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Standard X

Chemistry

Electrolysis and Electrolytes

The specific ...

Question

The specific conductance at $25^{\circ} C$ of a saturated solution of $S r S O_{4}$ is $1.482 \times 10^{- 4} o h m^{- 1} c m^{- 1}$ . Molar ionic conductance of $S r^{2 +}$ and $S O_{4}^{2 -}$ ions at infinite dilution are 59.46 and $79.8 o h m^{- 1} c m^{2} m o l e^{- 1}$ respectively. $[S r = 87.6, S = 32, O = 16]$
If the concentration in (g/L) is $1934 \times 10^{- x}$ , then what is the value of $x ?$

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Solution

$Λ_{S r S O_{4}}^{\infty} = λ_{S r^{2 +}}^{\infty} + λ_{S O_{4}^{2 -}}^{\infty} = 59.46 + 79.8 = 139.26 o h m^{- 1} c m^{2} m o l^{- 1}$

$Λ = \frac{1000 κ}{C}$

$139.26 o h m^{- 1} c m^{2} m o l^{- 1} = \frac{1000 \times 1.482 \times 10^{- 4} o h m^{- 1} c m^{- 1}}{C}$

$C = 1.064 \times 10^{- 3} M$

The molar mass of strontium sulphate is $87.6 + 32 + 4 (16) = 183.6 g / m o l$

The concentration of strontium sulphate in g/L is $1.064 \times 10^{- 3} M \times 183.6 g / m o l = 0.1934 g / L = 1934 \times 10^{- 4}$
$x = 4$
Ans- $4$

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