Copper Chloride Hydrate Lab Report

Using a scoopula, add 5-6 grams of the hydrate into the dish and measure the mass of the hydrate and the dish

This purpose was reached. The water percentage in the hydrate was 52.3% and the number of water molecules in the hydrate was 7. This lab showed that a hydrate can have the water of hydration removed from the anhydrous solution by heating the original hydrate. This is important because during chemical reaction, the experimenter must know if an anhydrous solution is hygroscopic or not, to make sure to incorporate the water molecules that would be present during a reaction. For example, the hydrate sodium sulfate is used as a drying agent for removing traces of water from organic solutions, however, if the hydrate gets too hot, it will release water, and do the opposite effect than it was meant to do. The lab also showed that rounding measurements may produce the theoretical answer, but maybe no the true experimental

The wire reacted with the solution to yield copper; any remaining aluminum was dissolved with a few drops of 6M HNO3. Following the isolation of the copper, it was separated from the solution with a Büchner funnel and flask. A piece of filter paper was weighed, and its mass was recorded. Then, the filter paper was placed on the vacuum flask, which was turned on, and the copper solution was poured over it. The copper was also rinsed with 95% ethanol solution before being set on a paper towel to dry. Finally, one day after the previous step, the copper was weighed, and its mass recorded. The recorded masses were then used to determine the mass of copper, chlorine, and water in the unknown copper chloride hydrate. The resulting masses were used to find the formula of the unknown copper chloride hydrate according to CuxCly•nH2O.

Used stirring rods to completely remove copper from that wire. And then completed the removal of copper using 5 drops of 6M HCl, adding it onto copper. There will produced copper in a solution. Connected Buchner flask to the vacuum line and place filter paper in it to completely washed off the copper. Then, add 95% ethanol to copper and leave it for 1 min and turned section back for 5 mins. Measured mass of clean, dry watch glass. Transfer copper to watch glass and dry it under heat lamp for 20 mins, allowed it to cool to room temperature and then accurately determine its mass.

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.

The percent of water can be determined in a hydrate by first determining the mass of the hydrate Copper (II) Sulfate penta-hydrate. The substance will be a deep blue color when it is a hydrate. By heating the substance, water is evaporated, removing the water from the hydrate, making it anyhydrous through a simple decomposition reaction. Evaporation is completed when the substance turns from a blue to a white/ grey color. The mass of the water in a hydrate is determined by subtracting the mass of the hydrate from the mass of the anhydrate. The mass of the water is then divided by the mass of the hydrate, and multiplied by one hundred, resulting in the percent of water in the hydrate, which is 36.35%. The percent error is determined by subtracting

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

4. Allow the crucible to cool with the lid on. When cool, determine the mass of the crucible and lid with the dehydrated compound. 5. Examine and describe the anhydrous compound in the crucible.

Introduction: The purpose of this lab was to learn the proper techniques of roasting, smelting, and volumetric analysis to determine an unknown sample of copper mineral.

We then took the mass of the crucible and the hydrated staple which is 18.382 grams and the mass of dehydrated with the crucible is 18.243 grams. After that, we used the molar mass of water to find either the mass of copper or the mass of chlorine in the sample. We have done this by dissolving the sample in water, which gave us a result of green crystals changing into a bright greenish color containing copper and chloride ions. To the solution, we an aluminum metal wire and the aluminum reacted chemically changing into a darker color. The aluminum oxidized itself and the copper metal appeared on the wire with the reddish color of copper.

We used a bunsen burner to burn the hydrate off and took the mass of the hydrate to make sure it was all gone.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Results In the part 2 of the experiment conducted, another salt was used, called Calcium Chloride. Calcium chloride is created from the ionic bonds that form between calcium cations and chloride anions. Calcium ions have a charge of +2, while chloride ions have a charge of -1, thus making its structure like this: Table 2. The table shows the data obtained from the experimental set-up.

The first step of the experiment is to make sure the crucible and cover are clean by washing them off with water. To dry the equipment place on the clay triangle and leave in the hottest part of the flame for 3 mins. Once time is up, allow the crucible to cool. Once cooled, measure the mass of the crucible with the scale. The next step would be to break the 10cm magnesium ribbon into small pieces, and place these pieces in the crucible. Find the mass of the crucible and the contents. Place the cover on the crucible and lay on the clay triangle. Heat the crucible and contents gently for 2 minutes. After this time is up, tilt the cover to provide and air opening. Tilt the cover using the crucible tongs. Now, heat the crucible and contents strongly

12. The crocodile clips are attached to the copper electrodes of the experimental apparatus and the power supply is turned on. Simultaneously, the stopclock is started. The thermometer is checked every 30s. 13. After 300s the stopclock is stopped and the power supply is turned off. The negative cathode is carefully removed and is dried using a hair dryer. 14. When dry the negative cathode is placed on the electronic milligram balance and its final mass is recorded. 15. The positive anode and negative anode of the experimental apparatus are disposed and the electrolyte is poured out to ensure that the anode slime (impurities) does not contaminate the solution. 16. The electrodes of the experimental apparatus are replaced with new copper strips. 17. Steps 7 to 16 are repeated. However, this time, the rheostat is adjusted using the calibration apparatus until the multimeter shows approximate readings of 0.40 A, 0.60 A, 0.80 A and 1.00 A respectively. 18. Time permitting, the entire experiment is repeated. Safety Copper sulphate may cause irritation and burns if it comes into contact with the eyes. As standard lab procedure, safety goggles and lab coats must be worn at all times. Control of Variables Volume of Electrolyte Used