Consider the statements S_1 and S_2:S_1: Cond | vedclass

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(A) Conductivity $(K)$ is defined as the conductance of a unit volume of solution. As the concentration of an electrolyte decreases,the number of ions

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$S_1$ is wrong and $S_2$ is correct

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(A) Conductivity $(K)$ is defined as the conductance of a unit volume of solution. As the concentration of an electrolyte decreases,the number of ions per unit volume decreases,leading to a decrease in conductivity. Thus,$S_1$ is incorrect.Molar conductivity $(\lambda_m)$ is defined as $\lambda_m = \frac{K}{C}$. As the concentration $(C)$ decreases,the volume of solution containing one mole of electrolyte increases significantly,which outweighs the decrease in conductivity $(K)$. Consequently,molar conductivity increases with a decrease in concentration. Thus,$S_2$ is correct.

Consider the statements $S_1$ and $S_2$:
$S_1$: Conductivity always increases with decrease in the concentration of electrolyte.
$S_2$: Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the following is

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What is the $SI$ unit of conductivity?

What is the $SI$ unit of conductivity?

At $25^{\circ} C$,the molar conductances at infinite dilution for the strong electrolytes $NaOH$,$NaCl$ and $BaCl_2$ are $248 \times 10^{-4}$,$126 \times 10^{-4}$ and $280 \times 10^{-4} \ S \ m^2 \ mol^{-1}$ respectively. The value of $\lambda_m^{\circ} Ba(OH)_2$ in $S \ m^2 \ mol^{-1}$ is:

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Consider the statements $S_1$ and $S_2$:$S_1$: Conductivity always increases with decrease in the concentration of electrolyte.$S_2$: Molar conductivity always increases with decrease in the concentration of electrolyte.The correct option among the following is

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Molar conductivities $(\Lambda ^o_m)$ at infinite dilution of $NaCl$,$HCl$ and $CH_3COONa$ are $126.4$,$425.9$ and $91.0 \ S \ cm^2 \ mol^{-1}$ respectively. $(\Lambda ^o_m)$ for $CH_3COOH$ will be .......... $S \ cm^2 \ mol^{-1}$.

What is the $SI$ unit of conductivity?

What is the $SI$ unit of conductivity?

At $25^{\circ} C$,the molar conductances at infinite dilution for the strong electrolytes $NaOH$,$NaCl$ and $BaCl_2$ are $248 \times 10^{-4}$,$126 \times 10^{-4}$ and $280 \times 10^{-4} \ S \ m^2 \ mol^{-1}$ respectively. The value of $\lambda_m^{\circ} Ba(OH)_2$ in $S \ m^2 \ mol^{-1}$ is:

The dissociation constant of $n$-butyric acid is $1.6 \times 10^{-5}$ and the molar conductivity at infinite dilution is $380 \times 10^{-4} \ S \ m^2 \ mol^{-1}$. The specific conductance of the $0.01 \ M$ acid solution is

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Consider the statements $S_1$ and $S_2$:
$S_1$: Conductivity always increases with decrease in the concentration of electrolyte.
$S_2$: Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the following is