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(B) The molar conductivity $(\Lambda_m)$ of an electrolyte depends on its degree of dissociation. For a strong electrolyte,the degree of dissociation

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$X 	o NaCl, Y 	o CH_3COOH$

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(B) The molar conductivity $(\Lambda_m)$ of an electrolyte depends on its degree of dissociation. For a strong electrolyte,the degree of dissociation is already near $100\%$,so dilution causes only a small increase in $\Lambda_m$ due to the reduction in inter-ionic attractions. For a weak electrolyte,dilution significantly increases the degree of dissociation,leading to a sharp increase in $\Lambda_m$. In this case,$X$ shows a small increase ($1.5$ times),indicating it is a strong electrolyte (e.g.,$NaCl$). $Y$ shows a large increase ($20$ times),indicating it is a weak electrolyte (e.g.,$CH_3COOH$). Therefore,$X$ is $NaCl$ and $Y$ is $CH_3COOH$.

Two solutions of electrolytes $X$ and $Y$ are taken in two beakers and diluted by adding $500 \ mL$ of water. The molar conductivity $(\Lambda_m)$ of $X$ increases by $1.5$ times,while that of $Y$ increases by $20$ times. What could be the electrolytes $X$ and $Y$?

Similar Questions

Calculate the cell constant of a conductivity cell containing $0.01 \ M \ AgNO_3$ solution having a resistance of $1440 \ \Omega$ and a conductivity of $0.001262 \ \Omega^{-1} \ cm^{-1}$. (in $cm^{-1}$)

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