Answer:
[tex]\begin{array}{l}{\text { The mistake of adding less amount of as assigned distilled water will not affect the acid }} \\ {\text { dissociation constant value " } \mathrm{k}_{\mathrm{a}} \text { " as determined in Part-B. }}\end{array}[/tex]
Explanation:
The quantitative measurement of strength of an acid in solution named as acid dissociation constant [tex]^{\prime \prime} \mathrm{K}_{2}^{\prime \prime}[/tex]. For acid-base titration this analysis is preferred and it is equilibrium constant for a chemical reaction. [tex]\mathrm{k}_{\mathrm{a}}[/tex]is constant despite of concentration, for example it measures breakdown of an acid into the conjugate base [tex]\mathrm{A}^{-}[/tex]and hydrogen ion [tex]\mathrm{H}^{+} \text {in following equation: }[/tex]
[tex]\mathrm{HA} \leftrightarrow \mathrm{H}^{+}+\mathrm{A}^{-}[/tex]
[tex]\underline{\mathbf{k}}_{\mathbf{a}}=\frac{\left[\mathrm{H}^{+}\right] \cdot[\mathrm{A}]}{[\mathrm{HA}]}[/tex]
Here amount of [tex]\mathrm{H}^{+}[/tex]produced is proportional to the amount of H-A from which started. Therefore amount of [tex]\mathbf{k}_{\mathbf{a}}[/tex]remain constant for a particular acid despite a change in concentration of both acid or base with which it is reacting.
