ĞÏࡱá > şÿ H J şÿÿÿ G ÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿì¥Á 5@ ğ¿ ² bjbjÏ2Ï2 %&. Academic year. 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. Hydrate Lab; Hydrate Lab. Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. However, there must be a few sources of errors that affected the data. Less moles of magnesium sulfate in the beaker would have then increased the ratio as the number of water moles would have been divided by a smaller value. Heat the content of the crucible with its … ratio of water/salt (actual value, and then the closest integer) formula of hydrate. Hydrates are solid ionic compounds that contain water that is chemically bound to the crystal. 2018/2019. 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. Name: Lab Report #: Chemistry Rubric for Percent of Water in a Hydrate Lab Composition ____ Heading Name, Partner’s Name, Experiment Date, Report Due _____/ 5 pts ____ Title: Descriptive, short and unambiguous (eg: The Effect of Various Doses of Alcohol on the Reproductive Abnormalities In doing this lab, the percentage of water contained in various hydrates, if dehydration is a reversible or irreversible change, and the mathematical relationship between starting mass and mass lost. Chemistry (CHM104) Uploaded by. Determining the Chemical Formula of a C S. From Copper to Copper Lab. By measuring the compound before heating and after, the hydrate number of the magnesium sulfate can be determined, answering the original lab question. University. Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO. Back to your hydrate lab report the original red burgundy color going from the data if the color of an interesting variation on the metal was taken out data. Students also viewed. Carbohydrates are essential in foods as an energy source (starch is the main source of human calories), a flavouring (simple sugars are usually sweet) and as a functional ingredient (sucrose allows ice cream to be soft in the freezer; xanthan gum thickens a low-fat salad dressing). LABS Lab Equipment Density Lab Percent Composition of a Hydrate Lab Freezing and Melting point of water Freezing Point of Naphthalene LAB SEPARATION METHODS #1 Separation Methods #2 Chromatography Pure substances, Mixtures and Compounds Flame Test Lab Ionic or Covalent? Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Example #1. It is important to know how much water is in the hydrate because when performing scientific experiments, it is required to know the mass of each substance. This phenomenon could have deviated the ratio by causing a loss in the amount of water and anhydrate. Rockland Community College. listed below. How can we experimentally determine the formula of an unknown hydrate, A? 3 grams of an unknown hydrate (in plastic bags or bottles) Procedure: , 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. 9H2O), 1.48g CuSO4 x 1 mol CuSO4 / 159.61g mol-1 CuSO4 = 0.009273 mol CuSO4, 1.47g H2O x 1 mol H2O / 18.02g mol-1 H2O = 0.08158 mol H2O, number of moles H2O / number of moles CuSO4, = 0.08158 mol / 0.009273 mol = 8.80 mol H2O / 1 mol CuSO4     (3 significant figures), 1.48g MgSO4 x 1 mol MgSO4 / 120.36g mol-1 MgSO4 = 0.01230 mol MgSO4, number of moles H2O / number of moles MgSO4, = 0.08158 mol / 0.01230 mol = 6.63 mol H2O / 1 mol MgSO4, 1.48g FeCl3 x 1 mol FeCl3 / 162.20g mol-1 FeCl3 = 0.009125 mol FeCl3, number of moles H2O / number of moles FeCl3, = 0.08158 mol / 0.009125 mol = 8.94 mol H2O / 1 mol FeCl3, 1.48g Fe(NO3)3 x 1 mol Fe(NO3)3 / 241.86g mol-1 Fe(NO3)3 = 0.006120 mol Fe(NO3)3, number of moles H2O / number of moles Fe(NO3)3, = 0.08158 mol / 0.006120 mol = 13.3 mol H2O / 1 mol Fe(NO3)3. Magnesium sulfate, the only left option, is white in appearance which makes it a possible identification for our hydrate. Thus, at the end, we learned that there are countless numbers of applications of stoichiometry in chemistry. 3.) Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Antonopoulos at Salve Regina University. Hydrate Lab Report Elizabeth Herman, Zara Jordan, & Emily Motallebi Performed on: 10/08/2018 Final copy printed on:10/25/18 The purpose of this lab was to determine the hydration number (n) in the hydrate. 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. Less amount of the hydrated salt removing the identity of the water of hydrate. The last idea we learned was how to apply the knowledge of colors of specific ions and solids. By knowing that ions such as Cu, have their designated colors, we were able to eliminate three options for the anhydrate, FeCl. Types of Reactions Lab Report. This particular lab explores the relationship between the anhydrous salt and water in a hydrated sample; it helps students to better understand the concept of the Law of Definite Proportions. Record the mass of the crucible, cover and sample. University. A hydrate is a substance that water. By using both quantitative and qualitative approaches, we can successfully predict the identity of the hydrate and its structure consisting of anhydrate and water. Hydrates are solid ionic compounds that contain water that is chemically bound in the crystal. 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. 2.) Dissolve all in a lab answers by mass of the crystals are specific number of hydration for crucible tongs to the lab today in hydrate! save Save Unknown Hydrate Lab For Later. 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. Furthermore, this lab illustrated a new term for the group - hydrate. If the heating continued on for longer, more water could have evaporated to the air, leaving less amount of anhydrate left in the beaker. 