PURPOSE To investigate the reactions of a typical acid (dilute hydrochloric acid) with metals, metal oxides, carbonates and bases. APPARATUS The following materials in order to complete this experiment: Dropper bottles containing 0.1M solutions of hydrochloric acid or limewater (calcium hydroxide) and sodium hydroxide. Dropper bottle of bromothymol blue indicator Small samples of the following metals: zinc, copper turnings, magnesium and iron Copper (II) oxide powder Magnesium oxide Marble chips (calcium carbonate) Sodium carbonate 12 test tubes and test tube holder Bunsen burner Stopper or cork Wax taper and matches PROCEDURE (a) REACTION WITH METALS Place a small piece of magnesium ribbon in a test tube and add about 2mL of dilute HCL. Stopper the test tube and allow the gas to accumulate. Remove stopper and test for the gas that evolved by holding a lighted taper to the mouth of the test tube.
4.) Use pipette to accurately measure 10cm3 of HCl into the 1dm3 volumetric flask. 5.) Add distilled water in a wash bottle to the acid until the level has almost reached the white line, then use a teat pipette to fill it up to the point where the meniscus is just on the line. 6.)
Remove approximately 0.35 g into a 250 mL beaker. check the balance and record the mass of the remaining mixture in the vial. In the laboratory hood, dissolve the copper with ~ 3 mL of nitric acid. Allow the beaker to remain under the hood until the fumes cease. The remaining solution should be blue.
The dropper was placed into the ammonium nitrate solution, and a bit more copper (II) sulfate solution was added. A piece of copper was added to the dropper. A half cell containing 0.1M Silver Nitrate and a wire of silver medal was prepare vial with the copper electrode. The voltmeter leads were attached to the copper and sliver electrodes so there as a positive reading. The initial Ecell was recorded along with the polarity.
Phenolphthalein indicator will turn slightly pink when the solution is neutralized. Materials: • 0.05 M of Sodium Hydroxide solution (NaOH) • Vinegar (Acid “A” and Acid ”B”) • Phenolphthalein indicator • Two 150ml beakers • 50ml Burette • Three 250ml Erlenmeyer flasks • 10ml pipette and pipette bulb • Wash bottle • Funnel • Retort stand and clamps Procedure: 1. Clamp the 50ml burette to the retorted stand and add the sodium hydroxide solution (base) using a funnel. 2. Clean one of the Erlenmeyer flasks using a wash bottle and add 10ml of Acid “A” into it.
You should be left with 250cm3 of 0.1 mole dm3 sodium carbonate solution. Method of Titration =================== 1. Attach clamp to stand and then clamp the burette vertically (place the burette high enough so the conical flask can fit underneath it). 2. Place a funnel into the top of the burette and then rinse the burette out by letting some sulphuric acid run through it.
2. Prepare a test cell to measure the voltage of the copper and zinc half-cells. 3. Put approximately 2 mL 1.0 M zinc nitrate solution in one of the center wells of a 24-well plate. 4.
The equipment I will use is: · Hydrochloric acid · Sodium Thiosuphate · 2 x Measuring cylinders · 2 x Test tubes · stop clock · 2 glass beakers · 2 thermometers · Bunsen burner · water · tripod · heat mat · gauge · paper with pencil cross I will make sure my results are accurate by referring to graphs, e.g. : if one point is greatly out of alignment, it should be repeated. Also I will make sure that the meniscus of the hydrochloric acid and Thiosuphate is flat and not to one side of the test tube or measuring cylinder. I will take five measurements with a 10 gap interval and I will repeat this twice and take an average to make my results more accurate. Back ground Research - Trial Experiment I conducted a trial experiment to find out the correct quantities of sodium thiosulphate and hydrochloric acid for the main experiment.
In your Data Table, record the samples added to each test tube, describe the reaction observed, if any, and whether or not a chemical reaction took place. D. Put on your safety glasses and let¡¦s begin: 1. Put the amount of 0.1M cobalt (II) chloride hexahydrate that fills the end of a spatula into a test tube. Then add 2mL of 95% ethanol. Tap the end of the test tube to mix the solution and record the pertinent data in section 1 of the Data Table.
2. Method Table 1: Synthesis of K2[Ni(CN)4] Amount of Reagents used Method Observations NiSO4 • 7H2O : 6.00 g KCN : 3.01g In 20ml water NiSO4 • 7H2O was dissolved and the solution containing KCN (dissolved in 7ml water) was added to the Nickel solution. This solution was filtered and the precipitate was washed with small quantities of water. This precipitate was added to the solution of KCN (dissolved in 3ml of water). This solution was heated and swirled so that the crystals that formed dissolved.