Procedure: A. Reaction between the elements copper and sulfur To begin the lab, a 5 cm copper wire was obtained and observed. Properties such as luster, malleability, and color were noted. Then, a pencil was used to make a small coil by wrapping the copper wire against it. The coil was placed in a crucible afterwards. Sufficient powder sulfur was added in. The crucible was then covered and conscientiously placed upon a clay triangle on an iron ring. Next, the crucible was heated with the hottest part of flame at the bottom of it. This was to get a red color to appear at the bottom of the crucible. The heating was continued until there was no sign of smoke occurring. Using tongs, the crucible was removed from the clay triangle without extracting …show more content…
2 mL of 6 moles of HCl was then incorporated into the test tube. Information was recorded. Using another clean test tube, an inch piece of Copper wire was placed inside along with the addition of 2 mL of 6 moles of HCl. After information was documented, a new test tube was obtained and an inch copper wire was placed inside. Then, 1 mL of concentrated nitric acid, HNO3, was added and observations were noted. After that, 1 mL of 0.1 mole of Sodium Oxalate was placed in a clean test tube. An addition of 10 drops of 6 moles of Sulfuric acid was mixed in. Afterwards, 1-2 drops of 0.1 mole of KMnO4 was added in and stirred. Information was recorded on data. Then, a 3 mL of 0.1 mole of sodium hydroxide solution was added and stirred. A drop of 0.1 mole of KMnO4 was placed inside and observations were made. Finally, 2 crystals of potassium permanganate were added to 1 mL of 6 moles of HCl in a test tube and information was recorded once again on …show more content…
Several drops of 6 moles of HCl were mixed in and observations were made of the changes. Then, the process was repeated and recorded with Sodium sulfite and Zinc Sulfide. Afterwards, 1 mL of 0.1 mole of lead nitrate had been placed in a test tube. A few drops of 6 moles of HCl was then added into 1 mL of 0.1 mole of Barium chloride solution, 2 drops of 1 mole of K2CrO4 were added. Information was noted down. To 1 mL of Barium chloride of another test tube, several drops of 3 moles of ammonium carbonate was added. Information was recorded when changes occurred. After precipitate has settled, the excess liquid was carefully poured out. 1 mL of water was then added to a test tube. it was shaken and allowed to let precipitate to settle down. The final steps included the liquid was poured out and several drops of 6 moles of HCl had been added to the remaining solid. Observations were
Reaction 3- 1. Obtained a clean and dry test tube and placed a small amount ( about the size of a jelly bean) of ammonium carbonate into the test tube.
As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.
The main objective of this experiment is to differentiate between a physical change and a chemical change.
***Repeat steps 2-4 for each of the following: 5 mL of oil and 2 g each of cornstarch, sodium chloride, and sodium bicarbonate.
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.
In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor
Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.
We only added a small amount of HCl to the water and sodium chloride. We did not continue to add more HCl after a significant drop in pH was recorded. We added a total of 2 mL of HCl to both H20 and NaCl before the pH changed. The 1 gram solution of sodium acetate and acetic acid changed after a 8 mL, and the other two never dropped before we reached our total of 10 mL HCl.
Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, 1M NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9, ammonia which was identified by its pungent odor, was added, an inky dark blue color was made. Iron (Fe (NO3)3) was determined to be in test tube K-2. KSCN was found in test tube K-11 since Fe (NO3)3 and KSCN makes a bloody color when mixed together. Flame tests were conducted in which K-8
The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once
Copper wire turned white when submerged in distilled water, little crystal-like substances forming on copper
|1. Copper metal (penny) at the start |Tarnished, worn out, brownish, copper-colored, fine solid. |
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:-
Electrolysis of copper sulfate has great importance in the mining industry as it is a better metal extraction process compared to simply mining the ore from the rocks. This is because electrolysis refines copper so that the copper is high quality and removes the impurities of it. This is particularly important for the copper to be used in industrial processes. (1) Copper is used in industry to make electrical wiring and components due to copper being a very good conductor of electricity. Electrolysis is the process where an electric current is passed through ionic substances causing them to break down into simpler substances.
The reaction characteristics of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite (Cu_2 Cl(OH)_3 ), beside alkali copper carbonate, was formed because of incomplete reaction at a copper content of 53.9 wt%. Lack of sodium carbonate may cause incomplete reaction with copper chloride (II) because of low pH (6.0) of the solution [12]. The copper content according to the reaction mole ratio were 57.7, 50.5, 58.8, 59.3, and 59.8 wt% at the reaction mole ratios of 1.20, 1.32, 1.44, 1.56, and 1.68, respectively.