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In the conductometric titation of HCl vs NaOH, the conductance initially decreases, reaches a minimum at equivalence point, and then the slope of the curve becomes positive:

Source: https://chart-studio.plotly.com/~ramesh.ammanamanchi/25/conductometric-titration-curve/#/plot

How can this be modelled like I could do for pH?


Edit: This is my attempt. Is it correct?

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    $\begingroup$ The site expects that you write explicit compact summary of your prior effort to answer the question, based on your knowledge and on searching for existing related info or answers. It would prevent others to tell you what you already know or what you could easily find yourself. $\endgroup$
    – Poutnik
    Jun 11 at 17:44
  • $\begingroup$ I don't know where to start. Will Kohlrausch law be applicable here? $\endgroup$
    – Shub
    Jun 11 at 18:10
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    $\begingroup$ The start is to understand underlying chemistry.. Modelling comes after. You must know, what you are modelling. Ongoing reactions and conductivity related laws. $\endgroup$
    – Poutnik
    Jun 11 at 18:16
  • $\begingroup$ You should use your effort to solve this problem before we can intervene. You should also think about following facts: Must use dilute aqueous solutions; The ion mobility is dependent on temperature so make sure temperature didn't increase during the titrarion (strong acid/base reaction is exothermic); Also, if your model is for weak acid or base, their ka or kb is also temperature dependent. $\endgroup$ Jun 11 at 21:48
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    $\begingroup$ Just from looking at the image without distracting information like correct labels on the graph it should be almost painfully obvious: linear fit on the left and the right, where they intersect is the equivalence point. $\endgroup$ Jun 13 at 2:31

1 Answer 1

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Expressed in $\pu{\Omega ^{-1} cm^2 mol^{-1}}$, the ionic conductance of usual ions like $\ce{Na+, K+, Ca^{2+}, Cl-, SO4^{2-}}$ are between $50$ and $80$. But the two ions $\ce{H+}$ and $\ce{OH-}$ have a rather high conductivity : $350$ for $\ce{H+}$ and $198$ for $\ce{OH-}$. This property explain the change of the conductance observed in the titration of $\ce{HCl}$ solution by $\ce{NaOH}$.

In the beginning of the titration, [$\ce{H+}$] is large. So the conductance of the solution is large. When adding $\ce{NaOH}$, the ion $\ce{H+}$ is replaced by the ion $\ce{Na+}$ which has a poor conductivity : the conductance of the solution decreases.

At the equivalence point, the conductance is low, as it is only due to the ions $\ce{Na+}$ and $\ce{Cl-}$. If more $\ce{NaOH}$ is added after the equivalence point, the aded ions $\ce{OH-}$ aren't destroyed and stay in the solution. So its conductance increases. This is what you have observed experimentally.

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  • $\begingroup$ Thank you for the explanation :) Have I done this correctly? $\endgroup$
    – Shub
    Jun 12 at 11:10

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