The Gravimetric Analysis of Chloride Salt

The hypothesis is correct. Potassium chloride mixed with silver nitrate creates a white precipitate. Barium

First, we were to measure and record the mass of a beaker, then transfer about 1 gram of the salt mixture into the beaker, measure, and record the combined mass. Then, we had to fill a 400-ml beaker with deionized water and test it to make sure that the ph was just basic. We then combined the deionized water and salt by adding about 150ml of the deionized

The color of the solution was turning slightly into yellow and the color of the iron strip into white.

The two most obvious formation of the precipitate were the combinations with the MgSO4. The MgSO4 and NH3 solution became very opaque and the MgSO4 and Na2CO3 turned from liquid to a full solid white substance. The Na2CO3 and CH3COOH did not have as strong of a reaction, however, the precipitates were able to be visualized with in the clear

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

To begin the procedure of the gravimetric analysis of chloride, 0.501g of Amine (C8H9NO) was weighed on an analytical balance and added to a 10mL volumetric flask. At this point 5mL of deionized water was added to dissolve the Amine. Then 5mL of 1 M AgNO3, which was already combined with 4 M HNO3, is added to the 10mL volumetric flask and stirred. To collect the AgCl precipitate,

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

10. Ba (NO3)2, barium nitrate produces pale precipitate when put in reaction with sulfuric acid.

The purpose of this experiment was to find the amount and percent of water in a hydrated salt. Hydrated salt contains water molecules chemically bound to it while anhydrous salt is a substance that fire can readily remove the water molecules. Using the gravimetric analysis method, the sample salt was measured, heated, and was measured again after cooled down to room temperature; this procedure allowed the weight of water lost in the salt to be obtained. After two trials, the water in the salt was determined to have an average percent water of -35.04%. The null hypothesis, the heat will not affect the amount of water lost, was rejected ,however, the alternative hypothesis, the heat will allow for there to be water lost, was not supported.

Finally ensure that your results are accurate. You should have a light blue precipitate remaining when the sodium carbonate reacts with the copper chloride and when sodium sulphate ionises with copper chloride no precipitate should have formed.

then we know Ca2+ is involved in the solution. Next we add OH into the

However, based on the data obtained in Table 1, Figure 1 shows that all of the chemical substances formed a precipitate, while the tertiary substrate 2-chloro-2-methylpropane formed a precipitate the fastest. This makes sense because as a rule in SN1 reactions, the more stable the carbocation is the faster the reaction will occur. Also, SN1 reactions will prefer tertiary substrates to secondary substrates and secondary substrates to primary substrates. The next substrates to form a precipitate were 2-bromobutane followed by 1-bromobutane. However, it was expected that 2-chlorobutane would form a precipitate before 1-bromobutane because 2-chlorobutane is a secondary substrate, and therefore has a more stable carbocation. The reason that this occurred is because bromine is a better leaving group than chlorine, which allows it to bind easier with the silver ion. The reactions that formed the heaviest precipitate were 2-bromobutane, 1-bromobutane, and 2-chloro-2-methylpropane. This is because these reactions occurred at a faster rate and therefore, generated more of a product than 2-chlorobutane and 1-chlorobutane, which only formed a precipitate upon cooling from the warm water bath.

AgNO3 easily undergoes reactions with tertiary alkyl halides (SN1). The four tubes should not all have undergone reactions because that would give an unclear indication whether or not the alkyl halides were primary or tertiary. Two tubes were supposed to undergo reaction and two should not have. It is likely that the error that made the extra two test tubes react was contamination. If the test tubes contained traces of both solvents, it would be possible that the alkyl halides would react in all the test tubes.

Gravimetric analysis is a quantitative (i.e. how much?) method of classical analysis. The element to be determined is isolated in a solid compound of known identity and definite composition. The mass of the element that was present in the original sample can be determined from the mass of this compound.

In the fifth reaction, 2.29 g of zinc was added to the copper (II) sulfate solution under the fume hood. The balanced equation for this reaction is written as followed: