Introduction Acid-base titrations are used to calculate properties of an acid or a base by titrating them with a strong Acid or base. In a titration, certain amount of volume of one substance usually a strong acid or base, a titrant, is added to another substance, an acid or base of some kind, until a change in properties are observed. Strong acids and bases are used because they allow the neutralization reaction between the acid and base into salt to go to completion. By titrating an unknown concentration of acid or base with a known concentration of acid or base, you can calculate properties such as the concentration and pKa of the analyte. During the standardization part of this reaction, we are adding Sodium Hydroxide, NaOH to a solution
…show more content…
The concentrations are very precise, with an extremely small standard deviation. Error could have resulted from accidently going past the equivalence point of the reaction, after the indicator changed colors, or from an incomplete transfer of the acidic salt into the analyte solution.
Discussion of Titration of Cola:
The objective of part B was to calculate the pH of a sample of cola by titrating it with a known concentration of a strong base measuring the pH with a pH probe.
The first equivalence point was at the addition of 9.25 mL of NaOH at a pH of 4.19. The second equivalence point was at the addition of 25.75 mL of NaOH at a pH of 8.63. The equivalence points were identified by locating the local maximums of the change in pH per volume of titrant.
(A19+A18)/2 was the formula used to calculate the avg. volume of titrant added per data point.
The initial pKa, pKa1 was calculated to be 1.46.
The formula used to calculate the initial concentration of H3PO4 was ((F30*F9)/(C13)).
The formula to calculate the pKa1 was
The concentrations are very precise, with an extremely small standard deviation. Error could have resulted from accidently going past the equivalence point of the reaction, after the indicator changed colors, or from an incomplete transfer of the acidic salt into the analyte solution.
Discussion of Titration of Cola:
The objective of part B was to calculate the pH of a sample of cola by titrating it with a known concentration of a strong base measuring the pH with a pH probe.
The first equivalence point was at the addition of 9.25 mL of NaOH at a pH of 4.19. The second equivalence point was at the addition of 25.75 mL of NaOH at a pH of 8.63. The equivalence points were identified by locating the local maximums of the change in pH per volume of titrant.
(A19+A18)/2 was the formula used to calculate the avg. volume of titrant added per data point.
The initial pKa, pKa1 was calculated to be 1.46.
The formula used to calculate the initial concentration of H3PO4 was ((F30*F9)/(C13)).
The formula to calculate the pKa1 was