Zinc and Hydrochloric-Acid
Abstract:
We observed the reaction between zinc and hydrochloric acid and recorded it in a table and learned wether the percentage of zinc is effected by the amounts of both substances added to the solution.
Introduction
The purpose of this experiment is to determine if the amount of zinc and hydrochloric acid will effect the percentage of the zinc in the out coming solution. We are reacting zinc metal with hydrochloric acid to produce a compound of zinc and chlorine atoms. We are then recording our data and observations and place it in a logical data table.
Purpose
The whole purpose of this experiment is to determine wether or not the amount of the zinc and or hydrochloric acid effects the out coming percent of the solution after under going chemical reaction.
Procedure
$ 1. Weigh the zinc metal pieces and place them in a test tube
$ 2. Pour some hydrochloric acid over the zinc pieces. Observe
$ 3. Allow the zinc d hydrochloric acid to set over night to make sure that the reaction reaches completion.
$ 4. Weigh a clean dry evaporating dish.
$ 5. Decant the liquid remaining in your test tube into the evaporating dish.
$ 6. Pour 2-3 ml distilled or de-ionized water into test tube and rinse any remaining zinc with water and decant the water into the evaporating dish also. If you have no remaining zinc pieces, rinse the test tube and decant the liquid into the dish.
$ 7. Heat the evaporating dish until there is no more liquid remaining in the dish. The solid remaining will have a puffy and waxy look. Do not overheat but remove from the hot plate and turn off the heat source because the product has a relatively low melting point and it will melt and evaporate away in a white cloud
$ 8. When th evaporating dish has cooled sufficiently, weigh the dish with its contents.
$ 9. Clean up by washing and drying your evaporating dish.
$ 10. Calculate and report your % zinc in the compound to your teacher for comparison with other lab groups.
Data and Observations
I observed that as the chemicals reacted together in the test tube the solution began to create bubbles while the zinc rested at the bottom and then the test tube became hot to the touch from the chemical reaction.
5.) One at a time, place your test tubes in the water bath and heat the first test tube to 25 , the second to 50 , the third to 75, and the last to 100 degrees c. Remeber to stir with your stirring rod every so often.
Abstract: This week we experimentally determined the rate constant k for the reaction 2HCl (aq) +Na2S2O3 (aq) → S (s) + SO2 (aq) + H2O (l) + 2NaCl (aq). In order to do this the average reaction time was recorded in seconds during two trials. The data from the experiment shows this reaction is in the first order overall: rate=.47s-1 [HCl]0 [Na2S2O3]1. These findings seem to be consistent with the expected results
An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases as you move down in the same group. With this in mind, the reactions of the substances involved in this experiment may be hypothesized, observed, and validated.
About 25ml of distilled water was added. Then 2-3 drops of phenolphthalein indicator solution were put in. It was swirl to dissolved the solid.
neutralize 35ml of our base. Once we weighed out the KHP we then dissolved it
To begin this experiment, I purchased two boxes of borax to pour inside of the pot, two tall glass glasses to hold the borax solution, one ball of string to dip in the glasses, and wooden pencils to hold the string on. The other supplies that I used were screws, a large bowl, ice, and plastic wrap.
3. Fill up the 50 milliliter beakers all the way up with deionized water. After, use your scopula to scoop out a small portion of one substance and put in into your beaker. Then put your hot plate onto medium temperature and rest the mixture onto the plate.
Place the evaporating dish on the iron gause and heat the hydrate on low for two minutes, then high for five.
One of these concepts had to do with solutions – a mixture composed of minor ingredients and a major ingredient, respectively, the solute and the solvent. In the experiment, CuxOy was mixed with HCl to create a copper oxide solution; the result of the mixture was copper chloride and water. By putting both compounds together, a double displacement reaction occurred. This sort of reaction happens when two ionic compounds switch anions and cations to form new ionic compounds. However, not only is this a displacement reaction, but it is also a neutralization reaction – a reaction with an acid and a base that forms salt and water. By reacting CuxOy with HCl, respectively a base and an acid, CuCl (a salt) and H2O was formed. In addition, a single displacement reaction occurred right after Zn was introduced to the solution. Rather than two ionic compounds reacting, the single displacement reaction happens when an element reacts with an ionic compound. The element forms a new compound with one of the components of the other compound, leaving a new compound and a new lone element; in the case of this experiment, CuCl reacted with Zn to create zinc chloride and elemental copper. This was done as a way to isolate the copper so that it can be weighed later. Nonetheless, once at the weighing stage, Cu was laced with water and isopropyl alcohol. To fully isolate the Cu, both the water and
...e will also become faster. In phase one, Nature of the Reactants five different metals were placed in the 2M HCl they all reacted differently with magnesium being the most reactive and copper being the least reactive. In phase two, Concentration, zinc was placed in different concentrations of 6M HCl. The higher the concentration was the more reactive the metal was. Next in phase three, Temperature, zinc was added to 6M HCl which was a different temperatures and the zinc was the most reactive with the HCl in the boiling water and least reactive with the HCl in the ice bath. Then in phase four, Surface Area, the powered zinc was more reactive then the piece of zinc in the 6M HCl because it had more surface area to be covered than the piece of zinc. Lastly in phase 5, Catalyst, the 3% H_2 O_2 was reactive with the 5 drops of 〖FeCl〗_3 but not with the 5 drops of water.
6. Place the test tube in the beaker. Secure the test tube and thermometer to the retort stand using clamps. Begin heating the water bath gently.
My goal in this experiment was to determine the amount of zinc (in grams) on 5 different galvanized nails to see if this specific box was up to standard, as well as how consistent the weight of the zinc is on each nail and do so by measuring the weight of the nail initially, then take the zinc off with the hydrochloric
Varying the n value carries out the experiment. Absorbencies of each of the ZLn complexes are obtained. The sum of the concentrations of the metal, Z, and the ligand, L, are kept equal. With the ratio of the ligand to the metal in the solution with the maximum absorbance for the ZLn complex, the value of n can be determined as well as the composition of ZLn.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).