Allow the crucible to cool down to room temperature (do not set the hot crucible on the bench top). 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. -Bunsen burner Coloring pages - Water facts, how it helps the brain, how it helps the body, ideas on drinking more water. When it is all white the water has been removed and the anhydrate is left. You should then decide if the compound is hygroscopic, efflorescent or neither using the change in the mass of the substance. Academic Chemistry - Three paragraph conclusion. -Pre soaked popsicle, Graded Assignment 2. 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. A student trying to determine if a white solid is a true hydrate heats the sample and finds that there is evolution of water, that the residue obtained is soluble in water and that the solution is colorless. When this color change appears to be complete, add 3 to 5 mL of water and observe the color of the dissolved substance. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Part B: Hygroscopic and Efflorescent Solids This lab will go in your lab book. Anhydrate: The compound after the water molecule has been removed. Then use that information to write the formula of the hydrate. Set the crucible with its cover slightly open on a clay triangle and heat strongly for at least 10 minutes. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of 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. 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! Learn more about Stack Overflow the company, and our products. 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! * Iodine The weight after cooling of the evap dish is constant. We would call this copper sulfate pentahydrate. 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. 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 Because the pipette was not exact, the amount of Copper Sulfate and distilled water that was put in the test tubes was not exact. 6. * Hot plate cup' method. 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. Explain. This mass was taken after the substance was heated. ** Interested in my other Chemistry Resources?? 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. Ferrous or iron(II) compounds can easily be oxidised to ferric 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. |Score | 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. (3 points) 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.) Will this likely lead to a higher or lower value of \(x\) than the actual value. This means, This lesson plan assists elementary students in understanding why it is important to drink plenty of water. 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. 3rd period or iron(III) compounds, when exposed to air. Measure out between 1 and 4 grams of copper sulfate hydrate that you have crushed into the crucible. You can check for this by looking for the telltale brown/black color of copper oxide. 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. In this lab, the five general types of chemical reactions were conducted and observations. Water is trapped in an ionic jail and can only escape using heat! 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. Your lab report must contain the following information: which is stored for some time will have iron(III) sulphate This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. 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. Your feedback is much appreciated and help me improve my resource materials to benefit you as an educator. Hydrates Lab Report Final - Chemistry Exp: Explore And Evaluate Bonding Heating maybe required to provide the required activation energy. For this step, you are just changing your grams of copper sulfate anhydrate (white powder) to moles using factor labeling. Distilled, Precipitation Reactions 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. Weigh the samples and record the masses as final masses. We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. 1. * Salt 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. This error is almost completely determined by the error in $W_e$. 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. Determining the Empirical Formula of a Hydrate Lab The results for the heating, Title: Title of lab/experiment. The water present in the latter case is called water of hydration or water of crystallization. What does that x value tell you? Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride. 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. A larger effect is decomposing copper sulfate to copper oxide and sulfur trioxide. 5: Properties of Hydrates (Experiment) - Chemistry LibreTexts 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. A. * Alka-Seltzer tablet The lab requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. AB1 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. Interpreting non-statistically significant results: Do we have "no evidence" or "insufficient evidence" to reject the null? To determine the mass of the water, subtract the anhydrate from the hydrate and put it in the proper space above. The name of this compound is "copper sulfate pentahydrate". Digication ePortfolio :: General Chemistry (Alexander Antonopoulos 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. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. The Composition of a Hydrate Lab - Teach Basic Percent Composition! 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 Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). Honors Chemistry - You do not need to write three paragraphs for this conclusion. ; (NH4)2S. 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. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water.