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Oxidation and Reduction

A 5.0 mmol dm...

Question

A $5.0 {mmol dm}^{- 3}$ aqueous solution of $K C l$ has a conductance of $0.55 m S$ when measured in a cell of cell constant $1.3 {cm}^{- 1}$ . The molar conductivity of this solution is $(m S) m^{2} {mol}^{- 1}$ . (Round off to the nearest integer).

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Solution

$G_{K C l} = 0.55 mS = 55 \times 10^{- 5} S$
Cell constant $= \frac{l}{A} = 1.3 {cm}^{- 1}$

$K = G (\frac{l}{A}) = 55 \times 10^{- 5} \times 1.3 S c m^{- 1}$
$λ_{M} = \frac{K \times 1000}{Molarity} = \frac{55 \times 1.3 \times 10^{- 5} \times 1000}{5 \times 10^{- 3}}$
$λ_{M} = 11 \times 1.3 \times 10 = 11 \times 13 = 143 {Scm}^{2} {mol}^{- 1}$
$λ_{M} = \frac{143 S}{(10^{- 2} m)^{- 2}} {mol}^{- 1}$
$λ_{M} = 143 \times 1000 \times 10^{- 4} (m S) m^{2} . m o l^{- 1}$
$λ_{M} = 14.3 (m S) m^{2} . {mol}^{- 1}$
Nearest integer $= 14$

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