6.03 Calorimetry Lab Report Conclusion

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The purpose of this experiment was to determine the identity of nine solutions using the results of reacting pairs of solutions in an organized systematic manner. Known solutions were used on the first day. The second day, the solutions were placed in code-labeled bottles. The reactions from the previous day were then used to help identify which solutions were which, by closely monitoring which unknown solutions mixed with other unknowns and how they reacted, such as: color changes, precipitates, and gases. Those that did not have reactions were also useful in the deduction process.

To fully understand how this elimination process works, one must have a better conceptual understanding of aqueous solutions, acid-base reactions, precipitates, and the solubility rules. An aqueous solution is any solution in which water is the solvent. Simply put, it dissolves in water. In order for a substance to dissolve in water, it must either match or exceed the strong attractive forces that water molecules generate between themselves. Those solutions that cannot do so form precipitates. Precipitates are defined as “insoluble ionic products of a reaction, formed when certain cations and
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A bicarbonate is considered an acid-base neutralization reaction. Compounds with carbonate and bicarbonate ions are considered bases because they accept hydrogen ions from acid molecules, thus neutralizing the acid. This is very similar to an acid-base neutralization reaction, the only difference being that this produces a carbon dioxide gas, as well as water and salt. Similarly, when a metal sulfite and an acid are mixed, it produces water, salt, and a sulfur dioxide gas, as opposed to carbon dioxide. Both a metal sulfide and acid-base reaction, and an ammonium salt and strong base reaction, produce a hydrogen sulfide gas and a salt. (LHS AP Chemistry,

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