The data obtained from the lab is here: Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. 1.1 THE NATURE OF SUBSTANCES AND CHEMICAL REACTIONS (p) how to calculate the formula of a compound from reacting mass data; WJEC Combined science. Explain. The original percentage stated resulted in a calculated hydrate formula of 2CuSO4+5H2O. PROCEDURE: When copper (II) sulfate hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as copper (II) sulfate. 4. Then the percentage composition will be determined by weighing the mass of the white crystals. Answer key Problem #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. Abstract: The Purpose of this lab was to find the chemical formula for ZnSO 4 through determining the amount of anhydrate and hydrate. Determining the Chemical Formula of a Hydrate. My lab partner and I measured and did all that good stuff. An example would be CaSO 4. The mass of the white crystals, when cooled was recorded. Solution: 1) Determine mass of water driven off: 15.67 minus 7.58 = 8.09 g of water 2) Determine moles of MgCO3 and water: Stirring the compound was essential to making sure all the blue crystals were heated. 2.545 g of hydrate is heated and 63.85% of the residue is found after heating. The beginning weight (uh mass?) The actual hydrate formula for the copper (II) sulfate compound was CuSO4+5H2O. mass of water in hydrate = 4.24 - 3.62 = 0.62, % water = 100% * mass H2O/mass hydrate = 100% * 0.62 g / 4.24 g = 14.6%, The last two hydrates from above have lots of water so lets try the calcium sulfate, mass of hydrate = Ca + S +4 O + 2 H2O = 40.0 + 32.1 + 4x16.0 + 36.0 = 172, % water = 100% x 36.0 g / 172 g = 20.9 % (strike 1), % water = 100% x 36.0 g/ 244 g = 14.8% (home run if we allow for a little experimental error). (Synthesis path should be mentioned in full details.)? Suppose that you heated a sample of a hydrated ionic compound in a test tube. Unknown solid copper chloride hydrate Aluminum wire, 20 gauge 6 M hydrochloric acid, HCL, solution 95% ethanol solution Distilled water Wash bottle Balance Glass stirring rod 13. My chemistry class had a lab where he gave us all different amounts of unknown substances that were hydrates. 3. of this hydrate is “magnesium sulfate heptahydrate”. Water of hydration MgSO 4 • 7H 2 O. Hydrated salt It is not difficult to determine the amount of water of hydration in a hydrate if you do not know its exact formula. Get your answers by asking now. Join Yahoo Answers and get 100 points today. The experiment compound was safely disposed of and the materials that were used were properly put away. Chemistry equilibrium constant expression? Sanus. Join Yahoo Answers and get 100 points today. In our experiment we did see this happen but it would be more evident in a test. Carousel Previous Carousel Next. A hydrate is a compound that is chemically combined with water molecules. Experimental Question: How can we experimentally determine the formula of an unknown hydrate, A? We did this in my science class last year in high school. 1. 1. Explain your answer. CuSO4= 100 - 31.49 H2O Class Average= 34.4%. What might you expect to see inside, near the mouth of the test tube? i had chemistry two years ago and all that knowledge is gone now.. hopefully someone will tell you the answers. Give the empirical formula of each of the following compounds if a sample contains the following quantities of each element.? PURPOSE: To determine the percentage of water in a hydrate. 4.) You obtained the mass percent of water in the copper sulfate hydrate. Aktualności; Usługi; Specjaliści; Galeria; Kontakt; Diety; formula of a hydrate lab answers Determining the Chemical Formula of a hydrate, please help!? : In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. When the solution is heated the hydrate will convert to an anhydrous ionic compound. Still have questions? Determining the Chemical Formula of a Hydrate. As the first step, use the percent composition to derive the compound™s empirical formula. Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. When a hydrate is heated the water molecules are driven off as steam, leaving behind the water-free anhydrate. b.) A community website for the residents of Upware in Cambridgeshire, UK. The percent H30 in the hydrated salt is 180.159 *100%-62.959%H20 180.159+105.989 In this experiment, you will determine the mass percent of water present in the hydrate of copper (II) sulfate and then you will determine the chemical formula of the hydrate. Virtual Lab Hydrate.docx. What two things make up hydrates? In the case of a hydrate, and assuming you know the formula of the associated anhydrous ionic compound, do you think it is more useful to have the mass perventage composition? a.) 3H 2 O. Hay, attendance sometimes leads to understanding. Table salt has the chemical formula NaCl. 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). Measure the mass of the crucible and lid with the hydrate in it. Measure the mass of the crucible and lid, without the hydrate in it. 2. 