Silver chloride

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substance that is not aqueous was formed. The reactions that did not form a precipitate were DNR, which means that they did not react. At station one barium chloride and potassium nitrate did not react but barium chloride and silver nitrate reacted to form barium nitrate and silver chloride. The precipitate at station one was silver chloride. Both reactions at station two did not react. Station three had a reaction occur between sodium carbonate and calcium sulfate forming sodium sulfate and…

for the possible ions, 1.0 mL of silver nitrate and 1.0 mL of nitric acid were used for the ion test. Ammonium chloride and calcium chloride were the two compounds that were tested on to see if either were the unknown compound. After obtaining a balanced chemical equation that would allow for the synthesis of calcium chloride, it was determined that 0.858 g of magnesium chloride and 0.902 g of calcium carbonate needed to be used in order for 1.000 g of calcium chloride to…

Part III: TRIAL 1 TRIAL 2 Mass of sample KNO3 1.039g 1.041g Drops of AgNO3 27 drops 28 drops 1. Net ionic eq. for formation of solid silver chloride from aqueous solution NaCl(aq)+AgNO3(aq)→ NaNO3(aq)+AgCl(s) Na+(aq)+Cl-(aq)+Ag+(aq)+NO3-(aq)→ Na+(aq)+NO3-(aq)+AgCl(s) Cl-(aq)+Ag+(aq)→ AgCl(s) 2. Net ionic eq. for formation of solid silver chromate from aqueous solution K2CrO4(aq)+2AgNO3(aq)→ 2KNO3(aq)+Ag2CrO4(s) 2K+(aq)+CrO42-(aq)+2Ag+(aq)+2NO3-(aq)→ 2K+(aq)+2NO3-(aq)+Ag2CrO4(s)…

other compounds. After performing the four anion tests, a positive identification was able to be made showing that the unknown compound contained a chloride ion since a white precipitate was formed from the reaction (Table 1). The sulfate, nitrate, and carbonate tests all yielded negative results when no precipitate was formed. The reaction of the chloride anion is as follows: Cl- + AgNO3 -->…

based on temperature or solute concentration. The determination of precipitates also come from solubility rules. According to Cooper, almost all sodium, potassium, and ammonium salts are soluble which mean that they will not form a precipitate.1 All chlorides, bromides, iodides, and fluorides, nitrates, chlorates, perchlorates, and acetates, and sulfates are also soluble. The only exceptions are as follows: Ag+, Hg2+, Pb2+, Mg2+, Ca2+, Sr2+, Ba2+, Pb2+. For week three, the goal was to determine…

two-part experiment meant to have us practice our skills and then use those skills in actual data collection and analysis. In part one we used a sample of sodium saccharinate combined with a sample of a metal halide salt, our group used copper(II) chloride. The combination of these two samples allowed for the synthesis of a metal complex. In part two of the experiment we used a procedure similar to part one in order to collect phosphorus out of a sample of fertilizer. This sample was then…

However, the resulting solution was a lot more basic. Reacting the unknown compound with sodium nitrate (NaNO3), a salt, did not have a visible reaction nor did the pH of the resulting solution change. The last reaction involved the unknown compound and silver nitrate (Ag(NO3)2), another salt. A milky, white precipitate was produced (AgCl2) and there was no change in pH. After performing these reactions, it was apparent that our unknown compound (KCl) was not very reactive. There were some…

and barium chloride. If a sulfate anion was present in the unknown solution, then the anion would combine with the barium and form the precipitate, BaSO4, and the chlorine ion would combine with the unknown’s cation. In this case a sulfate anion was present in the unknown so the sulfate combined with barium in the form of a precipitate, and the potassium combined with the chloride ion as an aqueous solution. The same fundamentals are used when testing for a chloride anion. If a chloride anion…