percent water in a hydrated salt lab report experiment 5

Example; . hypothesis was that if the salt was heated multiple times, the mass would decrease as hydrated salt (%), Average percent H 2 O in hydrated salt What will be the probable effect if you kept the crucible completely covered during the entire heating and cooling processes? Several calculations were made to determine the Salt Unknown. Work in groups to design the experiment. Compare this value to the experimental percentage you obtained. Discussion A hydrate salt is composed of anions negative ions and cations positive ions which are surrounded by and weakly bonded water molecules. water through evaporation from heating the hydrated salt sample using laboratory apparatus such The hypothesis of this experiment was accepted on the basis that heat. Record exact mass. Experiment 605: Hydrates . Mass of water lost (g 4, Percent by mass of volatile water in hydrated salt (%) Data Analysis, B Average percent H2O in hydrated salt (%H2O) Data Analysis, C * 6 Standard deviation of%H,0 Data Analysis, D 7, Relative standard deviation of % H2O in hydrated salt (%RSD) Show calculations on next page. This was done by heating a hydrated salt sample multiple times via O is named sodium thiosulfate pentahydrate. Don't forget to submit your proposal. Hydrates are ionic compounds that contain water molecules as part of their crystal structure. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}): \[m_{\ce{H2O}} = m_{\text{Hydrate}} - m_{\text{Anhydrous Solid}} \label{3}\]. Percent water in a hydrated salt lab report experiment 5. The main objective of this experiment was to use gravimetric analysis to determine the Section 1: Purpose and Summary . 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(Repeat this process, if necessary, until the mass of the sample is within0.01g of the previously recorded mass.). calculations were made. Nwanze Abstract The purpose of experiment five was to calculate the percent of H 2 O in an unknown hydrated salt. Since your instructor/TA won't be there in person tosupervise your experiment, you will need to upload a few photos taken during the lab: Complete your Lab Report and submit it via Google Classroom. Average % H 2 O = (43 + 42 + 43) / 3 = 43%, Discussion Cross), The Methodology of the Social Sciences (Max Weber), Laboratory Manual For Principles Of General Chemistry - 10th Edition (dragged), EXP 9 and 10 Volumetric and Vinegar Analysis Lab Report.docx, Summary Chemistry: A Molecular Approach Ch. B.4 by Mass of Volatile Water in Hydrated Salt (%) It determines the, mass of water in a hydrated salt after it is heated to form an anhydrous salt. also learning how to handle laboratory apparatus. This is also called theanhydrous salt. weighed again, and the test tube was then heated for 5 minutes. When the denominator of the fraction is bigger, the answer (percent of water) will decrease. Instructor Name: Daniel de Lill Mass of fired crucible and lid ) 39.674 40.796 39.683 40.236 41.620 40.593 2. The crucible is used with tongs to hold the hydrated salt that is being heated. Bunsen burner would have been incorrect. Using your clean and dry scoop, place the blue hydrate on the paper until you have between 3. After heating in Part A.1, the crucible is set on the lab bench, where it is contaminated with the cleaning oil used to clean the lab bench, but before its mass is measured. would be reported as being too high simply because the crucibles mass repeat this to ensure accuracy. need help with the blanks with work shown. apparatus, Final mass of test tube and anhydrous calculations show the decrease in mass as our salt was being heated multiple times. and h s. Instructor's approval of flame Mass of crucible, lid, and anhydrous Ist mass measurement (e) 2nd mass measurement (g) 3rd mass measurement (g) 5. J.A Beran, laboratory manual for principles of general chemistry. Experimental errors that could have occurred during the Determine the number of moles of water, x, per mole of anhydrous salt and write the chemical formula of the hydrate sample. Explain. The mass of of anhydrous CaSo4 salt is 1. Experiment 5: Percent Water in a Hydrated Salt. Before experimenting, one This percentage can be determined through a series of steps, including drying the salt, weighing it, and then rehydrating it with a known volume of water. Careful control of the temperature and time of the drying and rehydration processes, as well as accurate measurement of the masses, is crucial for obtaining accurate results. Hydrates are ionic compounds that contain water molecules as part of their crystal structure. Experiment_605_Hydrates_1_2_1 is shared under a CC BY license and was authored, remixed, and/or curated by LibreTexts. Keep in mind, that you have to use your own data and no two reports can be exactly the same. A. Beran (10th Ed.). This will give the percentage of water in the hydrated salt. Experiment 5: Percent of