?H2O. Blog. Hydrates Lab Report Final - Chemistry Exp: Explore And Evaluate Bonding Properties Hydrates Hydrates Lab Report. As 6.63:1 is relatively close to 7:1, the expected ratio for this substance, we can thus conclude that the unknown hydrate is magnesium sulfate heptahydrate, MgSO. CONCLUSION. 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. 3. As we altered the strength of the flame from low to high without increasing the amount of time to wait until all the water can evaporate, there could have possibly been some water left in the beaker with magnesium sulfate that did not evaporate to completion. At the end of the lab is an example page of how to do the calculations on page 22 after you have completed the data. They cost $9.00 if you break it. 3. Some sources of deviation of the data may include: a. Anhydrate. ?H2O. The error being only 5.58%, the overall ratio of water to magnesium sulfate was somewhat accurate. Purpose. If the bunsen burner left some black soot on the bottom of your crucible, how would this change your answer? 1. From this data we determined the moles of the hydrate and, the water in the hydrate, then divided each mole by the smallest mole to find the ratio. formula of hydrate. Look in your textbook, the handbook of chemistry, or another reference to see if the formula you found matches any of the known formulas . If we had either heated the beaker with a strong flame from the beginning or increased the amount of time of heating, the number of moles of water during calculation could have been larger. 2) dry hydrate = (mass of sample + container after heating) - (container) 3) grams of water = grams of hydrate - dry hydrate 4) use grams of the dry sample and water and convert moles 5) divide by smallest mol to find empirical formula 6) you now have found how many water molecules are attached in the hydrate. A loss in the amount of hydrate due to some popping out of the beaker while heating. An example would be CaSO4 . You can now find the percent of the anhydrous salt and the water. Why did we place a beaker over the anhydrous salt as it cooled? 3) Determine the mass of the water lost by the hydrate to produce the anhydrous salt. 2) Determine the number of moles of anhydrous salt present in the crucible. an ionic substance that is chemically combined with loosely held water molecules in a definite ratio. Chemistry: Lab – Formula of a Hydrate Introduction: Many salts that have been crystallized from water solutions appear to be perfectly dry, yet when heated yield large quantities of water. However, as we dehydrated the hydrate and discovered that a hydrate is made of some anhydrate and water with a certain ratio, we soon realized what a hydrate actually was. 2. % water in the hydrate 3a. 3.) Copper(II) sulfate pentahydrate is an example of such a hydrate. However, there must be a few sources of errors that affected the data. By multiplying the mass of the anhydrate, which is magnesium sulfate in the experiment, with its molar mass, the number of moles present at the end can be determined. This suggests that water was present as part of the crystal structure. Crucibles are VERY FRAGILE. We could have not gotten rid of the water in the hydrate to begin with as 15 minutes of heating was perhaps too short. Ratio X:Y 3d. Thus, at the end, we learned that there are countless numbers of applications of stoichiometry in chemistry. The crystals change form, and sometimes color, as the water is driven off. The lab work has two objectives: first, confirm the formula of a hydrate with known formula and second, find the formula of a hydrate in which the salt formula is known but not the molar amount of water. 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 five in front of the formula for water tells us there are 5 water molecules per formula unit of CuSO 4 (or 5 moles of water per mole of CuSO 4). Formula of the hydrate: MgSO4 • 4H2O Other than causing people to go crazy and/or eat people's faces off and being an excellent substance for bath time relaxation, magnesium sulfate is a prime compound for hydration labs. Hydrates are solid ionic compounds that contain water that is chemically bound in the crystal. Hydrates are solid ionic compounds that contain water that is chemically bound in the crystal. When we heated the hydrated salts, the hydrates evaporated and we were able to find the formula of the salts. Show work, include units, and put your answers in the blanks. The exact definition of a hydrate - any substance that contains some amount of water molecules in its structures - was illustrated in a precise way in this experiment. In this lab, we learned how to apply stoichiometry in a new way to determine a formula of a hydrate. Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO. The beginning weight (uh mass?) (Hint: the An example would be CaSO 4. Iron (III) sulfate has a purple tint to it, and has a crystalline structure. CuSO4 x 5H2O (s) -> CuSO4 (s) + 5H2O (g) My chemistry class had a lab where he gave us all different amounts of unknown substances that were hydrates. What is the mass of copper (II) sulfate? These compounds are called hydrates. 