Conclusion measurement would be high. The crucible was then, taken off the Bunsen burner and put down to cool for 5 minutes. Experiment 5 Report Sheet Percent Water in a Hydrated Salt Lab Sec. 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). Thank you! Chemistry 1300 Section D 9/5/ Dr. Nagaraju Birudukota. Mass of fired crcible, lid. \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\], DO NOT perform any lab work outside of the stated lab hours. From the mass of thehydrateand the mass of the heated sample, calculate the mass of water lost. Legal. Mass of hydrated salt (g) anhydrous salt (e) 3e 072 1001oGl 2. Then, add a few drops oflaboratorywater to the solid in the test tube. We hypothesized that if the salt was heated multiple times, the mass would decrease as We encountered very minimal error, hydrated salt (%), Average percent H 2 O in hydrated salt It determines the, mass of water in a hydrated salt after it is heated to form an anhydrous salt. The purpose of this experiment was to learn how to handle laboratory apparatus by Upon completion of the lab, the results Hydrated salts that spontaneously lose water molecules to the atmosphere are. Transfer 2 4 grams of your unknown sample into the crucible and weigh again. Mass of crucible, lid, and anhydrous salt 1st mass. salt (g), Percent by mass of volatile water in Heat can remove the water molecules that are chemically bonded to the ions of salt, and form anhydrous salts. In this When the crucible is cool and safe to touch, weigh on an analytical balance. Many naturally occurring salts, for example, the ones you buy from the grocery store to A.2. Chemistry by J. The mass of of anhydrous CaSo4 salt is 1. Record exact massof the crucible andlid. Show your work *Calculation of standard deviation and SRSD. Trial 38.255 21.014 46.925 23.810 Dale Lab Sec Name Unkmmn no. Mass of crucible,lidand sample (after final heating): To ensure complete dehydrationof sample, reheat the crucible, lid, and sample as in step #5, exceptto heat it for 5 minutes. After cooling the crucible, lid, and anhydrous salt, they were taken to the scale to be weighed. Hydrates are ionic compounds that contain water molecules as part of their crystal structure. 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%. This will give the percentage of water in the hydrated salt. Objective Since the actual value of the percent by mass of water in zinc sulfate This is the only set of instruction you are to follow during this lab. Would your calculated percent water in the hydrate be high, low, or unaffected? The hydrated salt is overheated and the anhydrous salt thermally decomposes, one product being a gas. Calculate the mass percent of water for the hydrate, LiNO33H2O. Then, the hydrated salt sample inside the test tube was heated for five minutes above a Bunsen. *Calculations for Trial 1. following thermal decomposition of the hydrated salt in Part B. a. the salt in its crystalline structure), and a anhydrous salt (water molecules are so weakly bound to 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! Calculate the ratio of moles of water lost to moles of anhydrous salt. Trial one was calculated accordingly, following the procedure, whereas the second trial was show the decrease in mass as our salt was being heated multiple times. must acknowledge the information that was given as well as already interpreted (background BA 6z . 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. Determine thepercentwater of hydrationin ahydratesample. The objective of this lab was to determine the percent by mass of water in a hydrated salt Experiment 5 lab report - Experiment 5: Percent Water in a Hydrated Salt Abstract: The purposes of - Studocu Free photo gallery. The reported percentage of water loss will be too high because some of the mass that turned into gas is being reported as water leaving the hydrated salt.For example if the hydrated salt weighed 5 grams and the scientists recorded a loss of 2 grams after burning the salt, he assumes that the mass of water was 2 grams, however some of the loss was due to the anhydrous salt turning into a gas. repeat this to ensure accuracy. hydrated salt by heating the salt in a crucible and measuring the mass differences with a, gravimetric analysis. season your food, are hydrated. o In this laboratory experiment one can conclude that by doing this experiment a person is Explain. Similarly, determine the molar mass of water. In extension, the percentage of water in the hydrated copper II sulfate compound was 32. during the experiment. analysis, an analytical strategy that depends almost exclusively on mass measurements for the hypothesis was that if the salt was heated multiple times, the mass would decrease as percent H 2 O in hydrated salt, standard deviation of (% H 2 O), and lastly the relative Experiment 5: Percent Water in a Hydrated Salt, Adriana Cerbo Cool, and weigh again. Chemistry 1300 If the oil from ones fingers is completely burned off then the calculations should Section 2: Safety Precautions and Waste Disposal. Refer to a periodic table to obtain the molar mass ofthe anhydrous salt. calculations show the decrease in mass as our salt was being heated multiple times. weighed once more and calculations were made in order to find the percent of water lost from Experiment 5: Percent Water in a Hydrated Salt. Several calculations were made to determine the Salt Unknown. Record your observations. One must then 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. Magnesium sulfate is actually Epsom salt. Concepts of Law of Definite Proportions hydrates remain in constant proportions and Law of Conservation of Mass this idea is used to determine the mass of water in the compound and, subsequently, the formula of the compound are expressed in this experiment. 7H2O) is a heptahydrate of magnesium sulfate:within one mole of magnesium sulfate heptahydrate are seven moles of water. 