Cations And Anions Lab

While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

After copper ions were filtered, approximately 15mL of .5 M was added to the filtrate, which made the mixture acidic. Then, 20 mL was added into the filtrate to raise the pH of the mixture.

Metal cations can be identified based on the colors they emitted off when heated in a flame.1 When atoms of the ions that were tested are excited, their electrons move up to higher levels of energy.2 When the electrons relax and return to the original states, they emit photons of specific energy creating wavelengths of light that produces colors.3 The test wire and Bunsen Burner were used to excite the solution in the crucible. The standard metal cations that were tested and their outcomes are as shown in Table 1.

Copper Standard Solutions Preparation: To prepare the copper standard solutions the students added 15 M NH¬4OH (4mL) to a designated amount of stock solution (0.100 M) in a volumetric flask (50mL). Standards one through six contained the following mL of original stock solution: 1.00, 2.00, 4.00, 6.00, 8.00, and 10.00. Once each of these solutions were combined with the ammonium hydroxide (4 mL) they were filled to the mark on the volumetric flask (50mL) with distilled water and swirled. Recording Absorption

The converse was true for the 5% NaCl solution without Elodea and the 5% solution with Elodea (table 1). A comparative observation revealed that the beaker with Elodea in salt solution required more NaOH than did the beaker with Elodea in tap water (figure 1). Table 1. The number of drops of NaOH in each beaker Beaker Name Number of Drops Tap Water

Procedure The various solids and liquids were used for this lab. The first experiment had effects of the temperature towards the chemical reaction. The first experiment had two test tubes filled with same amount of substances to react, but one was at 10 ºC while the other one was at 50 ºC. The second experiment involved different molar concentration of substances reacting. Individual test tube was filled with 1.0,

3. Upon adding 20 drops of NaOH, a white precipitate was formed signifying acidic impurity. In the second NaOH mixture, about 20 drops were administered and no precipitate formed indicating that the ample is more pure than before. Data: Weight of flask = 75.10 grams Weight of the flask with solids =

Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.

If bubbles are not produced, perform the sulfate test 10. Record if there is a precipitant, if not use the halide test to find out if it’s a chloride, bromide or iodide 11. If the precipitant is white it’s chloride, if its off white/cream its bromide, if its yellow its iodide Results Unknown Chemical Letter: 1 Test Observations Flame test Orange Sodium Solution colour No reaction Precipitant No Carbonate test No reaction

The purpose of the “Titration of the Unknown Acid” lab is to determine how much of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows: 0.1M NaOH, Acid solution, Anthocyanin (which is found in red cabbage leaves) indicator, Burets, Ethanol 95% and DI water. First Professor Greenberg assign a labeled unknown acid solution, then we recorded the solution’s identity and bottle code.

These will then be tested with the pH scale to find out the results. Method

In this experiment, each of the unknown solutions were tested for the presence of chloride, nitrate, and acetate. For unknown 2, there was no precipitate formed during the chloride test, concluding that it did not contain chloride. Unknown 2 also produced a negative for the nitrate test, since a brown ring did not form, indicating that it did not contain any nitrate ions. The last test, the acetate test, was not conducted on unknown 2 due to the results from the cation tests. For unknown 4, the chloride test also produced a negative result, indicating the absence of any chloride ions.

2ml of 10% ammonium citrate was added to each beaker. The pH was then adjusted to 8.5 by adding 10 drops of 5M NH4OH(aq) to each beaker. 3ml of 0.1% cuprizone was added to each beaker. The four solutions were then transferred to 25ml volumetric flasks. The beakers were washed with de-ionized water, and the washings were combined with the solutions in the 25ml volumetric flask.

The chemical equation for this experiment is hydrochloric acid + sodium thiosulphate + deionised water (ranging from 25ml to 0ml in 5ml intervals)  sodium chloride + deionised water (ranging from 25ml to 0ml in 5ml intervals) + sulphur dioxide + sulphur. As a scientific equation, this would be written out as, NA2S2O3 + 2HCL + H2O (ranging from 25ml to 0ml in

The lid was secured over the bottle and the contents were then shaken thoroughly. A piece of tape was placed onto the bottle with the groups names, and space for the concentration of NaOH and standard deviation to be written at the end of the experiment. After 0.1 M NaOH solution was prepared, the next step is to standardize the NaOH solution by using titration. To begin, a buret was cleaned with soap and deionized water to insure that there was no