If copper (II) sulfate when mixed with sodium carbonate at different quantities combine to form ions in definite ratios.…
| [Solubility Product Constant] | Experiment 11 | | Molly McCabe | 4/18/2013 | | Data Tables: Part 1 and Part 2 Experimental Data: Standard | Calculated volume of copper sulfate in standards | Absorbance values | Blank | 0.0 mL | 0.0 | 1 | 1.25 mL | 0.094 | 2 | 3.75 mL | 0.065 | 3 | 2.50 mL | 0.099 | 4 | 3.50 mL | 0.129 | 5 | 5.00 mL | 0.187 | Collected Data | Test tube 1 | Test tube 2 | Test tube 3 | Test tube 4 | Test Tube 5 |…
When hydrates are heated, the water of hydration evaporates and is released as vapor. The remaining solid is known as the anhydrous salt, which is the compound same compound without the water molecules trapped inside.…
| The iron bits turn from a darkish gray to a reddish-mud color. The blue of the copper solution turns lighter.…
This left us with the silver and chlorine which yield us silver chloride which is a solid. We did note on our observation that we had a change in color and a solid precipitate.…
Driving Question: What compound is formed when you add 7 g of CuSO4 to 2 g of Fe?…
The objective of this experiment was to identify the unknown pure copper salt compound of #9. To do this, the mass of copper in the unknown was calculated and then divided by the mass of the whole compound to get the percent copper. The molecular weight was also calculated by dividing mass of copper compound used by moles of compound in unknown sample. The percent copper averaged out to 31.6% while the molecular weight of the sample averaged out to 201.1mw. In conclusion, the unknown compound of pure copper salt was close to Cu(C2H3O2)2 •H2O which has a percent copper of 31.8% and a molecular weight of 199.654mw.…
In order to find the formula of the copper chloride hydrate, we had to separate the compound to find the mass of water and copper. To begin this process, we evaporated the water and created an anhydrous compound, meaning we were left with only CuxCly. By calculating the weight of both the anhydrous and the hydrated compounds, we could conclude that the difference in the weights was the weight of the H2O. From this we were able to calculate the percent composition of CuxCly and H2O (see Calculations: Part I: Dehydration of Hydrated Copper Chloride), which showed how much of the compound was copper chloride by mass. Since there are only two stable forms of copper chloride, we concluded that possible formulas would be either CuCl or CuCl2. Intending…
A sample of copper sulfate pentahydrate (6.285g) was weighed out. The copper sulfate pentahydrate was dissolved in water (11.99mL) in a 250mL beaker. The solution was heated on a hot plate to 90 degrees Celsius. A sample of potassium oxalate monohydrate (10.006g) was dissolved in water (50.0mL).…
A hydrate is a substance that holds water in a certain ratio. As Hydrates are compounds with constant composition, we were able to easily determine this ratio by evaporating the water and then calculating a common ratio. We had Copper sulfate pentahydrous. In our experiment and on further calculations we observed that generally ten molecules of water combine with one molecule of…
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.…
By calculating the difference in the mass of the hydrate copper (II) sulfate and the anhydride we were able to determine the mass of water in the hydrate. This information was then used to determine the empirical formula of the hydrate, defined as a compound formed by the addition of water to another molecule. In the first trial, the mass of water in the hydrate was determined to be 0.41 g, while in the second trial the mass of water was 0.52 g. Moles of water associated with a single mole of anhydride were then calculated for both trials, giving the values of 4.7 and 4.5 moles of water, respectively. This indicated that the empirical formula of the hydrate might be copper (II) sulfate pentahydrate – CuSO4·5H2O.…
while the copper was in the ionic state. The solid copper may have been lost in…
CuO (s, black) + 2 H3O+ (aq) + 3 H2O (l) → [Cu(H2O)6]2+ (aq, blue)…
One is that when a hydrate is heated up, it will change colors indicating that there is a reaction occurring. Also, that the color change is a physical change since the anhydrous Copper (II) Sulfate could be hydrated again by adding water. When the water is added back to the compound, heat is released and it sizzles as it re-hydrates. Another thing I learned was that you could evaporate the water in a compound to make it an anhydrous compound. Lastly that the hydrate is chemically bound to the Copper (II) Sulfate, but it can be separated with…