During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the
The solution had an opaque image, meaning if you were to look through the mixture you would only see a light blue liquid, thus the solution was not transparent. Furthermore, the solution from the Copper Chloride and Water dissolved together had demonstrated one solid colour- thus the light blue colour from the solution was spread evenly through the beaker and no other particles were visibly seen.
The main objective of this experiment is to differentiate between a physical change and a chemical change.
either barium (Ba 2+ ) or calcium (Ca 2+ ). Part C consisted of a series of cation flame tests using metal
When the zinc was dropped in the hydrochloric acid, the substance began bubbling vigorously, forming a precipitate. Eventually, the zinc dissolved completely. After the lit wooden splint broke the surface of the test tube, there was a loud popping noise. The gas that was released was hydrogen from the acid and the popping noise was a result of the Hydrogen being burned up by the fire creating a small explosion. Two chemical changes occurred in this test: one with the formation of a precipitate (a textbook sign of a chemical change), and the other when the explosion
Product bubbled upon addition to the hydrochloric acid; liquid turned cloudy ¡V precipitate was present; zinc sample disintegrated slowly and turned black in color.
To tube 3 a piece of litmus paper was placed into the tube. Then as is tube 2 concentrated HCl was added drop wise until the litmus paper indicated that it is acidic. No CO2 gas will evolve.
was too fast to measure and so for my scale to reach above that, I
This is a fair test because the only thing that is changed is the drop
At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.