water in a hydrated salt Professor: Obiajulu V. Nwanze Abstract The purpose of experiment five was to calculate the percent of H 2 O in an unknown hydrated salt. be unaffected because, as stated previously, the oil is being completely burned Such water, molecules are referred to as waters of crystallization. have been accepted as our weighing of the sample would have been off and our use of the Your instructor/TA will use them to come up with a final experimental protocol that you will be using during the next lab period. A hydrated salt sample was then placed in the test tube and the test tube was weighed again. Each type of, hydrate traps water in its own unique way but heating a hydrate will release the water and leave, the dehydrated material behind. The salt is then cooled and weighed once again. heptahydrate is 43%, there was some error that occurred during this experiment which can be Chemistry 1300 Section D 9/5/ Dr. Nagaraju Birudukota. Accessibility StatementFor more information contact us atinfo@libretexts.org. salt, mass of water lost, percent by mass of volatile water in hydrated salt, average 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. Your Lab Reports are individual assignments, but you're welcome to communicate with your group and discuss the results. What mass due to, Perform the calculations and record the following data in the table below. When the denominator of the fraction is bigger, the . B. %water= \(\frac{\text {massofwaterlost(g)}}{\text { massofhydrate(e)}}=\)x100. Anhydrous also will be a part of this lab because an anhydrous means to be with no water: describes compounds that contain no water, or crystals that lack chemically bound water of crystallization. Adriana Cerbo Chemistry 1300 Lab Section D Tuesday 3:00-5:45PM Instructor Name: Daniel de Lill Date Experiment was Performed: September 1, 2020. C. Excited electrons do. 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Since the, professor instructed to stop weighing after the mass of the anhydrous salt was less than 0.01, grams in change, this second measurement resulted in the final mass for both of the trials, performed in this experiment. Since you know the starting amount, and the final amount, you can calculate how much water was driven off. reading are complete, just need questions 4 to 7 completed. Propose the experimentprotocolto rest of the students in the class. water evaporates. : an American History (Eric Foner), Brunner and Suddarth's Textbook of Medical-Surgical Nursing (Janice L. Hinkle; Kerry H. Cheever), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Business Law: Text and Cases (Kenneth W. Clarkson; Roger LeRoy Miller; Frank B. Question: Experiment 5 Report Sheet Percent Water in a Hydrated Salt Lab Sec. Group of answer choices blue black green white Flag this Question Question 3 0.5pts What was the color of the copper sulfate after, Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. Salvador. Page 79- 84 Laboratory Manual for Principles of General Chemistry Hydrate Lab Report for Chemistry Lab The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. Record your observations. Abstract Gravimetric, analysis is a method that relies on mass measurements for analysis (Beran 85). Write the chemical formula of the hydrated form of your unknown sample. Percent by Mass of Volatile Water in Hydrated Salt (%) = [(Mass of water o In this laboratory experiment one can conclude that by doing this experiment a person is Our Experts are tested by Chegg as specialists in their subject area. The fired crucible is handled with (oily) fingers before its mass Course Hero is not sponsored or endorsed by any college or university. Experiment 5 Lab Report - Experiment 5: Percent Water in a Hydrated Salt Objectives To determine - Studocu experiment percent water in hydrated salt objectives to determine the percent mass of water in hydrated salt. tube. After heating the salt crystal is called ANHYDROUS, meaning without water. during the experiment. There was an error in calculating the mass of the crucible. The standard deviation of percent of water is 0. This was done in three different trials. The percent error is determined by subtracting 170 Words 1 Pages in an anhydrous salt. Percent by Mass of Volatile Water in Hydrated Salt= [0] (100) Instructors approval of flame and While heating, closely observe the solid and the inside wall of the test tube. Using a gravimetric analysis, the mass of the hydrated salt (Athens), would be measured, poured in a crucible to be heated in order to remove the hydrated water, molecules, and measured again. In this experiment, two trials were conducted instead of three, and 1.50 grams of unknown hydrated salt A, instead of 3 grams, were put into a crucible and weighed as instructed by the professor. When the crucible is cool and safe to touch, weigh on an analytical balance. Some compounds lose this water of hydration spontaneously (efflorescent) while some may require heating. This ratio is expressed in the formula of the compound. For your experiment design use the supplies mentioned above. Many salts in nature, the grocery store, or from chemical suppliers are chemically hydrated with water molecules, referred to as the waters of crystallization. Part A. Cross), Experiment 8 Limiting Reactant Lab Report, Experiment 7 Empirical Formulas Lab Notebook and Pre-Laboratory Questions-3, EXP 9 and 10 Volumetric and Vinegar Analysis Lab Report.docx, The main objective of this experiment was to use gravimet, Summary Chemistry: A Molecular Approach Ch. laboratory experiment include human error given that there is always of chance of We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Unformatted text preview: Experiment 04 - Percent Water in a Hydrated Salt- Lab Report C H M 1 0 4 5 L - D r. Furthermore, to figure out the percent water in the hydrated salt, divide the water lost by the mass of the hydrated salt and multiply by a 100. Hydrated salts that spontaneously lose water molecules to the atmosphere are. Experiment 5 Report Sheet Percent Water in a Hydrated Salt Lab Sec. The, mass of the hydrated salt is mass of the crucible, lid, and the measured 1 gram of the Athens salt, minus the mass of the fired lid and crucible. One must be able to handle the crucible properly with the use of tongs specifically after Mass of crucible, lid, and anhydrous salt 1st mass. Assemblea wire triangle supported on an iron ring attached to a ring stand. and h s. Instructor's approval of flame Mass of crucible, lid, and anhydrous Ist mass measurement (e) 2nd mass measurement (g) 3rd Objectives NOTE: You need to have both the total mass of the crucible,lidand sample as well as just the sample. This means that it will seem like that there was more sample was lost than it actually had, therefore making the reported mass of the anhydrous salt too low. Mass of anhydrous salt (8) 3. Mass of fired crucible, lid, and bydrated salt () 3. Responsible for the Safety component in all aspects of the experiment, Validates group members have the supplies, Responsible for formulating the purpose and the goal of the experiment. One deviation from the published procedure was that Most salts in nature are hydrated, in which the water molecules are, chemically bounded to the ions of the salt as a part of their structure (Beran 85). However, if the oil was failed to be completely burnt off of the fired crucible Calculate the mass of the heated(dehydrated)sample. Trial one was calculated accordingly, following the procedure, whereas the second trial was This percentage can be determined through a series of steps, including drying the salt, weighing it, and then rehydrating it with a known volume of water. Mass of water lost (g) 4. associated with each formula unit (Tro 105). Observe each sample occasionally as you perform the rest of this experiment. Mass of fired crcible, lid. percent by mass of water in this hydrated salt to be 43%. Salts are compounds composed of a metal ion plus a non-metal or polyatomic ion, e. Subsequently, in Part B. The experiment performed in this lab uses gravimetric analysis which Mass of anhydrous salt: 37. hydrated salt (%RSD), Mass of test tube and hydrated salt (g) Mass of test tube (g) = Mass of hydrated salt (g). With the use of both these terms and numbers calculated one Digication ePortfolio :: General Chemistry Alexander Antonopoulos by Alexander P. Use the letter n to represent the number of moles of water driven off per mole of anhydrous magnesium sulfate. Continueproviding highheatfor additional 10 minutes. After the mass was measured, the crucible, lid and hydrated salt were put on the, Bunsen burner for 5 minutes on low heat and 10 minutes on high heat. Spokesperson (Optional, for groups with 5 students). The 'x' here is a number which represents the number of molecules of water in the crystal. and h s. Instructor's approval of flame Mass of crucible, lid, and anhydrous Ist mass measurement (e) 2nd mass measurement (g) 3rd. Civilization and its Discontents (Sigmund Freud), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Psychology (David G. Myers; C. Nathan DeWall), 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.), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Biological Science (Freeman Scott; Quillin Kim; Allison Lizabeth), Give Me Liberty! After the salt has been dried and weighed, it is rehydrated by adding a known volume of water to it. The purpose of this experiment was to learn how to handle laboratory apparatus by Parameters you need to account for in your proposal: Each member of your team will have a role for the experimental design assignment. This was the average between trial 1 and trial 2. These calculations include the mass of hydrated salt, the mass of anhydrous a. In a hydrated salt lab report experiment, the percentage of water in a hydrated salt refers to the amount of water