Sodium Chlorine And Sodium Bromine Water Test

8 test tubes were then labelled A-H, 1ml of DCPIP was added to each of the test tubes. 2ml of NaHCO3 was added tubes A through G.

In the second part of the experiment, they took 3 test tubes, one containing a small amount of potassium chloride, one with a like amount of potassium chlorate, and one that contained a solution obtained from adding distilled water to the crucible, that was used in the first part of the experiment, and heated it for about a minute, and then they added 10 ml of distilled water to each and stirred. In each of the tubes, they added 5 drops of dilute (6 M) nitric acid and 5 drops of 0.1 M silver nitrate solution, then stirred each test tube and observed carefully.

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

Experimental Method: A filtration apparatus was set up. Solid iron(III) chloride hexahydrate was dissolved in water. In a separate container, sodium acetate trihydrate (NaC2H3O2 x 3 H2O) was also dissolved in water. Sodium acetate trihydrate was then added to iron(III) chloride. 2, 4-pentanedione (C5H8O2) was dissolved in methanol; it was then added to the iron(III) chloride/sodium acetate solution. The product of this mixture was filtered, and the precipitate

It should be noted that not all supplies are listed here as exactly what is needed to perform each method but a complete list can be found in the lab manual preceding each experiment.

items presently in solid form in the lab kit or purchased separately for this laboratory

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

(Hint the concentration of calcium ions in well 12 is 4.9 x 10-5 M.) Place 5 drops of 0.10 M NaOH in each of the wells 1 through 12. When the NaOH is added to each well, the initial concentrations of the reactants are halved, as each solution dilutes the other. Use an empty pipet to mix each of these combined solutions by drawing each solution up into the pipet and squirting it back into the well. (Hint the concentration of Ca2 ions in well 12 is 2.4 x 10-5 M.) Allow three or four minutes for the precipitates to form, then observe the pattern of precipitation. At one point the concentration of both ions becomes too low to have any precipitate form. We will assume that the first well with no precipitate represents a saturated solution. Part B NaOH varies, Ca(NO3)2 held constant To check your results, repeat the procedure but use a serial dilution of the NaOH. In a different row, put 5 drops of 0.10-M NaOH in well 1. Put 5 drops of distilled water in wells 2 through 12. Add 5 drops of the 0.10-M NaOH solution to well 2. Use an empty pipet to mix the solution by pulling the solution into the pipet and then squirting it back several times. The solution in this well, 2, is now 0.050 M in OH- ion. Continue this serial dilution to well 12, and then remove 5 drops from well 12. Add 5 drops of 0.10 M Ca(NO3)2 to each of the wells, and mix each with an empty pipet or stirrer. Again, determine the well where no more precipitate appears. Cleanup

Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was

Finally ensure that your results are accurate. You should have a light blue precipitate remaining when the sodium carbonate reacts with the copper chloride and when sodium sulphate ionises with copper chloride no precipitate should have formed.

* Please note that although you do not hand in items in observations, it is very important to do these as you may see some of these items on future/associated lab quizzes or be asked about some of these concepts on unit assignments.

For the first part of this experiment, six dry test tubes were obtained and labeled accordingly to test the following halides: 2-chlorobutane, 2-bromobutane, 1-chlorobutane, 1-bromobutane, 2-chloro-2-methylpropane, and bromobenzene. To each of the six test tubes 2ml of 15% sodium iodide in acetone was added. 4 drops of the appropriate halide was added to the test tube labeled for that specific halide. After adding the halide, the test tube was then shaken to mix thoroughly. If a precipitate formed the time it took was recorded. Since none of the solutions formed a precipitate at room temperature after five minutes, the test tubes were placed inside of a hot bath at about 50°C. After one minute, the test tubes were taken out of the hot bath and allowed to cool. If any test tubes formed a precipitate, the time it took was recorded on a table.

10ml of 2-chloro-2-methylbutane was added to 25ml of concentrated (12M) Hydrochloric Acid in a separatory funnel. The contents were swirled gently without the stopper and venting was done frequently to release excess pressure. Shake the funnel until the layers separate and able to recognize which one is the aqueous layer and which is the organic layer. The organic layer was washed with 10ml portions of saturated aqueous sodium chloride and cold saturated aqueous sodium bicarbonate. The organic layer was washed again with 10ml of water and saturated aqueous sodium chloride.

Predicting Precipitations Lab Report: explanation data of lab along hypothesis, and identifying possible errors of lab for further investigations. The reactions from 1A through 1D all have a precipitation formed because physical changes appeared. AgNo3 is a clear solution; when it is mixed with a yellow FeCl3, a precipitate is formed in a different color than the original colors. After a while, the precipitate became slightly solid. For 1B and 1C, the solid was formed in similar ways, it might be because both reactants contains a similar element.

b. For this lab the equipment used were electronic balance, graduated cylinders, and pipets.