The materials that this experiment needed was ten milliliters of ammonium hydroxide solution, beaker, five beral-type pipets, bunsen burner, twenty milliliters of copper(II) sulfate solution, evaporating dish, hot plate, twelve milliliters of hydrochloric acid, four pieces of magnesium ribbon, one milliliter of phenolphthalein indicator solution, two milliliters of potassium iodide solution, three milliliters of silver nitrate, two grams of sodium bicarbonate, one milliliter of sodium bicarbonate solution, seven milliliters of sodium hydroxide solution, two milliliters of sodium phosphate solution, test tube holder, fourteen 13 x 100 mm test tubes, five 20 x 150 mm test tubes, tongs, and water, deionized or distilled. First, reactant formulas, …show more content…
In reaction one, the magnesium ribbon was held, with tongs, in a burner flame and observations were made. Reaction two first heated fifty milliliters of water in a 150 milliliter beaker and was heated until it was boiling. After, the water was removed from the heat and using tongs, the magnesium ribbon was dropped into the hot water and two drops of phenolphthalein was added to the mixture. Observations were made and reaction three began. A 13 x 100 mm test tube was used and, using a beral pipet, five milliliters of the hydrochloric acid solution was added. After, the magnesium ribbon was put into the mixture and observation were taken into account. Lastly, the magnesium ribbon was cleaned and added to a 13 x 100 mm test tubes which contained about two milliliters of the copper sulfate solution and observation were made at the end of the …show more content…
In reaction eleven, 0.2 grams of solid sodium bicarbonate was placed in a 13 x 100 mm test tube. Using a beral-type pipet, one milliliter of the hydrochloric acid solution was added to the test tube and when the substance reacted, observations were made. Later, in a 13 x 100 mm test tube, one milliliter of sodium bicarbonate solution was mixed with one milliliter of the hydrochloric acid solution and the reaction between the two substances was studied and observed. Again, a 13 x 100 test tube was used and about one milliliter of the silver nitrate solution and one milliliter of the hydrochloric acid were mixed together to create a reaction. Observations were then made and written down. Finally, a 13 x 100 mm test tube was utilized to mix about one milliliter of the sodium hydroxide solution and one milliliter of the hydrochloric acid solution. Conclusively, observations were made and part III of the lab
Reaction 3- 1. Obtained a clean and dry test tube and placed a small amount ( about the size of a jelly bean) of ammonium carbonate into the test tube.
During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the
A 0.5 g of sodium tungstate dihydrate was weighed and transferred into a 50-mL round-bottom flask with a magnetic stir bar. Approximately 0.6mL of Aliquat 336 was then transferred carefully into the round bottom flask using a 1mL syringe. The round bottom flask and its contents were then set up in an oil bath. 11mL of 30% hydrogen peroxide and 0.37 g of potassium bisulphate were added to the reaction mixture in the round bottom flask and stirred using a magnetic stirrer. Lastly, 2.5mL of cyclohexene was added using automatic dispenser and the mixture stirred. A condenser was fitted on the round bottom flask, clamped and attached to water horses. The reaction mixture was then heated on the oil bath and the reflux process initiated for an hour while stirring the mixture vigorously. Half way while rinsing, any trapped cyclohexene in the condenser was rinsed. After 1 hour, the round bottom flask was rinsed
Magnesium ribbon was reacted with Hydrochloric acid in three different experiments to determine the charge on a metal ion. After running multiple tests in the three different procedures, the Crystallization method proved to be the best method for determining the charge of the metal ion by using mole to mole ratio.
The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.
