The following laboratory experiment calls for a moderate understanding of what a hydrate is, what its properties are, and how altering a hydrate’s chemical structure may cause the release of both water and acidic vapors. A hydrate itself is a chemical, typically a crystalline salt, which incorporates water (H2O) into its chemical structure. For example, the compound CoCl2 is merely cobalt (II) chloride, however, take the original compound and attach a water molecule and it becomes CoCl2 + 6 H2O. In other words, the original cobalt (II) chloride is now cobalt (II) chloride hexahydrate.
The bond between the compounds and the water molecules is weak and therefore easily broken. Typically, these bonds are broken through the heating of the compound.
5. Zoom Out by clicking on the green arrow next to the Save button. Click on the Stockroom and then on the Clipboard and select Balloon Experiment N2. Again, set the temperature, pressure, and moles to 298 K, 1.00 atm, and 0.300 moles, respectively. You may have to click on the Units button to change some of the variables to the correct units. Repeat the experiment with this gas labeling the data link ‘Real Gas N2.’
Pre-Lab: A) Hydrate- a compound, typically a crystalline one, in which water molecules are chemically bound to another compound or an element. B) Water of hydration (crystallization)- water that is chemically combined with a substance to form a hydrate and can be expelled (as by heating) without essentially altering the composition of the substance. C) Dehydration- the loss or removal of water from something.
A hydrate is a compound that is bonded with a certain number of water molecules. When heated, the water will be driven out, thus being left with an anhydrate. The anhydrate is the hydrate minus the water. The hydrate must be
Introduction: The purpose of this lab will be to determine the percent water in an unknown hydrate, determine the moles of water present in each mole of the unknown substance, and to use the molecular mass to find the empirical formula of a hydrate. In this lab and unknown hydrate will be heated two separate times over a Bunsen burner to remove as much water from the substance as possible, before and after heating the crucible the masses will be calculated and recorded for future reference. To participate in this lab it is important to know he formulas that will be worked with. The formula of the hydrate that will be used, Copper II Sulfate, is CuSo4 • 5H2O. Along with this, the formula used to calculate the percent water in the hydrate will
The substance evolved some in the form of color, turning from blue to white, however it’s overall consistency remained the same, despite the difference in mass. Conversely, some substances such as Epsom salt, do not undergo such a drastic alteration during the transformation to an anhydrous state. Due to the transformation of the hydrated copper sulfate to its original color upon adding water, it can be concluded that some hydrates do possess the capability of being rehydrated after dehydration and vice versa. Yet other substances, like sugar, do not possess this capability due to the fact its overall structure was changed upon applying heat. Applying heat to sugar involves the removal of water and an overall breakdown of the substance. Once broken down, the sugar does not possess the capability of reverting back to its’ original granule state, so it is an irreversible
Performing Qualitative analysis: Small amount of above prepared solution of unknown hydrate was taken separately in different test tubes reacted with given known aqueous solutions and reagents. 1. Reaction with Sodium sulfate: Few drops of sodium sulphate were added to the test tube. White precipitates were formed. 2.
Fulfilling the purpose, after concluding this experiment, the formula of an unknown hydrate was able to be identified. In order to obtain the data needed to develop a response to the purpose, multiple measurements were collected. The mass of an evaporating dish was measured without copper (II) sulfate hydrate (before and after heating), then measured with copper (II) sulfate hydrate before heating and with anhydrous after heating. Initially, the mass of an evaporating dish was recorded, then the dish was heated and the mass was again recorded. Through this additional step of heating, it insured that no excess water remained in the dish which, as a result, would alter the data. Copper (II) sulfate hydrate was added to the dish and the mass was
A hydrate is a chemical compound containing salt and water. Depending on the salt, there is a maximum amount of water molecules that can be absorbed by the salt. An anhydrous salt is when the hydrate loses water, which happens when the hydrate is heated
After the whole set up is done we will switch on the lamps, measure the initial length of water and start the stopwatch after as we see 2 or 3 bubbles (which signify process has started).
1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow
An anhydrate is a compound in which all the water is released as vapor when the hydrate is heated.
The results of the experiment show that the mass of the hydrate decreases as the temperature increases. In the Hydrate Lab, this was found when every single time the hydrate was heated, the mass got lower, but slowly for this specific experiment. When it was heated, all the water was disappearing. This fact can also be defended when Weiner, Susan A., and Edward L Peters states, “Upon heating, the water can be evaporated leaving an anhydrous salt”(para.3). The purpose of this lab is to determine the percent composition of water in a hydrate and to calculate the number of moles of water found in the hydrated salt.
For this experiment we analyze the percent water in a crystalline hydrate. By examining the percentage we then are able to identify the changes in compound and compare them to that of unknown possibilities. In order to identify what hydrate we’re experimenting with, it must first be weighted using an analytical balance and record its initial state. To begin the heating process, the hydrate is moved back and forth over a flame at a 45 degree angle in order to remove any water within the hydrate. Thus it becomes a anhydrous residue after heat is applied. In order to achieve a constant weight of 0.002g or less, the anhydrous needs to be heated several times in order to eliminate most of the water contained. By calculating the the initial and final stage of the hydrate, the percent water will be determined. Finally, by comparing the mass of water lost from the unknown hydrate, the compound can be referenced from a list of unknowns.
The purpose of this experiment was to determine the percent by mass in a hydrated salt, as well as to learn to handle laboratory apparatus without touching it. The hydrated salt, calcium carbonate, was heated with high temperature to release water molecules. Gravimetric analysis was used in this experiment to determine the percent by mass of water in a hydrated salt. The hypothesis of this experiment was accepted on the basis that the percent by mass of volatile water in the hydrated salt would be fewer than 30%. The percent by mass was determined by the mass of water loss devised by the mass of hydrated salt multiplied by total capacity
Hydrate-based CO2 separation is a new technology by which the exhaust gas containing CO2 is exposed to water under high pressure forming hydrates. The mechanism is based on the differences of phase equilibrium. Gas hydrates are crystalline solids, in which low molecular weight guest molecules are trapped inside cages of hydrogen-bonded water molecule. A given hydrate structure is typically determined by the size and shape of the guest molecule. Carbon dioxide is known to form structure I.