The aspirator was turned to medium high, and then the copper was poured onto wetted filter paper. Using distilled water to remove all copper from the beaker. Once completely on filter paper 6mL of acetone was added to the copper to help dry it out. The filter paper was then removed and set down to dry completely. Once dry the filter paper was weighed with the copper on it and subtracted from the original weight to see the amount of copper left after
The purpose of this lab is to focus on how to make zinc iodide in a different way using compounds instead of elements, which are barium iodide and zinc sulfate. We will see if the reaction between these two compounds will occur and make a prediction by writing a chemical equation. The procedures for this lab are to place a small test tube inside a 50mL beaker and weigh it. Then, using a spatula, add 0.45±0.03 g of zinc sulfate heptahydrate into the small test tube and record the mass. After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid.
The purpose of the laboratory is to determine the number of waters of hydration in aluminum potassium sulfate as well as the purity of the Alum we produce. Experimental1: The procedure for this laboratory was followed closely from Professor Abrams’ lab manual. In Part 1 of this laboratory an aluminum soda can was cut apart and the paint and lacquer was rubbed off with steel wool. Next, the aluminum can was rinsed off with tap H2O and then cut into small pieces. Using the analytical balance 1.0537 g of the aluminum can was weighed out.
Once the procedure was performed three times, the collected iron fillings mass was obtained by using the digital weighing scale. After removing the iron fillings, the sand was removed next by using the property of sand that the sand was completely insoluble in the water. The iron free solids mixture was dissolved in 15.00 mille liters of distal water and heated by using stove top in a beaker. The solution was mixed for a while the benzoic acid and salt were allowed to dissolve completely and solubility was enhanced by heating the solution. The solution was decanted into another beaker.
Liquids and Solids Purpose: The goal of this experiment is to be able to identify melting/boiling points of substances. We can then use these methods to identify unknown substances because of constants in melting/boiling points. Procedure: 1. Boiling Point a. Begin by adding 1 mL of rubbing alcohol to test tube and attach a thermometer to it.
After all the acid has been completely added and the reaction has stopped, use a pipette to add a few extra drops of acid into the beaker until the reaction stops. 7. Place the beaker on a hot plate and heat on a high setting to boil off the water. WARNING: THERE WILL BE A SMALL AMOUNT OF HYDROCHLORIC ACID BOILING OF THE MIXTURE. DO NOT PLACE YOUR FACE DIRECTLY ABOVE THE BEAKER.
10. The test tube was removed from the flask using tweezers and the contents were disposed of in the waste container. The equipments were cleaned and dried for the next use. 11. Steps 1-10 were repeated using Copper (II) Sulfate and sodium hydroxide solution Part B: 12.
Using a Buchner funnel, a hose, and a suction flask we created a vacuum filtrator which we used to help remove the remaining liquid on the copper so that we may make a more precise measurement of the mass of the remaining copper. Our final mass of copper was .7951 grams. Results and Discussion: Initial Mass of Cu: .25 grams When we mixed the 5 ml of 6 molar HNO3 the copper had disappeared, indicating it had been used in the reaction. The copper had undergone a single replacement reaction and a decomposition reaction. Initial equation: Cu(s) + HNO3(aq) -> Cu(NO3)2(aq) + NO2(g) +H2O(l) Balanced: Cu(s) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) The copper had replaced the Hydrogen in the HNO3 and the NO3 had also broken down into NO2 and O2- allowing the H+ to bond with it and create
In order to find which reactant is the limiting reactant, an equation based on the molarity of the Copper (II) Chloride may be used, or the products of the reaction may be observed. If the bluish tint of the Copper (II) Chloride fades, or disappears before the Aluminum is completely used to form Aluminum Chloride, then it can be said that the Copper (II) Chloride is the limiting reactant in this reaction. On the other hand, if all of the 1.5 grams of Aluminum pebbles are used to create Aluminum Chloride before the Copper (II) Chloride solution changes color, then it can be said that the Aluminum is the limiting reactant in this reaction. Hypothesis: If 1.5 grams of Aluminum pebbles are placed in 100 ml of 0.25 molarity Copper (II) Chloride aqueous solution in order to determine which of the reactants is the limiting factor, then the Copper (II)
SYNTHESIS 3 Purifying an unknown solid by recrystallization involved preparing cobalt amine chloride product. By adding five grams of cobalt II chloride into 20ml of 9M HBR in 250 mL beaker, plus 15 mL of deionized water. Dissolving the compound within pure water, filtration by gravity and adding two grams of activated charcoal and 25 mL of concentrated. Cooled after heating and additional six mL of 30 percent hydrogen peroxide. Filter by suction then collect the dark solid.