It is expected that the concentration of hydrochloric acid will increase the rate of the reaction between magnesium ribbon and hydrochloric acid. By increasing the concentration of
As the tube is still heating, a flaming splint will be placed in the opening. In the next reaction, one gram of copper carbonate will be added to a desiccator and heated to one hundred fifty degrees Celsius. In the step of acid-base reactions, two milliliters of hydrochloric acid will be inserted into a tube and mixed with two or three drops of phenolphthalein. Potassium hydroxide will be added in drop quantities until a pink color remains after being swirled inside. At last, the reactions of metals, gaseous products, and neutralization will have shown results that can be used to write chemical equations to represent the reactants and products of each
The many different aqueous solutions involved were potassium nitrate, zinc nitrate, potassium ferricyanide, sodium phosphate, sodium hydroxide, magnesium nitrate, copper (II) nitrate, sodium chloride, iron (III) nitrate, calcium nitrate, sodium sulfate, and sodium carbonate. These different reactants were combined to test whether or not a precipitate, color change, or both would occur in that in that those reactions. The purpose of this lab was to demonstrate what a double replacement reaction as well as a precipitate
Half a gram of magnesium was measured on a scale and 50 millimeters of 2M hydrochloric acid in a small graduated cylinder. The HCl was then added to the Erlenmeyer flask. The tube was secured to the Erlenmeyer flask and was ran under the large graduated cylinder in the tub. With the rubber stopper off and other equipment ready, the magnesium was added to the Erlenmeyer flask. Quickly, the rubber stopper was placed on top of the flask to ensure that no gas escapes.
Experiment to investigate the amount of sodium hydroxide needed to neutralize the solution of vinegar
Table #1 shows that the length of the sample of magnesium ribbon given was 1.67 cm (to 3 significant numbers), the barometric pressure (total pressure) was 95.81 kPa, the room temperature was 24.9 °C, and the measured gas volume converted from 24.72 mL to L was 0.02472 L. Then, the pressure of H2 was found by using Dalton’s Law of Partial Pressure, using the equation Ptotal = PH2+ PH20., found on Table #2 Part A. The pressure of H2O, 4 kPa, was determined by using Table H Vapor Pressure of Four Liquids on the Reference Table for Chemistry. Then, the pressure of H2O, 4 kPa, was subtracted from the total pressure, 95.81 kPa, to find the pressure of H2, 91.81 kPa. Next the mass of the sample of magnesium was found, shown on Table #2 Part B, given that the mass of Mg = 0.0100 g/cm. It was calculated that the mass of Mg per length found was 0.0167 g. Afterwards, the mass of Mg was converted to moles, using 3 significant numbers, shown in Table #2 Part C. The calculations shows that the number of moles of Mg found was 0.000687. Next, the mole ratio of Mg to H2 produced was determined by writing a balanced equation for the reaction, found on Table #2 Part D. The mole ratio of Mg to H2 produced was 1:1. Then, the number of moles of H2 produced (using 3 significant numbers) was found by using stoichiometry, shown on Table #2 Part E. The number of moles of H2 produced
Procedure To perform the experiment five chemical reactions where used: NaCl, NaI, Na2CO3, Na2HPO4 and Na2SO4. The unknown substance (unknown #8) would also serve as a chemical reaction, but would be separate from the five chemicals because it’s one of the five reactions that’s trying to be determined. Chemical standards, HNO3, Ba(NO3)2 + HNO3, AgNO3, AgNO3 + HNO3 and Thymol Blue, were also used to assure accuracy of the unknown
Using chemical principles that you have learned this year, explain why you used copper wire to make the basket that held the magnesium in place.
12. The crocodile clips are attached to the copper electrodes of the experimental apparatus and the power supply is turned on. Simultaneously, the stopclock is started. The thermometer is checked every 30s. 13. After 300s the stopclock is stopped and the power supply is turned off. The negative cathode is carefully removed and is dried using a hair dryer. 14. When dry the negative cathode is placed on the electronic milligram balance and its final mass is recorded. 15. The positive anode and negative anode of the experimental apparatus are disposed and the electrolyte is poured out to ensure that the anode slime (impurities) does not contaminate the solution. 16. The electrodes of the experimental apparatus are replaced with new copper strips. 17. Steps 7 to 16 are repeated. However, this time, the rheostat is adjusted using the calibration apparatus until the multimeter shows approximate readings of 0.40 A, 0.60 A, 0.80 A and 1.00 A respectively. 18. Time permitting, the entire experiment is repeated. Safety Copper sulphate may cause irritation and burns if it comes into contact with the eyes. As standard lab procedure, safety goggles and lab coats must be worn at all times. Control of Variables Volume of Electrolyte Used
Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid