Essay about Ionic Reactions

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

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

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

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

The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.

11. Write the balanced chemical reaction of zinc with HCl (same as problem 5). Is the product of

The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions.

Write a balanced chemical equation for each reaction #1-8. Classify each reaction using the information provided in the

5) Adding NaCl would increase [Cl⁻]. This will cause equilibrium to shift right and the solution would become dark purple.

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.

In part 1, the precipitate that forms is a aluminum hydroxide and in part 2 it is magnesium hydroxide. A precipitate is an insoluble solid that emerges from a liquid solution. When the emergence of the insoluble solid from solution happens, it is called precipitation. The property change in the reactants of the lab are when the water, alum, ammonia, react and create the aluminum hydroxide. When the precipitate is formed, it is an endothermic reaction because the change in the product, aluminum hydroxide, decreases in temperature. This is a chemical reaction because different elements rearrange themselves to form a new substance and while they do so, they either absorb heat or give it

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.

We are given solubility rules, which help us to predict with reactions would form precipitate. Procedure/Experimental First, partners predict which reactions would form precipitate by using the solubility rules as a guide. This resulted in the following reactions

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

The cations in both the known and unknown samples were identified by using qualitative analysis, of which were determined to be acidic, basic, or neutral by using litmus paper. Acid-base reactions, oxidation-reduction reactions, and the formation of complex ions are often used in a systematic way for either separating ions or for determining the presence of specific ions. When white precipitate formed after adding hydroxide, aluminum ion was determined to be present in the solution. However, nickel was determined to test positive when the solution changed to a hot pink color after adding a few drops of dimethylglyoxime reagent and iron was present when the solution was a reddish brown color when sodium hydroxide was added to the mixture at the very beginning of the experiment. Qualitative analysis determines that ions will undergo specific chemical reactions with certain reagents to yield observable products to detect the presence of specific ions in an aqueous solution where precipitation reactions play a major role. The qualitative analysis of ions in a mixture must add reagents that exploit the more general properties of ions to separate major groups of ions, separate major groups into subgroups with reactions that will distinguish less general properties, and add reagents that will specifically confirm the presence of individual