65.6g (1 mol/ 159.6086) Therefore the Molecular Formula is CuSO4 x 5H2O. An eye-opening lesson, Amanda Kloots surprised at the hate over vaccination, Here's what's next in the Trump taxes investigation, How Texas's electrical grid nearly collapsed, Biden laments 'truly grim' COVID-19 milestone, Taco Bell jumps into the chicken sandwich wars, McCain stands by Fauci criticism: 'I'm not a phony', These popular rain boots are 40% off at Nordstrom, 'Bachelor' star breaks silence on Chris Harrison scandal, Mariners CEO resigns after 'inappropriate' comments. Kimberly Graziano & Hyunjae Kim. Unit 2: Chemistry 1. When the solution is heated the hydrate will convert to an anhydrous ionic compound. a) Determine the value of x in the formula of the compound b) Science. An anhydrate is the substance that remains after the water is removed from a hydrate. To determine the formula of a hydrate experimentally, we must calculate the mole: mole ratio of the water portion compared to the anhydrate portion. About 4g of hydrated Copper (II) Sulfate was added to the beaker and the weight was recorded. By measuring the compound before heating and after, the amount of water in the original hydrate can be determined and the formula discovered. 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}). HERE ARE THE QUESTIONS THAT I AM VERY CONFUSSED WITH, your help is much appericiated: 1. Lab #5 Determining Chemical Formula of a Hydrate Zeeshan Saleem Nikki Pandey Brandt Farazian Hoang Phan 6/15/2015 Chem 1411.S2L. This chemical would be called calcium sulfate trihydrate. The mass was reduced to 7.58 g. What is the formula of the hydrate? 3. Lab Report: Determining Chemical Formula of Hydrate Results: Measurement Data Hydrate salt used Copper sulfatex hydrate Mass of hydrate sample 2.09 grams Mass of anhydrate in sample 1.3 grams Mass of water in sample 0.7 grams Experimental formula of hydrate Chemical Equation for Dehydration Reaction Conducted: Calculations: (neatly show all calculations, including all units; for more space use back of paper) Mass water: Mass percent water in hydrate… 2. A hydrate is an inorganic salt that has water molecules bonded to it. 4. Remove the filter paper with the copper from the funnel and leave it to dry. For … Menu and widgets 5. b.) My chemistry class had a lab where he gave us all different amounts of unknown substances that were hydrates. This experiment was done in order to find the percentage composition of a hydrate compound. Using your obervations, calculate the percentage composition of the copper sulfate hydrate. Therefore, the chemical formula is CuSO 4 5H 2 O. For example, Glucose is C6H12O6; it’s empirical formula is CH2O. An eye-opening lesson, 'Harry Potter' star admits he's embarrassed by early work. Still have questions? Woah! Mass of Beaker + Hydrated Copper(II) Sulfate 81.531g, Mass of CuSO4 x H2O Mass of H2O= 18.0152g Mass of CuSO4= 159.6068g, 1(15.9994) Mass of Hydrated CuSO4= 3.757g Mass of Anhydrous= 2.574g, 1a.) : ), sorry..... i would love to help you but i have no clue what all this means. An anhydrate is the substance that remains after the water from a hydrate has been removed through heating. 3.757 Difference 1.183 / 3.757 x 100% = 31.49%. for number three the amount of water will decrease of course 4. a) beaker not dry b) hydrate stuck on apparatus. I have no idea how to find the percentage of water, the empirical formula, or even what I have seeings as I have a crappy teacher and I was absent the day he taught this. The purpose of this experiment is to determine the empirical formula of a hydrate. You simply heat a small sample of hydrate to evaporate the water, and then compare the moles Explain how this would affect the calculated percent by mass of water in the compound and the molecular formula you determined. The formula of the anhydride is provided and based on the moles of the hydrate present before heating and the moles of the water lost upon heating, the empirical formula of the hydrate can be determined. These compounds often come in the form of a crystal which can then be heated in order to remove the water in the form of steam. tube because it is more confined than the beaker. Upware Residents Association. How many moles of sugar was added to 82.90 g of ethanol to change the freezing point of ethanol by 2.750 c. The mass of a beaker and stirring rod was found. In the chemical formula NaCl, there is a 1:1 ratio of sodium ions:chloride ions. The choice are (BUT ARE NOT LIMITED TO...) CaSO4*2H20, CoCl2*6H20, MgSO4*7H2O. My lab partner and I measured and did all that good stuff. Kimberly Graziano & Hyunjae Kim. Pre-Lab Questions: 1. Perhaps instead of giving us your ENTIRE homework, ask specifically which bits you are not understanding.. it's supposed to let you see the heat of the elements, all the different colors for all the different temperatures. The mass of the empty beaker, beaker + hydrated Copper (II) Sulfate, and mass of the beaker + anhydrous Copper (II) Sulfate was found through this procedure. The exercises below will provide additional practice in determining the chemical formula of a hydrate based on experimental data. Lab –Formula of a Hydrate - Help with calculations Magnesium sulfate (MgSO 4) is a molecule that loves to hold on to water (hydrophilic). What's something you just don't understand? Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. The beaker was placed on a hot plate, heated until the blue crystals lost there blue color. 14. Complete the folowing and submit your answers as a word document in Canvas. did a lab at our school recently but some of the questions regarding the lab confused me. Suggest a source of error (not already mentioned) that would result in a value of x that is. Sample Calculation An empty crucible has a mass of 12.770 grams. 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