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Traditional experimental methods
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Investigation to Determine the Relative Atomic Mass of Lithium
Introduction
My aim of this experiment will be to determine the R.A.M using two
separate methods
In the first method I will dissolve a piece of lithium of a known mass
in water, I will then collect the hydrogen gas produced, which can be
used to calculate the relative atomic mass of Lithium.
The balanced equation of our reaction is shown below;
[IMAGE]2Li + 2H2O 2LiOH + H2
In the second method I will do a titration experiment of lithium
hydroxide(produced in experiment 1)
The balanced equation of our reaction in experiment 2 is shown below;
[IMAGE]LiOH + HCl LiCl + H20
Background Information
Lithium is an alkali metal in group 1 of the periodic table. It is a
metallic element and does not decompose however it is highly in
contact with many other substances. It can react violently with water,
the humidity in air, and the moisture in other substances releasing
hydrogen gas.
[IMAGE]
Apparatus
* Lithium (0.1g)
* Pan Balance
* Conical Flask
* Bowl
* Measuring Cylinder (250cm3)
* Delivery tube and Bung
* Goggles
* Filter
* Clamp
Method
I set up the apparatus as shown above. I placed water into the bowl (I
used a big bowl because the measuring cylinder was 250cm3 which was
too big to fit into a beaker). I made sure their were no air in the
measuring cylinder and that it only contains water and I put it into
the bowl of water over the delivery tube, I then got a clamp stand to
hold the measuring cylinder
The lithium was taken and the oil was removed off it using the filter.
The lithium was then placed in a pan balance once removing as much oil
as possible. The measured mass of lithium was placed in a conical
2. Drop a gummy bear into each of your prepared beaker or cup and place the beaker or cup
Next, making sure that the stopcock of the buret is closed, use a buret funnel to add 5-10mL of NaOH to the buret to rinse it. Drain all of the NaOH into the waste beaker by opening the stopcock. Rinse the buret in the same manner two more times.
10. Point the flask away from everyone and open the two-way valve in order to release pressure from the flask. Remove the stopper assembly, then fill up the flask with water. Discard of the solution in the sink.
Lithium has an atomic number of 3, and an atomic weight of 6.94. In general, lithium is more stable than hydrogen, and slightly less stable than nitrogen, carbon, and oxygen. When looking at chemical ion properties, it is useful to consider three main characteristics: the size, or radius, of the ion, the charge, and the ion's electron affinity. Lithium has a similar charge to radius ratio to that of magnesium, which is in group IIA of the periodic table, and so chemists say that the two elements are "chemically similar.
4. Pour about 300mL of tap water into the beaker. Set up a hot-water bath using a hot plate, retort stand, and thermometer clamp. Alternatively, use a Bunsen burner, retort stand, ring clamp, thermometer clamp, and wire gauze.
The first step that we took to accomplish our goal was to put on our safety goggles and choose a lab station to work at. We received one 400ml beaker, one polyethylene pipet, two test tubes with hole rubber stoppers, two small pieces of magnesium (Mg), one thermometer and a vial of hydrochloric acid (HCl). We took the 400ml beaker and filled it about 2/3 full of water (H20) that was 18 OC. Then we measured our pieces of Mg at 1.5 cm and determined that their mass was 1.36*10-2 g. We filled the pipet 2/3 full of HCl and poured it into one of the test tubes. Then, we covered the HCl with just enough H2O so that no H2O would be displaced when the stopper was inserted. After inserting the stopper, we placed the Mg strip into the hole, inverted the test tube and placed it in the 400ml beaker. HCl is heavier than H2O, so it floated from the tube, into the bottom of the beaker, reacting with the Mg along the way to produce hydrogen gas (H2). We then measured the volume of the H2, cleaned up our equipment and performed the experiment a second time.
Now, assemble and arrange all of the needed supplies so that they are easily accessible. Connect the IV tubing to the solution bag and allow the fluid in the bag to run through the entire length of the tubing, also known as priming the tubing. When this is done, clamp the tubing closed. You will then need to tear several pieces of tape, six to eight inche...
I am going to carry out an experiment to measure the change in mass of
Determining the Relative Atomic Mass of Lithium An experiment has been carried out to determine the relative atomic mass of Lithium by using two different types of methods The first method that was carried out was to determine the volume of Hydrogen produced. In this experiment a fixed amount of Lithium was used, in my case it was 0.11g. At the end of this experiment, the volume of Hydrogen gas I collected was 185cm³. Then using the solution of lithium hydroxide made from experiment one, I used it in the titrating experiment, to find out the total volume of Hydrochloric acid used to titrate the lithium hydroxide. RESULTS TABLE Experiment Initial Volume ( cm³) Final Volume ( cm³) Total volume Of HCl used ( cm³) Rough 0.2 30.3 30.1 1 6.3 35.8 29.5 2 2.7 32.0 29.3 Average 29.6 CONCLUSION Method 1 [IMAGE]2Li (s) + 2H20(l) LiOH(aq) + H2(g) Number of moles of Hydrogen. Volume of hydrogen gas was 185 cm³. Weight of Lithium was 0.11g. N = __V__ _185_ = 0.0077 MOLES 24000 24000 Number of moles of Lithium.
Rinse your beaker thoroughly to wash any excess powder. 12. Repeat steps 7-11 3 more times for reliability. To make sure the temperature still stays hot by continue heating the water a little bit using the hot plate. 13.
Sodium is an element on the periodic table with the chemical symbol as Na. Sodium, discovered by the English Chemist Sir Humphry Davy, is in the Alkali Metals group on the Periodic Table and it is a soft, silver/white color. Sodium, which is found in the Earth's crust, is important to society.
From the Greek word "lithos" meaning "stone", it was so named due to the fact that it was discovered from a mineral source; whereas the other two common Group 1 elements, Sodium and Potassium, were found in plant sources. Its symbol, Li, was taken directly from its name. Soon after stumbling upon Lithium, Arfvedson also found traces of the metal in the minerals Spodumene and Lepidolite. In 1818, C.G. Gmelin discovered that Lithium salts color flames a bright red. Neither, Gmelin or Arfvedson, however, were able to isolate the element itself from the Lithium salts. They both tried to reduce the oxide by heating it with Iron or Carbon, but neither met with the success of W.T. Brande and Sir Humphrey Davy. They managed to perform the first isolation of elemental Lithium by the electrolysis of Lithium oxide. Electrolysis is a chemical reaction, which is brought about by the passage of current from an external energy source such as a battery. In 1855, the scientists Bunsen and Mattiessen isolated larger quantities of the metal by electrolysis of Lithium chloride.
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
Remove the extra solvent on a steam bath under a hood while flushing the flask with N2 gas, leaving the crude extract. Weigh extract.
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).