A flame test was then conducted and the identity of the cation was determined. To determine the anion, the anion had to be separated first from the cation in the unknown compound. To do this, 0.1 grams of the unknown compound and 0.5 grams of sodium carbonate had to be boiled in 5 mL of distilled water. Once the solution boiled for 10 minutes, the precipitate was centrifuged out and the anion solution was left. 0.1 M silver nitrate was added to the anion solution and a precipitate was formed.
10 drops of each solution was added to the appropriate centrifuge tube. 6 M NaOH was added drop wise to each solution until a precipitate was formed, or until 20 drops were added. Another 10 drops of 6 M NaOH were added to the solutions that formed a precipitate. Again, 5 centrifuge tubes were labeled for the same 5 cations and 10 drops of each solution were added to the appropriate centrifuge tube. The 15 M NH4OH was added drop wise until a color change occurred, or until 20 drops were added.
Mix using a plastic pipette. f After 10 seconds, use the plastic pipette to place one drop of the mixture on the first drop of iodine. The iodine solution should turn blue-black. Squirt the rest of the solution in the pipette back into the test tube. g Wait another 10 seconds.
Boil at least 10 minutes. 7. While the metal is still in the boiling water bath, measure the temperature of the boiling water carefully with a thermometer and record to tenths, one decimal place, in Data Table 2 8. After the metal has been heating 10 minutes, remove the metal from the boiling water bath using the string. Immediately transfer the metal into the calorimeter cup so that the water covers the metal.
Use the pipet to place 10ml of water into an empty test tube 3. Place two drops of red dye into the test tube 4. Place one drop of yellow dye into the test tube 5. Compare the controlled color to the new color 1. Repeat steps one and two 2.
Then, 10 mL of distilled water was added to the precipitate. And 9 mL of H2SO4 was added drop by drop. For the last step, 0.3056g of zinc was weighed out, and was added in reaction mixture to react. After decanted, 5 mL of 6 M HCl was added to react with remaining zinc. A vacuum filtration apparatus was assembled.
Equipment List * Boiling Tube * 10 cm3 1mol dm-3 Hydrochloric Acid (HCL) * 15 cm3 1mol dm-3 Sodium Hydroxide (NaOH) * pH and Temperature Probes * Data Logger * Measuring Cylinder ‘ * Boiling Tube * Teat Pipette Method * Add 10ml of Hydrochloric acid, measured in a measuring cylinder, into a boiling tube. * Into a data logger, plug in both pH and temperature probes and switch on data logger. * Put in both the probes and measure both the temperature and pH before adding any other substances. * Add 1cm3 of Sodium Hydroxide, measured in a measuring cylinder, to the Hydrochloric acid, and
Then, 3 drops of 3 M HCl was added to each of the solutions and the color of each was recorded. Then, the spot plate’s contents were put into the waste beaker and the plate was cleaned. After that, 1 drop of each of the five transition metal cations was added to separate holes in the spot plate, 3 drops of 3 M NH4OH was added to each hole and the color of each was recorded. Then the spot plate was cleaned again and 1 drop of each of the five transition metal cations was added to the separate holes. After that, 1 drops of dimethylglyoxime (DMG) was added to each and the color of each was recorded.
Introduction The purpose of this lab is to determine the normality of an unknown base using a volumetric titration. The volumetric titration used for this experiment consisted of a standard acid called potassium hydrogen phthalate (KHC8H4O4) titrated with a weak unknown base. An acid-base indicator called phenolphthalein is used in order to view the reaction proceeding to completion. The indicator allows visualization of the acid changing colour when the solution has reached the end point. The normality of the unknown base is calculated after the solution has reached the end point.
.40g of NaH_2PO_4, and .40g of Na_2HPO_4 was measured into a 150 mL beaker. 50mL of distilled water was then measured in to a graduated cylinder and added to the 150ml solution of NaH_2PO_4 and Na_2HPO_4. 20 drops of the .04% Bromothymol blue solution was then also added to the buffer solution. After adding the 20 drops the tint of the liquid changed to a light green. The Vernier pH probe was calibrated and used to determine the pH of the phosphate buffer solution which was 6.81.