The concentration of Ag - ions in a given saturated solution of AgCl at 25 0 C is 1-06- 10 -5gm ion litre- The solubility product of AgCl is-

The correct option is C 1.12× 10 ^ 10 AgCl dissociates as, AgCl → Ag^++Cl^ #160; #160; #160; #160; #160; #160; #160; # ...

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Standard XII

Chemistry

Solubility Product

The concentra...

Question

The concentration of ${A g}^{+}$ ions in a given saturated solution of $A g C l$ at $25^{0} C$ is $1.06 \times 10^{- 5}$ gm ion litre. The solubility product of $A g C l$ is:

0.353 \times 10^{- 10}

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0.53 \times 10^{- 10}

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1.12 \times 10^{- 10}

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2.12 \times 10^{- 10}

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Solution

The correct option is C $1.12 \times 10^{- 10}$
$A g C l$ dissociates as,
$A g C l \to A g^{+} + C l^{-}$
$s$ $s$
where $s$ is solubility of that particular ion.
Hence,
$K_{s p} = [A g^{+}] [C l^{-}] = s^{2}$

$= (1.06 \times 10^{- 5})^{2}$

$⟹ K_{s p} = 1.12 \times 10^{- 10}$

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Similar questions

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The concentration of Ag+ ions in a given saturated solution of AgCl at 250C is 1.06×10−5gm ion litre. The solubility product of AgCl is:

The correct option is C 1.12×10−10AgCl dissociates as,AgCl→Ag++Cl− s swhere s is solubility of that particular ion.Hence,Ksp=[Ag+][Cl−]=s2 =(1.06×10−5)2⟹Ksp=1.12×10−10

The concentration of ${A g}^{+}$ ions in a given saturated solution of $A g C l$ at $25^{0} C$ is $1.06 \times 10^{- 5}$ gm ion litre. The solubility product of $A g C l$ is:

The correct option is C $1.12 \times 10^{- 10}$
$A g C l$ dissociates as,
$A g C l \to A g^{+} + C l^{-}$
$s$ $s$
where $s$ is solubility of that particular ion.
Hence,
$K_{s p} = [A g^{+}] [C l^{-}] = s^{2}$

$= (1.06 \times 10^{- 5})^{2}$

$⟹ K_{s p} = 1.12 \times 10^{- 10}$