The identity of different unknown solutions can be determined by measuring their respective pH values. Those solutions who possess pH values less than that of 7 is considered as acids, those with pH values greater than 7 are known to be bases, while those having pH equal to 7 is identified as neutral substances (Petrucci, 2011). Identifying its electrolytic property also helps to characterize the given solutions. Strong electrolytes, such as strong acids and bases and salts are known to fully dissociate its ions in the solution, making it a good conductor of electricity. On the other hand, the presence of weak electrolytes, such as weak acids and bases, do not dissociate its ions completely, making the solutions less conductive (Chang, 2010). Solution A was classified to contain strong acid, solution B has a strong base, solution C is said to be neutral, solution D has a weak acid, solutions E and G possess acidic salts, while solution F is said to contain basic salt.
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Ka, or the acid dissociation constant, gives a measure to which an acid dissociates in a solution. It also provides a measure of the strength of an acid. If the value of Ka is high, the said acid s largely dissociated, making the acid strong. However, when the value of Ka is small, the little amount of acid is dissociated, making the acid weak. In the experiment, acetic acid (HOAc), is shown to have a computed Ka of 1.1148 x 10-5. It has a very little value meaning it is considered as a weak acid. Likewise, another measure of equilibrium, the solubility product constant (Ksp) was determined in the experiment. The Ksp of Ca(OH)2 was computed to measure how soluble the substance is in the solution. The computed Ksp of Ca(OH)2 is 2.6791 x 10-5. The higher the Ksp means higher concentrations of ions in the solution, thus having greater solubility in a given
Ka, or the acid dissociation constant, gives a measure to which an acid dissociates in a solution. It also provides a measure of the strength of an acid. If the value of Ka is high, the said acid s largely dissociated, making the acid strong. However, when the value of Ka is small, the little amount of acid is dissociated, making the acid weak. In the experiment, acetic acid (HOAc), is shown to have a computed Ka of 1.1148 x 10-5. It has a very little value meaning it is considered as a weak acid. Likewise, another measure of equilibrium, the solubility product constant (Ksp) was determined in the experiment. The Ksp of Ca(OH)2 was computed to measure how soluble the substance is in the solution. The computed Ksp of Ca(OH)2 is 2.6791 x 10-5. The higher the Ksp means higher concentrations of ions in the solution, thus having greater solubility in a given