that is chemically bonded to the salt molecules. to some of these salts, the bonds between the water molecules and the salt itself breaks, resulting Percent by Mass of Volatile Water in Hydrated Salt= 44% After cooling a second time the crucible, lid and anhydrous salt were weighed, which gave, a reading of less than 0.01 grams in change from the first anhydrous salt measurement. Tuesday 3:00-5:45PM This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. This is a two period lab where you will be working in your Kitchen Chemistry Lab while connected with your group via Zoom Breakout Rooms. The hydrated salt is overheated and the anhydrous salt thermally decomposes, one product being a gas. To determine the percent by mass of water in a hydrated salt. (100) Our results reflect our hypothesis because the final mass the percent water in the hydrated salt be reported as being too high, too low, or 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. Introduction A.2. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. following thermal decomposition of the hydrated salt in Part B. Your Teammates have to be able to see and hear you. Many naturally occurring salts, for example, the ones you buy from the grocery store to hydrated salt. We reviewed their content and use your feedback to keep the quality high. yielded align with and support our hypothesis that the anhydrous salt would weigh less than the Trial 1 Trial 2 Trial 3, Only need ONE example of each type of calculation, 91 g - 90 g = 1 g While heating, the cleaning oil is burned off the bottom of the crucible. In conclusion, our hypothesis was accepted based on the fact that our calculations Since the actual value of the percent by mass of water in zinc sulfate Accessibility StatementFor more information contact us atinfo@libretexts.org. Record exact mass. Experiment 5 Report Sheet Percent Water in a Hydrated Salt Lab Sec. References On the other hand, an anhydrous salt (without water)canabsorb water from the atmosphere and spontaneously dissolve in its own water of hydration(deliquescent). 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. by learning how to properly use different laboratory apparatus like tongs, Bunsen burners, and Molar mass of water, H2O: ___________________g/mol. Many water molecules are chemically bound to the ions of salt in its crystalline Whatchanges did you see? Mass of fired crucible and lid ) 39.674 40.796 39.683 40.236 41.620 40.593 2. The percent water in the hydrated salt will be too high because the contamination will add more mass creating a larger gap between the initial measurement of the hydrated salt and the final measurement of the anhydrous salt. Lab Section D Using a test tube holder, grasp the test tube containing the hydrate and heat over a Bunsen burner flamewhileholdingthe test tube at a 45angle. Percent by mass of volatile water in hydrated salt (%) 5. analysis, an analytical strategy that depends almost exclusively on mass measurem, analysis, to determine the percent by mass of water in a hydrated salt. Check for stress fractures or fissures. Pearson One must then repeat this to ensure Calculate the ratio of moles of water lost to moles of anhydrous salt. Explain. apparatus, the method of gravimetric analysis is used by heating up a hydrated salt sample over a, Sample Name: El Salvador Hydrates contain water molecules in their crystalline structure these molecules can be removed by heat. Heat can remove the water molecules that are chemically bonded to the ions of salt, and form anhydrous salts. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Antonopoulos at Salve Regina University. Record exact massof the crucible andlid. Thank you! An anhydrate is the crystalline compound without the water molecules bound to it. Final mass of test tube and anhydrous salt (g) Mass of test tube (g) = Mass of anhydrous salt Final mass of crucible, lid, and anhydrous salt () Calculations 1. Bunsen burner and then weighing it on a balance. Mass of Water Loss (g)= 0 Trial | Trial ! One of these laboratory materials being the crucible. The ratio calculated(j)is expressed in the formula of the compound (hydrate). Mass of hydrated salt (g) anhydrous salt (e) 3e 072 1001oGl 2. The bound water is called the water of hydration. off. What is the empirical formula of the copper sulfate hydrate? The molar mass of water is 18.015 g/mol and the molar mass of, Which of the following statements is true?A. water evaporates. sample of hydrated salt being El Salvador. These terms being efflorescent (hydrated salts that spontaneously, Suppose the original sample is unknowingly contaminated with a second anhydrous salt. 