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The conductivity ofa solution may be tak...

The conductivity ofa solution may be taken to be directly proportional to the total concentration of the charge carriers (ions) present in it in many cases. Using the above, find the percent decrease in conductivity (k) of a solution of a week monoacidic base BOH when its 0.1 M solution is diluted to double its original volume. `(K_(b) = 10^(-5) for BOH) (take `sqrt(50) = 7.07`) (mark the answer to nearest integer)

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The coductivity of a solution may be take to the directly proportional to the total concentration of the charge carriers (ions) present in it in many cases. Using the above fid the percent decrease in conductivity (k) of a solution of a weak monoacidic base BOH when its 0.1 M solution is diluted to double its original volume (K_(b)=10^(-5) for BOH) (take sqrt(50)=7.07 ) (mark the answer to nearest integer)

Why does the conductivity of a solution decrease with dilution?

Knowledge Check

  • Conductivity of a solution is directly proportional to

    A
    Dilution
    B
    Number of ions
    C
    Current density
    D
    Volume of the solution

  • The conductivity of an electrolytic solution decreases on dilution due to

    A
    decrease in number of ions per unit volume
    B
    increase in ionic mobility of ions
    C
    increase in percentage ionisation
    D
    increase in number of ions per unit volume

  • The conductivity of 0.20M solution of KCl at 298K is 0.0248Scm^-1 its molar conductivity is

    A
    `1.24Omega^-1mol^-1cm^2`
    B
    `124Smol^-1cm^2`
    C
    `12.4Omega^-1mol^-1cm^2`
    D
    `0.124Smol^-1cm^2`

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    Which of the following expression for % dissociation of a monoacidic base (BOH) in aqueous solution at appreciable concentration is not correct?

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