Determination of Ka for a weak Acdi Essay

IntroductionIn the experiment preformed the objective is to quantify a weak battery- sharp with a stiff 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 give occur is the pass transfer of protons from the weak acid to the hydroxide ion. The data gathered will be represented on the titration trim back, a represent of the volume of titrant universe the strong base plotted against the pH .The pH is an indicator of an acids strength. The titration curve tush be used to determine the pKa. By reading the graph the equivalence point can be found which is the point where pertain parts acid and base have reacted by knowing this the one-half-equivalence can be found pH=pKa.ProcedureIn the experiment pH paper will be used instead of a pH meter. The pH will be set at the beginning and the obliterate of the titration and the data table will be used to calculate the liaise values. A burette is a more accurate piece of glasswork used to deliver the titrate in the lab being performed available pipet will be used making it very central to consistently dispense the same size completes. Before the titration the volume of a drop must be determined. A pipet is completely ingest with distilled water. The average image of drops in a mL and the average measure of a mL represented by on drop is metric and recorded. Water is added drop by drop to a graduated piston chamber from a pipet at the first, second and third mL lines the water drops are recorded. The average number of drops are calculated per mL. The average of the cadence of a mL represented by a drop is as well recorded.A data table is set up to represent the racetrack averages. First 2.0 mL of unknown acid is measured into graduated cylinder and thus poured into a beaker the volume is the recorded. By using a toothpick a drop of acid is placed onto low portion of pH paper, the pH level is recorded. One drop of the ph enolphthalein indictor is added to the acid and the color is recorded. The beaker is set on a white sheet of paper before moving on. Next, a well in the 24-well plate is filled with NaOH solution and then sucked up into anempty pipet. The pipet is the held vertically slowly adding drop by drop the NaOH into the beaker of the unknown solution. Drops are added until a color change occurs, changing to a faint pink for at least 30 seconds. A shaping spoon is used to stir after the addition of each drop. The number of drops of NaOH is recorded and the equivalence point is now determined. A drop of the acid is now transferred by toothpick to the high range pH indicator strip. The pH level of the acid is recorded before titration. The contents of the beaker are poured cut out the drain and all equipment is thoroughly cleaned. The above procedure is repeated twice more, all data is recorded to 4 decimal places for each hale on the data table. The average of the 3 trails is calculated an d data is recorded.At the top of the pH column the unknowns acids starting pH level before titration is entered. Next, the pH level of the acid after the titration, at its equivalence point is entered at the bottom of the pH column. The appropriate pH levels for each 2 drop interval is then calculated, by subtracting the initial pH from the final pH and dividing the resulting difference by the number of rows minus 1. This number is then added to the previous pH value.A graph is then made, pH is plotted on the y axis vertebra and volume of NaOH added on the x axis. This represents the titration curve. The pH that corresponds with the equivalence point and half equivalence points are located and the pKa is determined for the unknown acid, pH=pKa. The Ka is determined by taking the inverse log of the pKa(10-pka).