ACID-BASE PROPERTIES OF SODIUM CHLORIDE, SODIUM FORMATE AND AMMONIUM CHLORIDE
INTRODUCTION
The objective of this experiment is to examine the definitive characteristics of acids and bases by investigating the characteristics of strong versus weak acids; more specifically, why these differences are important in the process of titrations. In this experiment, there are two titrations performed and measured the pH of one salt solution. This experiment includes a strong acid and strong base titration, weak acid and strong base titration, and the pH measure of a salt solution. In performing a titration, a stir-bar, stir-plate, burette and pH meter. In the process of titration, it is required that the amounts of base added from the burette is as …show more content…
The first part of the experiment proved to be successful as the pH at the equivalence point was 7.21. This is a successful titration because in a strong acid and strong base titration, the equivalence point should be ~7. Since HCl fully dissociates into H_3 O^+ and 〖Cl〗^- and NaOH fully dissociates into 〖Na〗^+ and 〖OH〗^-, by forces of electrostatic attraction, the H_3 O^+ and 〖OH〗^- will combine to produce H_2 O and 〖Na〗^+ and 〖Cl〗^- will combine to produce NaCl. At the equivalence point, it is found that 〖[H〗_3 O^+] = 〖[OH〗^-]. Since both molecules fully dissociate, at the equivalence point, there are no other products than NaCl and H_2 O. Since the salt was a negligible pH, the pH that is being measured is H_2 O, which is pH = …show more content…
Both titrations in this lab reflected these properties, such as acid-dissociation, acid-dissociation constants, etc. In parts A and B, it demonstrated the differences between strong and weak acids and why there is a significant difference between equivalence points, as one value was 7.21 and why the other was 8.38. Regardless that the pH differences are not dramatic, it is important to acknowledge the reasons why pH values occur as they do at the different stages of titration – pre-titration, buffer region and hydrolysis. Lastly, all pH’s are reflected by the concentration of hydronium ions in a solution, which is determined by the salt solution itself and its reactions with water. Just as in ammonium chloride, the solution has two possibly reactive ions with water and must evaluate and compare the equilibrium constants to determine the effect of the pH of the
INTRODUCTION
The objective of this experiment is to examine the definitive characteristics of acids and bases by investigating the characteristics of strong versus weak acids; more specifically, why these differences are important in the process of titrations. In this experiment, there are two titrations performed and measured the pH of one salt solution. This experiment includes a strong acid and strong base titration, weak acid and strong base titration, and the pH measure of a salt solution. In performing a titration, a stir-bar, stir-plate, burette and pH meter. In the process of titration, it is required that the amounts of base added from the burette is as …show more content…
The first part of the experiment proved to be successful as the pH at the equivalence point was 7.21. This is a successful titration because in a strong acid and strong base titration, the equivalence point should be ~7. Since HCl fully dissociates into H_3 O^+ and 〖Cl〗^- and NaOH fully dissociates into 〖Na〗^+ and 〖OH〗^-, by forces of electrostatic attraction, the H_3 O^+ and 〖OH〗^- will combine to produce H_2 O and 〖Na〗^+ and 〖Cl〗^- will combine to produce NaCl. At the equivalence point, it is found that 〖[H〗_3 O^+] = 〖[OH〗^-]. Since both molecules fully dissociate, at the equivalence point, there are no other products than NaCl and H_2 O. Since the salt was a negligible pH, the pH that is being measured is H_2 O, which is pH = …show more content…
Both titrations in this lab reflected these properties, such as acid-dissociation, acid-dissociation constants, etc. In parts A and B, it demonstrated the differences between strong and weak acids and why there is a significant difference between equivalence points, as one value was 7.21 and why the other was 8.38. Regardless that the pH differences are not dramatic, it is important to acknowledge the reasons why pH values occur as they do at the different stages of titration – pre-titration, buffer region and hydrolysis. Lastly, all pH’s are reflected by the concentration of hydronium ions in a solution, which is determined by the salt solution itself and its reactions with water. Just as in ammonium chloride, the solution has two possibly reactive ions with water and must evaluate and compare the equilibrium constants to determine the effect of the pH of the