posted by faruk on .
You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point.
The pH of the other half of the original solution is measured with a pH meter. The "neutralized" solution is added to the "original" solution and the pH of this combined "final" solution is also measured.
The following are the measured values:
Mass of unknown acid 1.6214 g
Volume of NaOH used in titration 15.88 mL
Concentration of the NaOH used 0.1849 M
pH of the original acid solution 2.64
pH of the final acid solution 4.45
CALCULATE the following
(a) Molecular Weight of Acid used in titration ___________________
(b) Molarity of UNKNOWN Acid solution from titration ___________________
(c) Ka of UNKNOWN Acid ___________________
(d) Concentration of undissociated Acid from pH measurements ___________________
(e) Total concentration of UNKNOWN acid from pH measurements ___________________