Lab: Dehydration of an Inorganic Salt
Hydrates are a type of compound that contains water integrated into its solid crystalline structure. In most cases the water can be liberated by heating. In this lab, you will be analyzing the composition of a hydrate by determining the ratio of water to salt. By weighing a sample before and after heating, the mass of water incorporated in the hydrate can be determined.


View tje Dehydration of an Inorganic Salt Hydrate power point. This will provide you with the necessary foundation for safely and successfully completing the lab.



Note:While you work on the lab,you are required to take certain images/photos of your labto document that you actually completed the lab yourself. Each photo should include anote card or a piece of paper with your name, the date you completed the experiment and your course section numberclearly visible.

Note Card Information:

My Name: Zack Aldawoody

Section Number:145454

Download the item:Dehydration of an Inorganic Salt Hydrate
Report attached below. This is what you will submit for grading. You can type your results and insert your images into this document. To be successful, you should open the file, save it to your computer with[your last name] Dehydration of Salt Lab.

Dehydration of an Inorganic Salt Hydrate: Lab Report General Pre-Lab Question (1 point) 1. The reaction below shows the decomposition of calcium carbonate when heated. CaCO3 (s) → CaO (s) + CO2 (g) When 10.00 grams of calcium carbonate are heated, the mass decreases by 4.40 grams. What mass of calcium oxide is produced? Click or tap here to enter text. What mass of carbon dioxide is produced? Click or tap here to enter text. Activity 1 Calculations (3 points) On a clean sheet of paper, clearly show the following 6 calculations using your data for Sample 1. Write your name and today’s date on it. Take a photo of it and insert the image below. (See example calculations on Pages 4 and 5 of the Investigation Manual.) 1. Epsom salt, original (hydrated) mass calculation 2. Epsom salt, heated (dehydrated) mass calculation 3. Mass of Water calculation 4. Moles of magnesium sulfate calculation 5. Moles of water calculation 6. Ratio of moles of water to moles of magnesium sulfate (round to nearest whole number) calculation Repeat the calculations for Samples 2 and 3, but you do not need to take pictures of these. Enter the data for all the calculations, samples 1,2 & 3 into the Data Table below. Data Table (3 points) Complete the table below with the measured (in bold) and calculated values (*) for each trial. Sample 1 2 3 Mass of aluminum dish 0.000.000.00 Mass of aluminum dish + Epsom salt 0.000.000.00 Epsom salt, original (hydrated) mass* 0.000.000.00 Mass of aluminum dish + Epsom salt after heating 0.000.000.00 Epsom salt, heated (dehydrated) mass* 0.000.000.00 Mass of water* 0.000.000.00 Moles of magnesium sulfate* 0.0000000.0000000.000000 Moles of water* 0.0000000.0000000.000000 Ratio of moles water: moles of magnesium sulfate* 0:1 0:1 0:1 Post-Lab Questions (1.5 points) 1. Write the correct formula for your experimentally determined hydrate of magnesium sulfate. Click or tap here to enter text. 2. Write the experimentally determined balanced equation for the dehydration of Epsom salt. Click or tap here to enter text. 3. Using your data from Sample 3, determine the mass percentage by weight of water in Epsom salt. % water by mass = Click or tap here to enter text. Images (1.5 points) A required part of this laboratory experiment is to capture pictures of the experimental process and results. Click on the icon in each of the boxes below to include the required images for this lab. Remember to include a card with your name, the correct date and the section number in each image. Note: Failure to submit these images with the identifying card as required will result in a grade of zero for this lab. Review the Inserting Images into a Worksheet tutorial for further instructions. Empty aluminum dish #1 with balance reading visible (Step 2) Aluminum dish #1 with Epsom salt before heating with balance reading visible (Step 3) Aluminum dish #1 with Epsom salt AFTER heating with balance reading visible (Step 14) Introduction to Graphing Dehydration of an Inorganic Salt Hydrate Laboratory CHEMISTRY 111 Overview •Review the basic mole concept ideas & the relationship to the coefficient in the formula for a hydrate. •Determine the empirical formula of salt to water for an inorganic hydrate. •Demonstrate how to balance the equation for the decomposition of a hydrate. Materials Needed Printed materials and needed from the kit: ◦ Printed Investigation Manual ◦ Printed Lab Report ◦ Safety goggles ◦ Gloves ◦ Electronic balance ◦ Forceps ◦ Plastic spoon ◦ Epsom Salt ◦ Wire Stand ◦ Aluminum weighing dish (3) ◦ Sterno can Materials Needed Needed but not supplied with the kit: ◦ Matches or lighter ◦ Marker or pen ◦ Oven mitt or tongs ◦ Trivet or cooling rack to place under Sterno can ( or use a heat-proof surface!) Prior to the Lab/Safety •Carefully review the entire Investigation Manual, including the Overview and Objectives, Background information, necessary materials, safety precautions, lab preparation and procedures for all activities, and the waste disposal and clean-up information. •Make sure your work area is clean and out of the reach of pets and children. •Put your safety goggles on, and be sure to leave them on for the entire experimental procedure. Special Safety Precautions •The Sterno gel is flammable. Keep long hair tied back and loose clothing away from the open flame. •The Sterno can will stay hot even after the flame is extinguished. Use the Sterno on a heat- resistant surface like a stovetop or trivet. •To extinguish the flame, use tongs or an oven mitt to place the cover back on the can of Sterno. •Keep other flammable household materials away from the work area. •Do not leave the flame unattended! Hydrates •When the oppositely charged ions of some salt compounds pack together in a complex crystal lattice, the three-dimensional array of residual open spaces in the solid structure can be occupied by individual water molecules, loosely held by dipole interactions with the surrounding ions. •The resulting solid thus has a formula with a specific mole ratio of water to ionic formula units and is referred to as a “hydrate”. The general formula for a hydrate is shown as MaXb· n H2O, where the “dot” indicates the weak bonding interaction that holds the water in the crystal lattice and the value of n shows the mole ratio of water. •A specific example of this type of compound is copper (II) sulfate pentahydrate, which has the formula CuSO4·5H2O, and has a characteristic blue color. If this hydrate is heated moderately, the loosely held water can be driven off, leaving “anhydrous” copper (II) sulfate, a white solid. •The loss of loosely-held water molecules on moderate heating is a common property of hydrate compounds and the mass lost versus the mass of the anhydrous residue can be used to calculate the value of “n” in the hydrate formula. Activity 1 – Lab Tips Be sure to label the aluminum dishes BEFORE weighing. The amount of Epsom salt in each dish does not need to be the same. Be sure to record all mass measurements to two places after the decimal. 0.3 to 0.8 grams is not very much material – be aware! You may use a plastic spoon from the kit to deliver the salt to the dish. Once lit, the Sterno can will burn for about 45 minutes, so make sure you have all 3 samples ready for heating before you light the can. Use the forceps or tongs to move the aluminum dishes as they will become very hot. Activity 1 – Lab Tips •After ALL THREE samples have been heated, allow the Sterno can to burn to completion and then cool for disposal. •Do not leave the flame unattended! •Follow the calculations on pages 4 and 5, but use MgSO4 in place of CuSO4. Images/Photos As you complete this lab, please capture images of the following steps of the lab procedure to include in your submitted lab report. • Image 1: Empty Aluminum Dish #1 on the balance with balance readout visible (See Page 8, Step 2). • Image 2: Aluminum Dish #1 with Epsom Salt on the balance with balance readout visible (See Page 8, Step 3). • Image 3: Cooled Aluminum Dish #1 AFTER HEATING on the balance with balance readout visible (See Page 9, Step 14). For each image you capture, include a card with your name, the appropriate date and section number written on it. This card must be visible in each image you submit with your lab report. Failure to include these images or the card with the image will result in a grade of zero for the submitted lab. Clean Up •Allow all of the equipment to cool and dispose the materials in accordance with the directions from Carolina. •Clean and dry all equipment used. •Place your equipment and supplies back into their safe storage location until you need them again. •Clean and disinfect all surfaces used. •Thoroughly wash your hands. Calculation Help Recognize that the mass loss on heating is the mass of water initially in the sample. The percent of water in your initial sample. (Mass of Water/Mass of the Original Hydrate Sample) x 100% Recognize that the residue after heating is the anhydrous salt. Determine the mass of 1 mole of either MgSO4 or ZnSO4 (? below) and perform the following calculation.) Mass of Residue x (1mol/ ? grams) Recognize that the mass lost on heating is the mass of water initially present in your sample. (1 mole water = 18.02 grams) Mass of water x (1mol/ 18.02 g)