Which of the graphs shown below would best re | vedclass

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(A) The titration involves two steps: $1$. $HCl$ is a strong acid and reacts first with $NaOH$: $H^+ + Cl^- + Na^+ + OH^- \rightarrow H_2O + Na^+ + Cl

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(A) The titration involves two steps: $1$. $HCl$ is a strong acid and reacts first with $NaOH$: $H^+ + Cl^- + Na^+ + OH^- \rightarrow H_2O + Na^+ + Cl^-$. The highly mobile $H^+$ ions are replaced by $Na^+$ ions,leading to a decrease in conductance.$2$. After $HCl$ is neutralized,$HCN$ (a weak acid) reacts with $NaOH$: $HCN + Na^+ + OH^- \rightarrow CN^- + Na^+ + H_2O$. The concentration of ions increases as $HCN$ is converted to $Na^+ + CN^-$,leading to a slight increase in conductance.$3$. After both acids are neutralized,adding excess $NaOH$ adds $Na^+$ and $OH^-$ ions,causing a sharp increase in conductance.Therefore,the graph shows a decrease,then a slight increase,followed by a sharp increase. This matches the pattern in Graph $A$.

Which of the graphs shown below would best represent the change in conductance $(G_{sol})$ when a solution containing $0.1 \, M$ each of $HCl$ and $HCN$ is titrated with $0.1 \, M$ $NaOH$ solution?

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