Essay about Determination of Cu2+ by Titration

At five minute intervals over the next fifteen minute period, record the color intensity of the solution of each test tube.

All standardizations are performed in triplicate. Weigh out .1000-.1200 gram KIO3. Add 70-80 mL of deionized water. Swirl and dissolve. Add 3 mL of 6M HCl. Swirl and mix. Quickly titrated the brow-red solution with 0.1M Na2S2O3 until it is light yellow. Then add 3.5 mL of starch indicator. Titrate again until the dark color first disappears.

We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

20) If the solid is still not dissolved, add a tiny amount of hexane and swirl again.

twice. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the red

Next, obtain a 96 well plate and take 1 sample of 190 μl from the blank and put it in well #A1. Then take 3 different 190 μl samples of concentration 0 and put it in Wells F2, G2, and H2. Repeat this step again by taking 3 more different 190 μl samples of concentra-tion 1 and putting it in wells F3, G3, H3. It should be noted that it is important to vortex each

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

I started with elemental copper metal and then reactions occur step by step as follows:

1) Pour 25 mL of the 1 M hydrochloric acid into the beaker and rinse the solid by swirling the acid around in the bottom of the beaker.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Squeeze one drop of food coloring into the water and observe closely for 1-2 minutes.

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

Remove the tubes and add 2-3 drops of Iodine – potassium – iodide solution to each tube.