- Classwork- Test Review- Quiz ReviewFeedbackHave questions or feedback? Accessibility StatementFor more information contact us atinfo@libretexts.org. 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. Will this likely lead to a higher or lower value of \(x\) than the actual value? Why don't we use the 7805 for car phone chargers? Hypothesis: If dyed lichen is exposed to certain chemicals, than color will color the solution. Chemicals: Copper (II) sulfate hydrateStudents will experimentally determine the percent composition of water in the copper (II) sulfate hydrate. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. $$\Delta X=\sqrt{\left(\frac{\partial X}{\partial W_0}\Delta W_0\right)^2+\left(\frac{\partial X}{\partial W_e}\Delta W_e\right)^2} \tag{2}$$ Tina Jones Heent Interview Completed Shadow Health 1, Test Bank Varcarolis Essentials of Psychiatric Mental Health Nursing 3e 2017, 1-2 Module One Activity Project topic exploration, (Ybaez, Alcy B.) Disposed of salt within the proper receptacle, cleaned crucible, and returned all equipment to its point of origin. We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. 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. Instead, as seen calibration results, more of each was used. * Milk
Also, suggest some reasons why your number might be off from the true number. 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? 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 1. To achieve this, a known mass of hydrated salt was heated, evaporating the water (essentially distillation). 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. when does coordination become the distinctive task of management why? Do Eric benet and Lisa bonet have a child together? The reason why this is a source of error is because as time passed between the measurements, the copper sulfate hydrate sample absorbed humidity (water) from the atmosphere and therefore increased its mass. Through this the appropriate reaction had to be determined out of the two possibilities. The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. Little or no prior knowledge of finding empirical formula necessary. Through the use of a vacuum filtration system the mass of Cu was, Flame Test Lab Report At that time, the copper sulfate had turned a yellowish-white. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. This was the same for all five trials. 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. \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\]. If youve read this far, Im already grateful, but Id be even more so, if anyone could suggest where the difference between 5 and 5.18 is coming from. Part B: Hygroscopic and Efflorescent Solids -Pre soaked popsicle, Graded Assignment Use crucible tongs when cleaning the crucible with concentrated nitric acid. 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}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. You might also like these related lessons! Firstly to clarify a chemical change is defined as a change resulting. Materials:
Some compounds may possess some of the properties of hydrates without being true hydrates. Pour the used nitric acid in the waste container provided. \[ \underbrace{\ce{CuSO4*5H2O (s)}}_{\text{Deep Blue}} \ce{->[\Delta]} \underbrace{ \ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{+ 5 H2O (g)} \label{1}\], \[ \underbrace{\ce{CuSO4 (s)}}_{\text{Ashy White}} \ce{->[\ce{H2O (l)} ]} \underbrace{ \ce{CuSO4 (aq)}}_{\text{Deep Blue}} \label{2}\]. 7. | |
Send me a message, I'd love to hear from you! Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. 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%. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. The purpose of the flame test lab was to further study the process of electron excitation. Follow the directions below to complete the lab. * Paper towel
Any time she touches the apparatus its under close supervision by myself. Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). - 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! (Qualitative Analysis). Hypothesis (answer in a complete sentence in lab book). So thats 4.81/18 = 0.267mol water, and * Water
Excellent layout. 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. ** Interested in my other Chemistry Resources?? Procedure A. Qualitative Determination of the Released Liquid after Heating CuSO 4.5H 2 O 1. Use MathJax to format equations. Thanks for contributing an answer to Chemistry Stack Exchange! This was determined by recording the absorbance values of five solutions of Copper Sulfate and distilled water of different molarities. 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. Period: 5 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. This lab will go in your lab book. { "01:_Using_Excel_for_Graphical_Analysis_of_Data_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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\newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 6: Types of Chemical Reactions (Experiment), Formula of a Hydrate (\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)), Part A: Reversibility of hydration (optional, by Instructor), Part B: Hygroscopic and Efflorescent Solids, Part D: Determination of the formula of a hydrate, Pre-laboratory Assignment: Properties of Hydrates, Part A: Reversibility of Hydration (Optional), Identification of hydrates in a group of compounds, Investigation of the properties of hydrates, Determination of the number moles of water of hydration in a hydrate.