The same process was followed using magnesium and Barium but the Barium had to be done in a fume cupboard and pH value and other observations were recorded.
Experiment 2: Reaction of the oxides with water and acid
Equipments:
Test tubes
Spatula
Chemicals:
Magnesium oxide
Calcium oxide
Barium oxide
Universal indicator solution
Hydrochloric acid
A spatula was used to transfer a very small quantity of the three oxides into separate test tubes. The test tubes were shaken after one-third of water was added in it. Observations were recorded. A few drops of universal indicator solution were added into the three test tubes. Any observations were recorded. Hydrochloric acid was added drop by drop to each of the three test tubes. After every drop, the test tubes were shaken in order to enable the solution to mix properly. The colour changes were recoded.
The experiment with Barium oxide was still completed in the fume cupboard.
Experiment 3: Solubility’s of the hydroxides and carbonates
Equipments:
Test tubes
Disposable pipette
Chemicals:
Magnesium nitrate solution
Calcium nitrate solution
Barium nitrate solution
Sodium hydroxide solution
Sodium carbonate solution
About 1 cm depth of magnesium nitrate solution was poured into two test tubes. One of the test tubes was added. An equal volume of sodium hydroxide solution and the same quantity of sodium carbonate solution was added to the other test tube. Both test tubes were shaken and the observation was recorded.
The same procedures were applied to Calcium nitrate solution and Barium nitrate solution but the Barium nitrate solution experiment was done in the fume cupboard. Observations were recoded.
Experiment 4 Thermal stabilities of the carbonates
Equipment:
Test tubes
Bunsen burner
Vent-plug
Beaker
Spatula
Chemicals:
Lime water
Magnesium carbonate
Calcium carbonate
Barium carbonate
About a 0.5 cm depth of solid magnesium carbonate was placed in a test tube using a spatula and the equipment was set up as in the diagram below:
A Bunsen burner was used to heat the test tube. The Bunsen burner was first set as a moderate flame to heat the test tube for a few minutes and then changed to a roaring flame if nothing happened. The observation was recorded.
After the experiment, the Bunsen burner was first removed otherwise the limewater would have been sucked back into the test tube, which would result in the glass test tube shattering.
The experiment using Calcium carbonate and Barium carbonate were done in the same way as the magnesium carbonate but the Barium carbonate was used in the fume cupboard.
After all the experiments had been completed all the used chemicals were placed into labeled container especially the Barium compounds. All the glassware equipments were rinsed out and left to the original places.
Results
Experiment1: reaction of the metals with water
These three elements all reacted with water. As the electron shells increased the reaction was more active.
The equations for the reactions were:
Mg (s) + H2O (l) MgO (s) + H2 (g)
Ca (s) + H2O (l) CaO (s) + H2 (g)
Ba (s) + H2O (l) BaO (s) + H2 (g)
[3]
Experiment 2: Reaction of the oxides with water and acid
All these three oxides reacted with acid and all were neutralized. The pH values were around pH11 when dissolved. Forming cloudy solution when water was added.
The equations of these reactions were:
MgO (s) + 2HCl (aq) MgCl2 (aq) + H2 (g)
CaO (s) + 2HCl (aq) CaCl2 (aq) + H2 (g)
BaO (s) + 2 HCl (aq) BaCl2 (aq) + H2 (g)
[3]
Experiment 3: Solubility’s of the hydroxides and carbonates
All three solutions were increasingly soluble in hydroxide but increasingly insoluble in carbonate.
The balanced equations for the reactions were:
For hydroxide:
Mg(NO3)2 (a.q) + 2 NaOH(a.q) Mg(OH)2 (s) +2 NaNO3 (a.q)
Ca(NO3)2(a.q) + NaOH (a.q) Ca(OH)2(aq) + 2NaNO3(a.q)
Ba(NO3)2(a.q) + NaOH (a.q) Ba(OH)2(aq) + 2NaNO3(a.q)
For carbonate
Mg(NO3)2 (a.q) + Na2CO3 (a.q) MgCO3(aq) + 2NaNO3(a.q)
Ca(NO3)2 (a.q) + Na2CO3 (a.q) CaCO3(s) + 2NaNO3(a.q)
Ba(NO3)2 (a.q) + Na2CO3 (a.q) BaCO3(s) + 2NaNO3(a.q)
Experiment 4: Thermal stabilities of the carbonates
Sequence of the thermal stabilities of the carbonates:
Mg
Ca
Less stable
This experiment didn’t use Barium due to its toxicity and the thermal stability could be predicted, which was less stable than calcium.
The thermal stabilities of the elements decreased as went down the group in the Periodic Table.
The general equation of a carbonate:
XCO3 (s) heat XO(s) + CO2 (g) [3]
The carbonate was decomposed into oxides and carbon dioxide. Carbon dioxide could be detected by lime water.
Lime water (i.e. calcium hydroxide) was used to test the carbon dioxide and the precipitate would produce to prove the existence of carbon dioxide.
Reaction of the lime water
Ca(OH)2 (aq) + CO2(g) CaCO3(s) + H2O (l)
Discussion
In experiment 4, there was a procedure to detect carbon dioxide by using lime water. Lime water was expected to become turbid once carbon dioxide was produced but in the experiment the lime water did not become turbid at all, this may be because the heating time was too short to enable the air in the test tube to come out. In addition, It also may be because there was not enough or no CO2 produced or there was something wrong with the lime water. Perhaps it was old. [7] To solve this problem, we could use fresher lime water or placed more substances in the test tube to enable there were enough CO2 to come out react with lime water and make it turbid.
Therefore, trends in the properties of alkaline earth metals and their compounds could be concluded as follow:
[3]
Reference
[1] ( Apr. 2008)
[2] The Chemistry of Group II Metals Handout from Michele Raychaudhuri. 1. Apr.2008
[3] Lewis. R. and Evans. W. 2006. Chemistry.Page197. 3rd edition. Palgrave Macmillan. New York.
[4] http://en.wikipedia.org/wiki/Magnesium#Biology ( Apr. 2008)
[5] http://en.wikipedia.org/wiki/Calcium#Applications ( Apr. 2008)
[6] http://en.wikipedia.org/wiki/Barium ( Apr. 2008)
[7] From Michele Raychaudhuri. Mon, April 7, 2008 8:58 am
