Comparing Magnesium, Sulfate And Hydrochloric Acid

b) Iron and Barium were present in unknown 3. Assigned unknown reacted with all 4 reactants and formed precipitate with 3 of them (Sodium carbonate, sodium hydroxide and Sulfuric acid). During the experiment it reacted very similarly to Iron (III) nitrate and Barium nitrate. For example, with it was tested against Ammonium Chloride, the color of the solution changed to a light green, very identically to Iron (III) nitrate and Ammonium Chloride. Besides, unknown 3 formed an orange brownish precipitate when it was tested with sodium carbonate. Iron (III) nitrate acted similarly. Moreover, unknown 3 reacted similar to Barium nitrate when it was tested against ammonium chloride and sulfuric acid. It did not form any precipitate with ammonium chloride but formed a very light white precipitate, which is identical to barium nitrate’s reaction against sulfuric acid. Therefore, the two present metal in unknown 3 are Iron and barium.

Chemical changes occurred in five out of the eight experiments completed in this lab. Although the main focus of experiment two was

this experiment had a similar scenario to part A except the metals were switched and replaced with

The type of reaction that occurs through reaction A through E is a chemical reaction. InReaction A, a redox reaction (oxidation-reduction) occurred. Copper metal reacted withnitric acid to produce copper (II) nitrate. It also created nitrogen dioxide, and water (which isdecomposed from nitric acid). In reaction B, a double displacement reaction occurred forthe reasons that when copper (II) nitrate reacts with sodium hydroxide, copper and sodiumdisplace each other to create copper (II) hydroxide and sodium nitrate.

The results of all the trials are in an attached document entitled "Results of all Trials". While observing our data, we noticed that the results of all the trials were pretty consistent and that the overall amount of a particular material reduced as time passed. Pectin Powder Test Results: Graph "Copper Testing Results" shows the copper levels in experiment 1 (Pectin Powder) after 30, 60, 90, and 120 minutes when purified with pectin powder. After 30 minutes, the pectin powder had reduced the copper concentration from 500 milligrams to approximately 352 milligrams.

Despite the results obtained were correct and proved that the experiment was a success a few variables emerged during the performance of the experiment that if improved could result to a more accurate result. We didn’t have enough time to do this experiment over and over again so we didn’t have enough results to compare. Another important factor that may have influenced in our experiment was the quantity taken of the lead nitrate. We didn’t have any colorimeter so our result might not be

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

The two experiments were, for the first experiment the group did the Magnesium and Hydrochloric acid (Mg and HCl)

The hyphotesis created for this experiement was accurate. Each element received a different reaction for each of the tests. No test had a similar outcome for both Iron or Sulfur. The reaction always proved to be quite different and even the oposite. Iron reacted to magnet, mixed with the substances while Sulfur did not react with the magnet nor did it mix with either water or M Hydrochloric Acid. This experient however could have had a couple of mistakes. The measurments werent exact ones. It would be impossible to do so everytime and the amount of substance or elements would always be a little off.

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.

After doing the experiment I realised a couple of things. For example that we could have done better testing, we could have done the experiment multiple times to make sure we are getting the same answer and ask teacher for help. As we couldn’t ask our teacher for help some of our answers maybe really different to others but we had to go with what results we already had. Conclusion I observed all of the test substance’s results after doing each one.

Magnesium + sulphuric acid → magnesium sulphate + hydrogen Mg + H2SO4 → MgSO4 + H2 Metal hydrogen carbonates and acids is also a common reaction. In this case, metal hydrogen carbonates are reacted with acids; this produces water, salt and carbon dioxide. A common example occurs between sodium hydrogen carbonate and hydrochloric acid, which react to form water, carbon dioxide and sodium chloride (a salt).

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the

Can the concentration of hydrochloric acid increase the rate of the reaction between magnesium ribbon and hydrochloric acid?

When mixed with hydrochloric acid (appendix 4), they react violently, hence why only a small portion was allowed for this experiment. This supports the hypothesis, that is, it was predicted that such a reaction would occur as these metals are highly reactive, hence why the hydrogen gas produced was clearly visible (appendix 5). Tin is less reactive, however, according to the Metal Reactivity Series, reacts with acids at an extremely slow rate. This was evident in the experiment; however, more of a reaction would have occurred if the time frame was expanded. The metal was only left in the acid for five minutes; therefore, it had no reaction but could of, had it been left a while longer. Magnesium and Calcium are both alkaline earth metals which means that they all have an oxidation number of ‘+2’, making them highly reactive. Calcium is more reactive than Magnesium even though it is located below it on the periodic table (appendix 6) because its electron configuration is ‘2,8,8,2’ while Magnesium’s is ‘2,8,2’. This means that Calcium has more shells which, therefore, means that there is less of an attraction to the nucleus. This makes it easier for Calcium to lose electrons and react more so than Magnesium. According to the Metal Reactivity Series, in order from the most reactive to the least reactive, tin is located at around the middle of the