Join Yahoo Answers and get 100 points today. Abstract: The Purpose of this lab was to find the chemical formula for ZnSO 4 through determining the amount of anhydrate and hydrate. Hay, attendance sometimes leads to understanding. Still have questions? 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). Observing our nitrate, it has a white crystalline structure, representing that … The mass of a beaker and stirring rod was found. This is because when you’re heating a hydrated ionic compound you are removing the water. Explain how this would affect the calculated percent by mass of water in the compound. Still have questions? and the molecular formula you determined. You will need to answer these and add them to your lab report. Measure the mass of the crucible and lid, without the hydrate in it. Measure the mass of the crucible and lid with the hydrate in it. 14. 2. The data obtained from the lab is here: Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. 3H 2 O. About 4g of hydrated Copper (II) Sulfate was added to the beaker and the weight was recorded. formula units and molecules. I assume you unknown was a white crystalline solid. The experiment compound was safely disposed of and the materials that were used were properly put away. For example, Glucose is C6H12O6; it’s empirical formula is CH2O. Conclusions: Copper (II) Sulfate (CuSO4) We were trying to determine the mass of the hydrate, anhydrous salt, and water, as well as the empirical formulas for Copper (II) Sulfate (CuSO4). One point is earned for the correct answer. Does the temperature you boil water in a kettle in affect taste? Aktualności; Usługi; Specjaliści; Galeria; Kontakt; Diety; formula of a hydrate lab answers Remove the crucible from the fire and allow it … How many moles of sugar was added to 82.90 g of ethanol to change the freezing point of ethanol by 2.750 c. Suggest a source of error (not already mentioned) that would result in a value of x that is. 5. \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\] An eye-opening lesson, 'Harry Potter' star admits he's embarrassed by early work. What is more dangerous, biohazard or radioactivity? Therefore, the chemical formula is CuSO 4 5H 2 O. Examine this data and complete the calculations below: Mass of … (Synthesis path should be mentioned in full details.)? Unit 1: CHEMICAL SUBSTANCES, REACTIONS and ESSENTIAL RESOURCES. Synthesize the following compounds from the listed materials. Chemistry equilibrium constant expression. 4.) 1. ... using experimental mass values to calculate percent composition is a highly effective manner of determining the chemical formula of hydrates and other compounds. You simply heat a small sample of hydrate to evaporate the water, and then compare the moles My chemistry class had a lab where he gave us all different amounts of unknown substances that were hydrates. A hydrate is a chemical that has water molecules loosely bonded to it. Suppose that you did not compelely convert the hydrate to the anhydrous compound. Hydrates are compounds that contain water with a definite mass in the form of H_2O in their molecular formula. Does the temperature you boil water in a kettle in affect taste? 3. Upware Residents Association. Give the empirical formula of each of the following compounds if a sample contains the following quantities of each element.? It is expected that the mass percent of water should be similar in all the groups, Group Mass(CuSO4 x H2O) Mass(CuSO4) % H2O, 3.) Hydrates are copper (II) sulfate and copper (II) nitrate. So rubbing two sticks together to make fire... even breadsticks? Pre-Lab Questions: 1. Lab #5 Determining Chemical Formula of a Hydrate Zeeshan Saleem Nikki Pandey Brandt Farazian Hoang Phan 6/15/2015 Chem 1411.S2L. b.) Lab –Formula of a Hydrate - Help with calculations Magnesium sulfate (MgSO 4) is a molecule that loves to hold on to water (hydrophilic). Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. i had chemistry two years ago and all that knowledge is gone now.. hopefully someone will tell you the answers. Stirring the compound was essential to making sure all the blue crystals were heated. This experiment was done in order to find the percentage composition of a hydrate compound. Measure 2-3 grams of CuSO4 hydrate. How do I decide whether to use a Heck or Suzuki reaction? Kimberly Graziano & Hyunjae Kim. 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. Get your answers by asking now. For example, sodium and chlorine combine to form sodium chloride, NaCl. A hydrate is an inorganic salt that has water molecules bonded to it. Please help as sooon as possible! We did this in my science class last year in high school. However, not all compounds form in a 4. The beginning weight (uh mass?) : 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. If that was barium chloride take care! Menu and widgets 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. 2.545 g of hydrate is heated and 63.85% of the residue is found after heating. ), 4. ? In order to determine the percent composition and the empirical formula of a hydrate, you must know how much water is in the hydrate. 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… 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. 1. 2. 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. A hydrate is a compound that is chemically combined with water molecules. 3.757 Differenceï 1.183 / 3.757 x 100% = 31.49%. 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: 65.6g (1 mol/ 159.6086) Therefore the Molecular Formula is CuSO4 x 5H2O. : ), sorry..... i would love to help you but i have no clue what all this means. When the solution is heated the hydrate will convert to an anhydrous ionic compound. 3. 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. of the substance was 4.24 g and after we heated it a few times the ending mass was 3.62 g. Now I have to figure out what I have. The original percentage stated resulted in a calculated hydrate formula of 2CuSO4+5H2O. Unit 2: Chemistry 1. What two things make up hydrates? Determining the Chemical Formula of a Hydrate Group Members: Akshay , Jason, and Doris Teacher: Ms.Misiri By : Ravinna Raveenthiran Course Code: SCH3U Due Date: May 2 2016 Chemistry Lab Purpose: The purpose of this experiment is to determine the chemical formula for the hydrate … Example: CuSO4 x 5H2O has 5 water … Complete the folowing and submit your answers as a word document in Canvas. My lab partner and I measured and did all that good stuff. Trumpâs taxes arenât the only records exposed, Do you know your privilege? 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. Remove the filter paper with the copper from the funnel and leave it to dry. What might you expect to see inside, near the mouth of the test tube? Kimberly Graziano & Hyunjae Kim. 