HCl (aq) + H2O (l) ↔ Cl- (aq) + H3O+ (aq)
Net ionic: HCl (aq) ↔ Cl- (aq) + H+ (aq)
From the experimental data, the [H+] decreases as the concentration of the HCl in each solution decreases. Since acids dissociate in water, the dilution of the acid’s concentration (Macid) will determine the number of free hydrogen ions in the solution, being that they are equal to each other when the -log is used. By changing the concentration of the HCl, the acid strength decreases, as shown in the change in pH, due to the presence of H+ ions as they break away from the original molecules of the acid. These free ions are in the form of hydronium ions, which shows in the decrease of the H+ in the table above.
The data collected indicates that the HCl is a strong acid, since the acid dissociates nearly completely in water. A strong acid is termed to be one that completely ionizes in a solution and as shown, its hydrogen ion concentration changed with the increase of dilution due to the dissociation of the HCl molecules. The H+ was equal to that of the concentration of the HCl.
The HCl does dissociate completely in water, as it is a strong acid and strong electrolyte. When combining the two solutions, heat was given off, indicating an exothermic reaction between the water and HCl. A strong electrolyte will dissolve completely in a solution with its ions, which would explain the decrease in the amount of hydrogen ions that changed when the solution was dissociating ions due to the reaction with the water molecules.
For the Acetic Acid
HC2H3O2 (aq) + H2O (l) ↔ C2H3O2- (aq) + H3O+ (aq)
HC2H3O2 (aq) ↔ C2H3O2- (aq) + H+ (aq)
From the experimental data, the hydrogen ion concentration of the acetic acid in each solution the [H+] dec...
... middle of paper ...
...r the solution formed during hydrolysis will be more acidic or more basic. The interactions of the cations and anions in the solution affect how the reaction will proceed, based on if a proton will be donated or accepted. A strong acid and base will only neutralize each other due to no interaction between ions in the solution. A strong acid and a weak base would form an acidic solution, as the cations would donate protons and a weak acid and a strong base would form a basic solution, as the anions accept protons. Certain metallic cations will also form an acidic solution due to the polarization of the OH molecule when one of the protons of the cation is donated. Overall, the pH ultimately proves the state of a solution and can change based on the concentration of the solution made. Color indicators can help in finding the range to narrow to the correct value for pH.
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