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Experiment 5: Percent Water in a Hydrated Salt. Put a clean, dry porcelain crucibleand lidon the wire triangle and heat over a Bunsen burner flame for about three (3) minutes to ensure complete dryness. This percentage can be determined through a series of steps, including drying the salt, weighing it, and then rehydrating it with a known volume of water. Once the oil is burned off the bottom of the crucible, it will make it seem like the sample has lost more water than it truly has. You should contact him if you have any concerns. After gentle heating for about 5 minutes, increase the heat applied tothe crucible, lid,and sampleuntil the bottom of the crucible turns red. Mass of. While heating, the cleaning oil is burned off the bottom of the crucible. 4. BA 6z . removed some of the water molecules of the hydrated salt to form an anhydrous salt. balances. Standard deviation of SHO Data Analysis, 7. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. (g) The mixture is then heated again, this time at a lower temperature, until all of the water has been absorbed by the salt. The mass of the anhydrous salt is final mass, measurement of the heated hydrated salt minus the mass of the fired lid and crucible. Because the cleaning oil was added, the crucible will be thought as having more mass than it actually does. Laboratory Manual for the Principles of General Chemistry, 10th Edition. Then you will use your data to calculate the. measurement would be high. As, result water was lost in the hydrated salt (Athens) but not enough; the percent error within this, measurement is 9.7%. heptahydrate sample then allowed us to calculate the average percent of water lost which came Using crucible tongs, place the lidand the crucibleon a wire gauze on the bench to finish cooling to room temperature. The reported percent of water in the hydrated salt will be too low because the second anhydrous salt will add mass, which means the overall total mass is higher. The purpose of this experiment was to determine the percent by mass of water in a hydrated salt by heating the salt in a crucible and measuring the mass differences with a gravimetric analysis. Suppose the original sample is unknowingly contaminated with a second anhydrous salt. (Mass of water lost / Mass of hydrated salt) * 100 = Percent by mass of volatile water in the heating of the hydrated salt sample. Results and Discussion An electron may fall back to ground state in a single step or in multiple steps. In addition to the hydrated salt being burned off, the oil is also burned off. must acknowledge the information that was given as well as already interpreted (background We hypothesized that if the salt was heated multiple times, the mass would decrease That Salt being El You'll get a detailed solution from a subject matter expert that helps you learn core concepts. the ions that heat removes them). analysis, to determine the percent by mass of water in a hydrated salt. From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid, the number of moles of water and moles of the anhydrous solid are calculated as shown below (\ref{4}, \ref{5}): \[n_{\ce{H2O}} = \frac{m_{\ce{H2O}}}{MM_{\ce{H2O}}} \label{4}\], \[n_{\text{Anhydrous Solid}} = \frac{m_{\text{Anhydrous Solid}}}{MM_{\text{Anhydrous Solid}}} \label{5}\]. can discover the identity of an unknown sample of hydrated salt. Date of Experiment: SUMMARY 5 PTS Please write short introduction for the experiment. Experiment 5: Percent Water in a Hydrated Salt, Adriana Cerbo Will the reported percent of water in the hydrated salt be too high, too low, or unaffected? { "001:_Preface_1_Course_Information" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "002:_Safety" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Experiment_1-_Measurements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Experiment_2_-_Nomenclature" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Experiment_3_-_Chemical_Formula" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Experiment_4_-_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Experiment_5_-_Calorimetry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Experiment_6_-_Atomic_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Experiment_7_-_Molecular_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Experiment_8_-_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Appendix_1_-_Precision_of_Measuring_Devices" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Appendix_2-_Quantitative_Techniques" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Homework : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Laboratory : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Text : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Worksheets : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FUniversity_of_Arkansas_Little_Rock%2FChem_1402%253A_General_Chemistry_1_(Belford)%2FLaboratory%2F03%253A_Experiment_3_-_Chemical_Formula, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 2.9: Calculations Determing the Mass, Moles and Number of Particles, Prefilled Hydrated Salt Lab Report is available in the.

percent water in a hydrated salt lab report experiment 5 2023