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. Virtual Lab Hydrate.docx. (I understand that it would change, but exactuly how? When the solution is heated the hydrate will convert to an anhydrous ionic compound. Sorry if I didn't help, I tried. What are the treatments of pleural effusion? By measuring the compound before heating and after, the amount of water in the original hydrate can be determined and the formula discovered. The water molecules are not actually part of the formula, so the formula is written slightly differently. a.) Experimental Question: How can we experimentally determine the formula of an unknown hydrate, A? An anhydrate is the substance that remains after the water from a hydrate has been removed through heating. What is more dangerous, biohazard or radioactivity? Woah! CuSO4= 100 - 31.49 H2O Class Average= 34.4%. 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}). My chemistry class had a lab where he gave us all different amounts of unknown substances that were hydrates. Sanus. When it has dried 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. a) Determine the value of x in the formula of the compound b) Science. So rubbing two sticks together to make fire... even breadsticks? Table sugar has the chemical formula C12H22O11. Why is (H2O2) known as hydrogen peroxide and not hydrogen dioxide? 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. 1. Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. 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). Determining the Chemical Formula of a Hydrate. Then answer the following questions. The purpose of this experiment is to determine the empirical formula of a hydrate. 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.) Heat the hydrate in the crucible with the lid partially on. My lab partner and I measured and did all that good stuff. Suppose that you heated a sample of a hydrated ionic compound in a test tube. The mass was reduced to 7.58 g. What is the formula of the hydrate? Suppose the hydrate heated too quickly and some of it spatted out of the container and was lost. An anhydrate is the substance that remains after the water is removed from a hydrate. An example would be CaSO 4. This chemical would be called calcium sulfate trihydrate. In the chemical formula NaCl, there is a 1:1 ratio of sodium ions:chloride ions. The exercises below will provide additional practice in determining the chemical formula of a hydrate based on experimental data. You would most likely see water vapour droplets. As the first step, use the percent composition to derive the compound™s empirical formula. The mass of the white crystals, when cooled was recorded. Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. What's something you just don't understand? PURPOSE: To determine the percentage of water in a hydrate. 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. The actual hydrate formula for the copper (II) sulfate compound was CuSO4+5H2O. 4. Chemistry equilibrium constant expression? When a hydrate is heated the water molecules are driven off as steam, leaving behind the water-free anhydrate. 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. Chemical Formula Detective: Determining the empirical formula of a hydrate Background Different elements can form chemical bonds to create compounds. Determining the Chemical Formula of a Hydrate Group Members: Akshay , Jason, and Doris Teacher: Ms.Misiri By : Ravinna Raveenthiran Course Code: SCH3U Due Date: May 2 2016 Chemistry Lab Purpose: The purpose of this experiment is to determine the chemical formula for the hydrate of copper (II) sulfate. Using your obervations, calculate the percentage composition of the copper sulfate hydrate. In our experiment we did see this happen but it would be more evident in a test. Determining the Chemical Formula of a hydrate, please help!? A community website for the residents of Upware in Cambridgeshire, UK. HERE ARE THE QUESTIONS THAT I AM VERY CONFUSSED WITH, your help is much appericiated: 1. of this hydrate is “magnesium sulfate heptahydrate”. When the crystals lost their color the heat source was removed and the beaker was left to cool. Explain how this would affect the calculated percent by mass of water in the compound and the molecular formula you determined. Carousel Previous Carousel Next. 2. It is so long I can't tell exactly what you mean. You obtained the mass percent of water in the copper sulfate hydrate Documents Similar To Determining the Chemical Formula of a Hydrate. 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 hydrate of copper (II) sulfate with formula CuSO4.xH2O has a molar mass of 250.0 g/mol. The beaker was placed on a hot plate, heated until the blue crystals lost there blue color. Explain your answer. The choice are (BUT ARE NOT LIMITED TO...) CaSO4*2H20, CoCl2*6H20, MgSO4*7H2O. You obtained the mass percent of water in the copper sulfate hydrate. Table salt has the chemical formula NaCl. Get your answers by asking now. Join Yahoo Answers and get 100 points today. Wife of drug kingpin El Chapo arrested in Virginia, Pat Sajak called out for mocking contestant, Woman’s license mistakenly features her in a face mask, Top volleyball duo boycott country over bikini ban, 'Bachelor' hopeful suffers horrifying skydiving accident, Raiders player arrested in Texas street-racing incident, Jobless workers may face a surprise tax bill, Actress confirms engagement to NFL star Aaron Rodgers, Trump’s taxes aren’t the only records exposed, Do you know your privilege? Explain. 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. 2.1 THE NATURE OF SUBSTANCES AND CHEMICAL REACTIONS (p) how to calculate the formula … For … Determining the Chemical Formula of a Hydrate. What's something you just don't understand? In addition, the mass 11) Clean up. Sample Calculation An empty crucible has a mass of 12.770 grams. If you were to heat the hydrated ionic compound in a test tube you would expect to, see steam rising which means that the water in the compound is being evaporated into, the air. b.) tube because it is more confined than the beaker. Then the percentage composition will be determined by weighing the mass of the white crystals. Why is (H2O2) known as hydrogen peroxide and not hydrogen dioxide? From the data collected the number of molecules of hydrated water will be determined per molecule of anhydrous salt. Purpose. It is toxic and should be considered hazardous waste and not washed down the sink. To determine the formula of a hydrate experimentally, we must calculate the mole: mole ratio of the water portion compared to the anhydrate portion. for number three the amount of water will decrease of course 4. a) beaker not dry b) hydrate stuck on apparatus. 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