Synthesis Lab Report Results

For example, silver nitrate formed a white precipitate when it was tested with ammonium chloride. In contrast, unknown 3 did not formed any precipitate with ammonium chloride. Ammonium chloride change the color of unknown 3 to a light green while the solution of silver nitrate and ammonium chloride was cloudy white solution. Likewise, the metal in unknown 3 could have been Calcium neither. Data and observation shows that calcium nitrate whether formed a white precipitate or did not react at all while unknown 3 formed an orange precipitate. Therefore, silver and calcium are not the two metal present in unknown

This was determined by observing significant reactions that occurred when the powders that Unknown Mixture #2 consisted of were individually tested with the liquid reagents. Alka-seltzer proved to be a highly reactive reagent as bubbling occurred whenever any of the liquid reagents were mixed with it. It appears that alka-seltzer created a neutralization reaction with each of the liquids. Since alka-seltzer and baking soda contain similar chemical properties, it can also be inferred that the bubbles that were apparent for each of these neutralization reactions was the gaseous carbon dioxide that was created during the reaction. While alka-seltzer seemed to be highly reactive, table salt wasn’t very reactive at all. Despite the fact that salt wasn’t very reactive, it can still be deduced that salt was in Unknown Mixture #2 without noticing any of its reactions. This is because it is already evident that baking soda and cornstarch are in Unknown Mixture #1. Since two of the four possible substances are already in Unknown Mixture #1 and none of their special properties were observed in Unknown Mixture #2, the presence of salt in Unknown Mixture #2 can be confirmed by using the process of elimination. By understanding how each of the powders reacts with each of the liquid regents, the substances of the unknown mixtures can be

The unknown contained silver, as both the unknown and silver solutions turned red and formed red precipitates with the addition of potassium chromate.

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

the  solution was recorded.  The  first test  performed was  an  Anion Elimination Test,  the Silver  Nitrate

In the last test, we had to test out a mystery powder (powder A, B, C), in its own separate test tube, in order to solve the Sherlock Holmes Mystery. Our group had powder C. When we mixed water in the mystery powder, it did not dissolve. When the litmus paper was put into the test tube it turned blue. When the vinegar was mixed it bubbled/foamed up. When we mixed the iodine solution, there was no reaction and the solution turned to a dark brown/black color. When we mixed in the baking soda there was no reaction and it turned to an even darker color.

D. You suspect dissolved silver ions in a solution. How would you test this solution to confirm the presence of the silver ions?

Ammonia was detected, and the anion test for chloride was positive while all other tests resulted negatively. Solution C displayed a dim purple flame during the flame test, indicative of potassium. All anion tests performed were negative, so

Unknown Solution 8 was identified as sodium oxalate from its formation of white silver oxalate precipitate with silver nitrate, clear brown solution formation with sodium sulfide, milky white solution formation with barium chloride (the white particles in the solution were barium oxalate), and white lead (II) oxalate precipitation reaction with lead (II) nitrate. Though Solutions 4 and 10 reacted with lead (II) nitrate to form a brown precipitate just as sodium sulfide would, the two unknown solutions did not form a clear brown solution with sodium oxalate and had different but similar properties in other binary mixings; this might be due to contamination, so Solutions 4 and 10 are likely sodium sulfide. Though it reacted differently with sodium sulfide, Unknown Solution 11 was identified as sodium oxalate because of its many white precipitate-forming reactions. Sodium carbonate formed a milky yellow-white precipitate (silver carbonate) with silver nitrate, a white precipitate (barium carbonate) with barium chloride, and reacted with lead (II) nitrate to form lead (II)

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

First, the iodine test was preformed. Two grams of the unknown mixture were put into two different divots. A drop of iodine was put into one divot. Since the mixture turned blue-black, the powder was corn starch and the vinegar test was not necessary. Then, the flame test was preformed. The unknown mixture was put into a vial which was then filled with water. The vial was shaken until the mixture dissolved. Once it was fully dissolved, the mixture was poured through a paper filter into a test tube in order to remove the corn starch. A platinum rod was dipped into the test tube. The platinum rod was then placed over a lit bunsen burner. The color of the flame was

Chloride did not have a colour to it which means it was clear. If large amounts of chloride is present in water then it's probably because of a reason related to salt. The reason may be because of water passing through salt formations. When this happens then water has a very salty taste. When we testing than sample C had the highest result, 60 ppm which doesn’t mean it's unsafe. It probably means that it’s very salty compared to the other two because it might have passed through salt formations. Sample B, 20 ppm which was also the closest to 250 ppm which is the highest drinking level water recommended for humans. Sample A was 0 ppm.

The aim of the experiment to perform a chemical neutralisation reaction by using hydrochloric acid and sodium hydroxide solution was achieved because the base plus acid turned into salt and water. While performing the flame test using a wire loop along with the white crystals from the evaporating dish turned the flame to yellow rather than yellowish-orange colour, which indicates sodium. The reason why the solution turned cloudy was that it indicated that the neutralisation reaction was complete. The worded solution that was formed was silver nitrate + sodium chloride → Sodium nitrate + silver chloride (AgNO3 + NaCl → AgCl +

Place two drops of the silver nitrate into every beaker to observe if sodium was present.

The Biology Department requested the identity of seven different samples. The aqueous ionic solutions were sent to be disposed of by the company Enviro Safe, Inc. However, the shipment containing seven, five-gallon carboys, was labeled Experiment 9 and did not include the names of solutions. The faculty in the Biology Department was unfamiliar with the contents but was able to locate a pre-laboratory notebook dated ten years prior, the notes only revealed that eight unknown solutions were involved in the experiment. Enviro Safe would have charged $350 per carboy to analysis the products if not identified by the laboratory class. In order to save the department money all seven samples had to be labeled correctly and the identity of the one missing solution revealed. To fulfill the Biology Department’s request, the experiment involved mixing the solutions together two at a time so the reactions, if any, could help determine the names of each solution.