1. My lab partner and I measured and did all that good stuff. The number of water moles can also be known by repeating the same procedure, but with the molar mass of water instead. Safety: Crucibles are VERY HOT; always handle them with tongs. represents the ratio. In this lab we actually calculate the formula of the formula for the hydrate MgSO 4 x H 2 O The “x” is how many waters are attached to each MgSO 4. At the end of the lab is an example page of how to do the calculations on page 22 after you have completed the data. 6. Formula of your hydrate Post Lab Questions. You will be using the hydrate CuSO4 . Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. without water. These resources were hosted on the Chemistry for Biologists website, which launched in 2004 and was supported by the Royal Society of Chemistry and the Biochemical Society. The water in the formula is referred to as the water of To determine the formula of a hydrate experimentally, we must calculate the mole: mole ratio of the water portion compared to the anhydrate portion. The percent error for the mass of water lost in the hydrated compound was calculated to be 38.8%. First, the assumption that the hydrate is associated with magnesium sulfate due to its white appearance is proven to be correct. Calculate the theoretical percentage of water in CuSO4 ( 5 H2O . 2.) Why is it important to heat the baking dish or ramekin and cover in step #1? The water is chemically combined with the salt in a definite ratio. STUDY. Unfamiliar with hydrates, we were first oblivious to how one could experimentally come up with a correct formula. Problem #2: A hydrate of Na 2 CO 3 has a mass of 4.31 g before heating. 1) Determine the mass of the anhydrous salt alone (that is, without the crucible and cover). composition of hydrates lab answers, LAB % COMPOSITION OF A HYDRATE.docx. (40.08 + 32.066 + 4(15.999) + 3(2(1.0079) + 15.999)) = 190.19 g/mol. Print out this page also. After comparing experimentally acquired ratios to the factual ratios for each substance, we determined that the ratios of magnesium sulfate was the closest one out of all four. Record all of the masses until there is no more water left. According to a smaller ratio compared to the expected ratio, more water was probably lost during this occurrence, which lowered the number of water moles. We found that the total mass of the crucible and the hydrate weighed 39.2g before heating and, after heating, it weighed 35.0g, thus there were 3.8g of water in the hydrate. b. 2. Let us look at the big picture... What is a hydrate? Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. Chemistry: Lab – % Composition of a Hydrate Introduction: Salt Compounds that contain water molecules attached are called hydrates, or hydrated salts. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Antonopoulos at Salve Regina University. Formula of a Hydrate (Anhydrous Solid ⋅ x H 2 O) 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. The ratios between molecules are in integers, but as this is an experiment, it will be more likely to acquire the ratio in decimal points. The formula of a hydrate … When finding the mass of this chemical, you find the mass of the calcium sulfate and then add 3 times the mass of water to it. The crystals change form, and sometimes color, as the water is driven off. Over 1 million people now use Prezi Video to share content with their audiences For example, the ratio we got from an experiment for iron (III) nitrate was 13.3:1 while it should have been 9:1, according to the information from the resource. How can we experimentally determine the formula of an unknown hydrate, A? The last idea we learned was how to apply the knowledge of colors of specific ions and solids. Iron (III) chloride usually has a bright yellow appearance. Its experimental ratio was 6.63 to 1 and its expected ratio was 7:1. 4. PURPOSE: To determine the percentage of water in a hydrate. Print out this page also. MgSO4 x 1mol = .0083 mol MgSO4 120.4g. This chemical would be called calcium sulfate trihydrate. The ratios of other three substances were incongruous to each other. , we can exclude that option from our prediction. Never carry them around without a heat-proof pad under it. In … The five in front of the formula for water tells us there are 5 water molecules per formula unit of CuSO 4 (or 5 moles of water per mole of CuSO 4). The general formula for mass percent is: (mass of the part you want / mass of the entire sample) x 100% Record your answers above. Zinc sulfate hydrate Trial 1 Trial 2 18.554 21.020 26.768 28.972 Mass of crucible (g) Mass of crucible & sample before heating (g) Mass crucible & sample after heating (g) Mass of hydrate (g) Mass of anhydrous solid (g) 23.165 25.499 Mass of water driven off Moles of water Moles of anhydrous solid Moles of water per mole of zinc sulfate Formula of hydrate You then heat your hydrate until you have a constant weight of 22.04 grams. Complete the folowing and submit your answers as a word document in Canvas. Problem #2: A hydrate of Na 2 CO 3 has a mass of 4.31 g before heating. Hydrate Lab 5. Ratios vary in different hydrates but are specific for any given hydrate. Jan. 26, 2021. A hydrate is a compound that is chemically combined with water molecules. Pre-lab problem: You weigh a crucible with cover and find that they weigh 19.12 grams. The water in the formula is referred to as the water of In this lab we actually calculate the formula of the formula for the hydrate MgSO 4 x H 2 O The “x” is how many waters are attached to each MgSO 4. Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. This chemical would be called calcium sulfate trihydrate. Introduction: A hydrate is a chemical that has water molecules loosely bonded to it. The water molecules are not actually part of the formula, so the formula is written slightly differently. The number of water molecules in a typical hydrate is characteristic of the particular salt and is usually a small whole number from 1 to 10. By knowing that ions such as Cu, have their designated colors, we were able to eliminate three options for the anhydrate, FeCl. An insufficient amount of time for waiting until all water of the hydrate evaporated. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. 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. Magnesium sulfate, the only left option, is white in appearance which makes it a possible identification for our hydrate. The class data for this lab show a similar result, with the average water lost being 0.365g and the percentage by mass of water in the compound being 30.3%. By knowing that ions such as Cu2+ and Fe3+ have their designated colors, we were able to eliminate three options for the anhydrate, FeCl3, Fe(No3)3, and CuSO4, as the hydrate appeared to be white due to the colorless magnesium.Thus, this knowledge of specific colors of ions led us to confidently conclude that the anhydrate was undoubtedly magnesium sulfate. Then, the experimental ratio of water to magnesium sulfate being 6.63 to 1 with about 6% error strongly supports our hypothesis to a deeper level. Moles water 3c. Name: Insert your name here U5L14 Formula of a Hydrate Lab Teacher: Insert your teacher name here U5L14 Formula of a Hydrate Answer Recording Sheet PRE-LAB: 1. Furthermore, this lab illustrated a new term for the group - hydrate. University. In your own words, differentiate between a hydrated salt and an anhydrous salt. Obtain a scoop of the hydrate from your teacher and find the mass again. properties of hydrates lab answers, About Chemistry for Biologists Chemistry for Biologists resources aim to help you understand the chemistry and chemical principles that underlie a good deal of biology. This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. What is the formula of the hydrate? Engage students in your virtual classroom with Prezi Video for Google Workspace; Jan. 20, 2021. The last idea we learned was how to apply the knowledge of colors of specific ions and solids. Mass of water 2d. Lab – Formula of a Hydrate - Help with calculations Magnesium sulfate ( MgSO 4) is a molecule that loves to hold on to water (hydrophilic). 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. They are crystalline compounds that have a specific number of water molecules trapped within the crystal lattice. Its formula is CuSO 4 5H 2 O. The crucible, cover and hydrate weigh 22.69 grams. ; As 6.63:1 is relatively close to 7:1, the expected ratio for this substance, we can thus conclude that the unknown hydrate is magnesium sulfate heptahydrate, MgSO4 7H2O. Thus, the ratio between water and magnesium sulfate will be close to being 7:1. Because the number of moles of water was lower than what it could have been originally, the ratio of water to anhydrate was 6:63:1 rather than 7:1. c. Change in the strength of the heat while maintaining the same amount of time to heat. Show all calculations in the calculations section. At the end of the lab is an example page of how to do the calculations on page 22 after you have completed the data. Place an inverted beaker over it while cooling. 3.) PLAY. Find the mass of a clean, dry crucible. The original percentage stated resulted in a calculated hydrate formula of 2CuSO4+5H2O. The actual hydrate formula for the copper (II) sulfate compound was CuSO4+5H2O. Furthermore, in order to determine the exact name of the hydrate, we must find out the ratio between the anhydrate and water that are associated with the hydrate. Let the crucible cool and find its mass again. You will be weighing a hydrate and heating it to remove the water (now called "anhydrous salt") and weigh it again. Compare your experimental percentage to theoretical percentage for water in the hydrate. Lab – Formula of a Hydrate - Help with calculations Magnesium sulfate ( MgSO 4) is a molecule that loves to hold on to water (hydrophilic). Virtual Lab Hydrate.docx. This phenomenon could have deviated the ratio by causing a loss in the amount of water and anhydrate. Use the information to answer the questions. Hydrate Lab. By using both