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. This experiment involves heating said hydrates … By using both quantitative and qualitative approaches, we can successfully predict the identity of the hydrate and its structure consisting of anhydrate and water. This means we can exclude these three options from our prediction. CuSO 4 • n H 2 O based on its consecutive masses. Magnesium Oxide Lab Report. (My answer - hydrate didn't reach room temperature, contamination, oil from the hand getting on crucible) Any more errors that are unavoidable. From this lab, we are able to conclude that our prediction was strongly supported in both terms. Once the numbers of moles of two substances are known, the ratio can be computed by dividing them. View Dehydration of a Hydrate Lab Report.docx from CHEM 151 at Central Carolina Community College. You must observe and analyze these as part of the lab.The Iced Tea Debate The Salty Soup The Fire Bug 2 Use the DATA chart provided for recording observation based on three demonstrations you will watch 3 Watch each part of the experimental demonstration and make preditions about wht will happen in each scenario . = 0.08158 mol / 0.009273 mol = 8.80 mol H, = 0.08158 mol / 0.009125 mol = 8.94 mol H, = 0.08158 mol / 0.006120 mol = 13.3 mol H, | (actual value - experimental value) / actual value | x 100%, From this lab, we are able to conclude that our prediction was strongly supported in both terms. Kimberly Graziano & Hyunjae Kim. A hydrate is a compound that is chemically combined with water molecules. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Cecilia Evasco. Lab Report. Before this, we had heard of this scientific word briefly in textbooks and in class, but we were never sure of its exact definition. The conclusion for this lab will consist of the answers to the discussion questions below, plus a brief summary paragraph. 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. Click here are the lab report must occur so that the gases that they are not lose material analysis or be. Lab Report Help Center. In this lab, we learned how to apply stoichiometry in a new way to determine a formula of a hydrate. Identity of the Hydrate: MgSO47H2O Magnesium heptahydrate, % Error = | (actual value - experimental value) / actual value | x 100%, = | (6.63 - 7.00) / (6.63) | x 100% = 5.58% Error. Its experimental ratio was 6.63 to 1 and its expected ratio was 7:1. Dehydration of an Inorganic Salt Hydrate Student Name Matthew Baldwin Date 1 Data Activity 1 Data But as soon as we used previous knowledge of stoichiometry by using molar masses and numbers of moles, we were easily capable of depicting a reasonable empirical formula for the hydrate. In this first lab we attempted to discover which of the materials given to us were hydrates by heating them and then dissolving them in water. 0 0. Hydrate Lab – Examples of Good “Discussion of Theory” Sections. percent of water lost by the hydrate can be calculated. They are crystalline compounds that have a specific number of water molecules trapped within the crystal lattice. final lab#1. By applying heat to our hydrate, we were able to get rid of the water in the compound and find the masses of the water and the anhydrous compound. 840 Words 4 Pages. Chem 1A 04 Lab 6 Conductivity Chem 1A 04 Lab 4 Precipitation Chem 1A 04 Lab 1 Measurements Report Exam Winter 2020, questions Lab Report … Aspirin Synthesis and Analysis. The purpose of this lab is for students to dehydrate a hydrate and use the mass data obtained in lab to calculate the number of moles of water that were attached to the hydrate. Helpful? 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. Get help on 【 Hydrate Lab Report for Chemistry Lab 】 on Graduateway Huge assortment of FREE essays & assignments The best writers! 6 6 upvotes, Mark this document as useful 1 1 downvote, Mark this document as not useful Embed. Print. Purpose. We obtained the percentages through experimental procedures of reacting Ca(NO3)2 with Na2CO3 , filtrating and drying CaCO3. Lab-report 4 - Calculation of Mass Percentage of Water in Unknown Hydrate Calculation of Mass Percentage of Water in Unknown Hydrate. 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. General Chemistry (CHEM 1A) Academic year. All these concepts were learned in class, and this lab was performed to demonstrate these concepts, and allow us to use them in a real world example. What does it mean by errors in the procedure, is it like the directions are not clear? Home Data and Calculations Conclusions Conclusions: This laboratory investigation explored the relationship between percent composition and molar ratios and how to use one to find the other. Since copper (II) sulfate is usually a bright blue due to Cu. The aim of experiments was to determine the percentage of water in hydrated Ca(NO3)2. Show the following calculations in your lab report for each trial: moles of water. Introduction. 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. Related titles. The chemical equation of… The calculated mass of water lost from the compound is 0.286g, and this number is calculated to be 28.1% of the total compound. This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. , we can exclude that option from our prediction. An insufficient amount of time for waiting until all water of the hydrate evaporated. 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. The number of water molecules in a hydrate is called the hydration number and it can be calculated using moles of water per mole of anhydrous compound.