Titration Of A Weak Acid Lab Report
Determination of Ka for a Weak Acid
Introduction In the experiment preformed the objective is to titrate a weak acid with a strong base. In a titration of a weak acid with a strong base the titrant is the strong base and the analyte is a weak acid. The reaction that will occur is the direct transfer of protons from the weak acid to the hydroxide ion. The data gathered will be represented on the titration curve, a graph of the volume of titrant being the strong base plotted against the pH .The pH is an indicator of an acids strength. The titration curve can be used to determine the pKa. By reading the graph the equivalence point can be found; which is the point where equal parts acid and base have reacted by knowing this the half-equivalence …show more content…
The relationship between Ka and pKa is that Ka is the equilibrium constant for the dissociation of a weak acid and pKa is the half-equivalence point where pH=pKa. In addition to the pH, Ka is an indication of an acids strength; pKa = - log Ka.
B. The potential sources for errors in this experiment are the inconsistent and miscounting of drops of NaOH in the titration. The pipet must be held upright dispensing the exact size drops to have an accurate measurement.
C. If your experimental Ka is 5.3 and the actual Ka of your unknown acid is 4.7, what is your %
Introduction In the experiment preformed the objective is to titrate a weak acid with a strong base. In a titration of a weak acid with a strong base the titrant is the strong base and the analyte is a weak acid. The reaction that will occur is the direct transfer of protons from the weak acid to the hydroxide ion. The data gathered will be represented on the titration curve, a graph of the volume of titrant being the strong base plotted against the pH .The pH is an indicator of an acids strength. The titration curve can be used to determine the pKa. By reading the graph the equivalence point can be found; which is the point where equal parts acid and base have reacted by knowing this the half-equivalence …show more content…
The relationship between Ka and pKa is that Ka is the equilibrium constant for the dissociation of a weak acid and pKa is the half-equivalence point where pH=pKa. In addition to the pH, Ka is an indication of an acids strength; pKa = - log Ka.
B. The potential sources for errors in this experiment are the inconsistent and miscounting of drops of NaOH in the titration. The pipet must be held upright dispensing the exact size drops to have an accurate measurement.
C. If your experimental Ka is 5.3 and the actual Ka of your unknown acid is 4.7, what is your %