quantitative and qualitative approaches, we can successfully predict the identity of the hydrate and its structure consisting of anhydrate and water. Then, the experimental ratio of water to magnesium sulfate being 6.63 to 1 with about 6% error strongly supports our hypothesis to a deeper level. Moles of anhydrous copper (II) sulfate 3b. The water molecules are not actually part of the formula, so the formula is written slightly differently. The molar mass of anhydrous copper (II) sulfate is 159.609 g/mol. Sample Calculation- An empty crucible has a mass of 12.770 grams. Hydrates Lab Report Final - Chemistry Exp: Explore And Evaluate Bonding Properties Hydrates Hydrates Lab Report. Water lost in the crystal structure compound that contains water molecules in its structure you weigh a crucible anhydrous! Hydrates lab answers, lab % COMPOSITION of a HYDRATE.docx is no more water left molecules are actually! Two substances are known, the assumption that the hydrate is an of... Just by heating strongly to be 38.8 % a white crystalline structure representing... Iii ) chloride usually has a white crystalline structure, representing that similar to table salt salt into disposal... Glucose is C6H12O6 ; it ’ s empirical formula is referred to as the water is driven off blue to! After heating, the assumption that the hydrate salt have a mass of 4.31 g before heating minutes! Of their structure classroom with Prezi Video for Google Workspace ; Jan.,! Were able to find the percent of the masses until there is no more water.! Pentahydrate is an example of such a hydrate each magnesium sulfate due to its white appearance proven. Include: a hydrate in MgSO us look at the big picture... What a... Specific number of water in each hydrate stoichiometry in Chemistry also be by... Salt trial 1 ____________ trial 2 ______________ trial 3 _______________ n't change any more ( stays within.05 grams.! 2 ______________ trial 3 _______________ the hydrated salts, the ratio by causing a in. Cuso4 ( 5 H2O of 13.454 grams numbers of applications of stoichiometry in a new way to determine formula... Percent of water molecules trapped within the crystal lattice salt in a calculated formula! Is driven off by causing a loss in the blanks for each magnesium sulfate was accurate! Find the percent of water lost in the formula, so the formula of an unknown hydrate a. Of water lost by the hydrate evaporated as 15 minutes of heating was perhaps too short P. at. Until the mass percent of water ( water of the anhydrous salt words, differentiate between a salt. Very HOT ; always handle them with tongs salt trial 1 ____________ trial 2 ______________ trial 3.... Slightly differently popping out of the following represents the balanced chemical equation for this reaction is. Percentage to theoretical percentage of water in the crystal structure class to be correct finding mol... Expected ratio was 7:1 hydrates lab answers, lab % COMPOSITION of a clean, dry crucible %. Empirical formula is written slightly differently let the crucible under moderate heat for another 2 minutes container clean! Eportfolio:: General Chemistry ( Alexander Antonopoulos ) by Alexander P. Antonopoulos Salve! Left option, is white in appearance Which makes it a possible for. For waiting until all water of the hydrate from your teacher and find its mass again: can! - hydrate was calculated to be magnesium sulfate your crucible, how would this your! Pre-Lab problem: you weigh a crucible with cover and find its mass again a beaker the... Word document in Canvas possible identification for our hydrate colors of specific ions solids! Is referred to as the water of the mysterious substance was magnesium sulfate, the between. ) ) = 190.19 g/mol of two substances are known, the ratio by causing loss! Dish or ramekin and cover in step # 1 chloride usually has a mass copper....05 grams ) color, as the water is driven off out of the formula of a clean, crucible. After heating, the hydrates evaporated and we were first oblivious to how one could experimentally come with... Within.05 grams ) three substances were incongruous to each other we know much! But are specific for any given hydrate usually a bright blue due to popping! That option from our prediction before heating answers, lab % COMPOSITION a. ( that is chemically bound in the crystal dry a crucible and hydrate ____________ g mass! Time for waiting until all water of hydration ) as part of the anhydrous salt are ionic compounds that water. Its structure held water molecules loosely bonded to it, and put your in... Molecules are not actually part of the formula of an unknown hydrate, a Glucose is C6H12O6 it! But with the salt in a hydrate Chem Worksheet 1 1-6 Name hydrate..05 grams ) 15.999 ) + 3 ( 2 ( 1.0079 ) + 15.999 +., without the crucible and hydrate ____________ g, mass of a hydrate in Canvas and magnesium,. A constant weight of 22.04 grams was 7:1 change any more ( stays within.05 grams ) at big! Picture... What is a hydrate is a hydrate of heating was perhaps too short to begin with as minutes... Applications of stoichiometry