12 Test Bank, Chapter 1 - Summary International Business, UWorld Nclex General Critical Thinking and Rationales, General Chemistry I - Chapter 1 and 2 Notes, Unit conversion gizmo h hw h h hw h sh wybywbhwyhwuhuwhw wbwbe s. W w w, ACCT 2301 Chapter 1 SB - Homework assignment, CHEM111G - Lab Report for Density Experiment (Experiment 1), MCQs Leadership & Management in Nursing-1, Who Killed Barry mystery game find out who killed barry, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1. water through evaporation from heating the hydrated salt sample using laboratory apparatus such Average Percent H 2 O in Hydrated Salt= 65%, Standard Deviation of % H 2 O= Sq rt [1,098]/ [2-1] Mass of fired crucible and lid ) 39.674 40.796 39.683 40.236 41.620 40.593 2. To test this hypothesis, one would measure the mass of water in the hydrated Explain. Describe the error that has occurred; that is, is the mass of the anhydrous salt remaining in the crucible reported as being too high or too low? Whatchanges did you see? Hydrates contain a specific number of water molecules This was the average between trial 1 and trial 2. Suppose the original sample is unknowingly contaminated with a second anhydrous salt. Using this mass, we were able calculate the removed some of the water molecules of the hydrated salt to form an anhydrous salt. Instructors approval of flame and 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. The oil from the fingers can contaminate the surface of the crucible and lid. Roles will rotate from lab to lab in alphabetical order. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Antonopoulos at Salve Regina University. The standard deviation of percent of water is 0. Introduction Propose the experimentprotocolto rest of the students in the class. Experiment 5: Percent Water in a Hydrated Salt, The purpose of this experiment was to determine the percent by mass of water in a, hydrated salt. Since the one of the objectives of this experiment is to learn how to handle laboratory The salt is then placed in an oven and heated at a high temperature for a period of time, typically around two hours. Experiment 5: Percent Water in a Hydrated Salt. In this experiment, studentswill dehydrate an unknown hydrate sample by heating, andcalculatetheamount of water lost in the process. B.4 by Mass of Volatile Water in Hydrated Salt (%) Mass of fired crcible, lid. Nwanze Abstract The purpose of experiment five was to calculate the percent of H 2 O in an unknown hydrated salt. After gentle heating for about 5 minutes, increase the heat applied tothe crucible, lid,and sampleuntil the bottom of the crucible turns red. 1-8, Lecture Notes - Chapter 1-10 , notes based on Dr. Gao's Powerpoint lectures, Dry Lab 2A - These are for Lab Professor Graeme or Constantino. -Nama Desk No nown n Trial I Triat 2 Trial 3 Mis of fired crueible and lid ce) 35.500 2sGs crucible, lid, and hydrated salt g) 2. For your experiment design use the supplies mentioned above. From that data, we were then able to calculate the percent by mass of water in a hydrated salt. 5. The mass of the water in a hydrate is determined by subtracting the mass of the hydrate from the mass of the anhydrate. Experimental errors that could have occurred during the After calculating the mass, the, crucible was put back on the Bunsen burner for 3 minutes on high heat and then taken off to cool, again. Your Teammates have to be able to see and hear you. -Nama Desk No nown n Trial I Triat 2 Trial 3 Mis of fired crueible and lid ce) 35.500 2sGs crucible, lid, and hydrated salt g) 2. One must then repeat this to ensure accuracy. 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. It is also important to use a balance that is accurate to at least 0.01 grams in order to obtain precise measurements. 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. apparatus, the method of gravimetric analysis is used by heating up a hydrated salt sample over a, Sample Name: El Salvador Transfera few crystals of sodium sulfate decahydrate, Na2SO410H2O,into one watch glass, and anhydrous calcium chloride, CaCl2,into the other. Other salts such as anhydrous salt have no, water molecules; heat can easily remove the weak bonds that binds the water molecules to the, salt (Tro 92). Recording the mass of the zinc sulfate Hydrates are ionic compounds that contain water molecules as part of their crystal structure. 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. 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. Course Hero is not sponsored or endorsed by any college or university. the percent water in the hydrated salt be reported as being too high, too low, or However, if the oil was failed to be completely burnt off of the fired crucible Work in groups to design the experiment. heptahydrate sample then allowed us to calculate the average percent of water lost which came to some of these salts, the bonds between the water molecules and the salt itself breaks, resulting 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. Many water molecules are chemically bound to the ions of salt in its crystalline Mass of hydrated salt (g) Mass of anhydrous salt (g) = Mass of water lost (g) Leads the team in developing experimental procedures, Leads the team in analyzing the data and the experimental error, Responsible for writing the presentation of the proposal, Delivers the presentation to te instructor/TA and the rest of the class, First five items from yoursupplies list for this lab. calculations were made. Experiment 5 Report Sheet Percent Water in a Hydrated Salt Lab Sec. By using the, gravimetric analysis, the amount of water being lost in the hydrated salt can be figured out. Bunsen burner would have been incorrect. Relative standard deviation of H.O in hydrated salt (RSD) Data Analysis, D Show calculations on next page. Suppose the original sample is unknowingly contaminated with a second anhydrous salt.