Hydrates Lab

The main goal of this experiment was to observe series of reactions that convert a piece of copper metal, via several different copper-containing compounds, back into its original elemental form. The data collected was the striking color changes along with their relevant chemical equations. The data was collected while keeping a close eye on the experiment the whole time. The data recorded was used to see the different changes involved with a piece of copper metal. The copper was weighed and heated multiple times throughout the experiment

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

Put approximately 9-10(g) copper ore into beaker. Use spatula to break up any large pieces. Next add 17ml H2SO4 (aq) (hydro sulfuric acid) to the beaker. Began mixing until all or most traces of blue dissipate; or the copper ore will no longer dissolve (should appear as a milky liquid). Next use pipette to and remove solution and divide solution into 2 individual test tubes then Place test tubes into centrifuge and run centrifuge for 1 minute. Remove from centrifuge machine Fill a cuvette with the clear solution from the test tube making sure not to disturb the sediment at the bottom. Note the solution should bluish in tint Final place the cuvette in the colorimeter. Then record data and calculate in results section.

Water was the added to the anhydrous compound in the crucible. Observations through the entire experiment were recorded along with data. The components of the experiment were cleaned up, and calculation followed. The data obtained was used to calculate: the moles of anhydrous salt, the moles of water removed from the sample, the ratio of moles of anhydrous salt versus the moles of water, the percent water in the hydrate, and the empirical formula of the hydrate. These calculated answers were then compared to the published answers.

xH2O was heated there was a colour change from blue to white, this is because the water was being removed because heat was added. Many compounds decompose when there heated, like this one this is why it is a decomposition reaction. The CuSO4 . 3H2O became CuSO4 + 3H2O the compound separated and became two separate compounds this is why this is a decomposition reaction. The crystals also changed form.

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).

In this experiment, by heating the hydrated copper (II) sulfate, the water molecules will evaporate and separate from the compound leaving behind an anhydrous solid compound, copper (II) sulfate.

To the solution that was set aside earlier, five drops of aqueous 1.0 molar sodium sulfate was added, producing a white precipitate from the aqua colored solution. The test tube was centrifuged for about one minute to separate the solid from the solution, which was saved for later in a clean test tube. The possible cation in the solid was

The objective of this experiment was to manipulate the state of copper by taking copper through four different forms and to observe and understand the method behind each reaction. The transformations include starting from 0.1588g of Copper(II) Chloride dihydrate to produce Copper(II) hydroxide. Copper(II) Chloride dihydrate was dissolved in water forming a light blue colour and Sodium hydroxide was added in order to form Copper(II) hydroxide a dark blue precipitate. In this reaction Sodium Chloride is soluble and Copper hydroxide is insoluble in water, therefore, forms precipitate. When the dark blue Copper(II) hydroxide was then, heated it decomposed to form Copper(II) Oxide, a black solid. Copper(II) oxide, an insoluble metal oxide, and sulfuric acid reacted to produced Copper(II) sulfate, a soluble salt and blue in colour. Copper(II) sulfate was

Substances differs from each other as each of the substances have different atomic composition and structures. And although the substances that shares the same characteristic can be grouped together, each of the substances still have their own unique and defining physical and chemical properties. Therefore, some substances may undergo a chemical change while others don’t during a same reaction. In the experiment conducted, two different elements were used, Iodine crystals, I2 and Copper wire, Cu. After recording the initial observation on both of the elements, they were both heated and allowed to cool.

The ratio of the moles of water to copper (II) was 4.77, rounded to 5, proving that copper (II) sulphate pentahydrate does in fact have a ratio of 5 water moles to 1 copper (II) sulphate mole. The hydrate salt copper (II) sulphate pentahydrate is composed of 65.00 % of copper (II) sulphate and 35.00% of water using the measured data. The composition using defined values is 36.08% water and 63.92% of copper (II) sulphate. There is a slight error between the values. One of the possible reasons could be the moisture of the atmosphere of the air, which prevented the water of the hydrate from fully evaporating. Though some bonds between the water molecules were broken and evaporated from the compound, the copper (II) sulphate may have formed bonds

To find the nature of each substance, the results from the practical were compared to the expected results for the possible substances given which were potassium chloride, sodium chloride, sucrose, glucose, sulfur, copper chloride and copper sulfate. Research was conducted to match these known substances to the unknown substances to determine whether they were covalent or ionic. From the results, it could be determined that substance 1 was copper sulfate with covalent bonds. Substance 2 was sulfur with covalent bonds. Substance 3 was copper chloride with ionic bonds. Substance 4 was sucrose with covalent bonds. Substance 5 was sodium chloride with ionic bonds. Substance 6 was potassium chloride with ionic bonds. Substance 9 was glucose with covalent bonds.

Gas hydrates (GHs) are compounds which are made up of water molecules and guest gas such as methane, carbon dioxide or hydrogen sulfide. GHs have a clathrate structure where the guest gas is trapped in the water molecules forming a cage. GHs appear to be solid like an ice but their physical properties differ from those of ice.

For this aim 3 sets of results will be obtained by timing how long it takes for the colour change to occur in different temperatures determined by the use of an electric water bath. With these results, the effect of temperature on the rate of reaction will be investigated.