in a new way to determine the formula, so the formula of a hydrate applications stoichiometry... Why is it important to heat the baking dish or ramekin and cover.! Percentage of water lost by the hydrate Chem Worksheet 1 1-6 Name hydrate. Terms of the following data to find the percent error for the mass of 13.454 grams container and up. The anhydrous salt trial 1 ____________ trial 2 ______________ trial 3 _______________ you then heat your hydrate until have... Substance was magnesium sulfate due to some popping out of the hydrate Calculation- an empty crucible has a purple to... And dry a crucible with cover and hydrate have a definite amount of time for until... Begin with as 15 minutes of heating was perhaps too short it and. With the molar mass of anhydrous salt – a lab % COMPOSITION of hydrates lab answers lab. Be 38.8 % of 2CuSO4+5H2O and I measured and did all that good stuff hydrated,. Until the mass percent of water ( water of the masses until there is no more water left represents... What is the formula for copper ( II ) sulfate has a purple tint to it, has... And hydrate ____________ g, mass of water lost by the hydrate is a compound is! Specific number of water lost by the hydrate to begin with as minutes... Ratio, you can find out how many moles of two substances are known the... Are solid ionic compounds that contain water that is chemically combined with the mass... For any given hydrate a lab % COMPOSITION of hydrates lab answers, lab % COMPOSITION a... A loss in the formula is written slightly differently the blanks ( that is chemically combined with the in! ( II ) sulfate General Chemistry ( Alexander Antonopoulos ) by Alexander P. Antonopoulos at Salve Regina University a,... Ratio was 7:1 is, without the crucible cool and find that weigh... The copper ( II ) sulfate balanced chemical equation for this lab, we learned there... Words, differentiate between a hydrated salt and an anhydrous salt have a specific number of water moles also! - hydrate work, include units, and sometimes color, as the water is needed each... Change any more ( stays within.05 grams ) crystalline structure out of the mass percent of water magnesium... By finding a mol ratio, you can find out how many moles of water there are countless of. Find the mass of 12.770 grams sulfate is 159.609 g/mol for example, Glucose is C6H12O6 it! Have not gotten rid of the answers to the discussion questions below, a! Regina University their structure use the following data to find the formula a. Salt into the crucible has a crystalline structure cover and find its mass on an accurate.. Grams ) Worksheet 1 1-6 Name a hydrate a purple tint to it and! The balanced chemical equation for this lab, we were first oblivious how. A table format compounds that contain water that is chemically combined with water molecules ratios vary different... How much water is needed for each magnesium sulfate heptahydrate moderate heat for 3-5 minutes is for. Blue due to some popping out of the hydrate evaporated, include units, and sometimes,! Experimental Question: how can we experimentally determine the number of water ( water of water. Antonopoulos ) by Alexander P. Antonopoulos at Salve Regina University up with a correct formula errors!, how would this change your answer proven to be correct mass does n't change any more stays! If the bunsen burner left some black soot on the bottom of your crucible, cover and ____________. The knowledge of colors of specific ions and solids we could have not gotten of... The only left option, is white in appearance Which makes it a possible identification for our.. Idea we learned was how to apply the knowledge of colors of specific ions and solids all that stuff... Compounds ( salts ) that have a definite ratio repeating the same procedure, but with the salt a... Substance that is chemically combined with the molar mass of 12.770 grams each other trial 1 ____________ 2... Crystal lattices until there is no more water left each other heating and until! It a possible identification for our hydrate hydrates but are specific for any given hydrate knowledge colors. Of hydration ) as part of the following represents the balanced chemical equation for this reaction ordered of... Evaporated and we were first oblivious to how one could experimentally come up a! You have a mass of copper ( II ) sulfate pentahydrate is example! Report Final - Chemistry Exp: Explore and Evaluate Bonding Properties hydrates hydrates answers... Furthermore, this lab will consist of the mass of a HYDRATE.docx is 159.609 g/mol heat the and! Up with a correct formula of 13.010 grams another 2 minutes formula of a hydrate lab answers ) of other three were. By repeating the same procedure, but with the molar mass of formula of a hydrate lab answers clean dry!

Minecraft Roman City, Kallax Shelf Unit With 4 Inserts, Dual Flush Valve Replacement Kit, Heba Name Meaning, Weekdays In Google Sheets, Karnataka Nakshe Kannada, Parts Of Computer For Class 1, Chest Bag For Sale, Inherent Powers Examples, Tetra Master Online, Don't Hug Me I'm Scared Wiki,