The solubility of Ag2C2O4 in acidified water of pH-5 is 2-46-10-x- The value of -x- is- Given- Ka1-5- 10-2- Ka2- 5-10-5 for oxalic acidKsp of Ag2C2O4 - 5-10-11-120-004 -4-93

Ag_2C_2O_4→ 2Ag^+ + C_2O^2 _4 .....(1) K_sp= [Ag^+]^2× [C_2O_4^2 ] = 5× 10^ 11 C_2O_4^2 +H_2O→ OH^ +HC_2O^ _4 HC_2O^ _4+H_2O→ OH^ +H_2C_2O_4 [C_2O^2 _4]_0=[A ...

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Byju's Answer

Standard XII

Chemistry

Solubility Product

The solubilit...

Question

The solubility of $A g_{2} C_{2} O_{4}$ in acidified water of $p H = 5$ is $2.46 \times 10^{- x}$ . The value of ' $x$ ' is:
$(Given: K a_{1} = 5 \times 10^{- 2}, K_{a_{2}} = 5 \times 10^{- 5} for oxalic acid$
$K_{s p} of A g_{2} C_{2} O_{4} = 5 \times 10^{- 11}, \sqrt[3]{120.004} = 4.93)$

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Solution

$A g_{2} C_{2} O_{4} \to 2 A g^{+} + C_{2} O_{4}^{2 -} . . . . . (1)$
$K_{s p} = [A g^{+}]^{2} \times [C_{2} O_{4}^{2 -}]$ = $5 \times 10^{- 11}$
$C_{2} O_{4}^{2 -} + H_{2} O \to O H^{-} + H C_{2} O_{4}^{-}$
$H C_{2} O_{4}^{-} + H_{2} O \to O H^{-} + H_{2} C_{2} O_{4}$

$[C_{2} O_{4}^{2 -}]_{0} = \frac{[A g^{+}]}{2} = [C_{2} O_{4}^{2 -}] + [H C_{2} O_{4}^{-}] + [H_{2} C_{2} O_{4}]$
$(∵ [C_{2} O_{4}^{2 -}]_{0} is the initial concentration)$
$= [C_{2} O_{4}^{2 -}] + \frac{[H^{+}] [C_{2} O_{4}^{2 -}]}{K a_{2}} + \frac{[C_{2} O_{4}^{2 -}] [H^{+}]^{2}}{K a_{1} K a_{2}}$
$= [C_{2} O_{4}^{2 -}] [1 + \frac{10^{- 5}}{5 \times 10^{- 5}} + \frac{10^{- 10}}{25 \times 10^{- 7}}]$

$\frac{[A g^{+}]}{2} = \frac{K_{s p}}{[A g^{+}]^{2}} [1.20004]$
$[A g^{+}]^{3} = 2 \times K_{s p} \times [1.20004]$
$[A g^{+}]^{3} = 2 \times 5 \times 10^{- 11} \times [1.20004]$
$[A g^{+}]^{3} = 10^{- 10} \times [1.20004]$
$[A g^{+}]^{3} = 10^{- 12} \times [120.004]$
$[A g^{+}] = 10^{- 4} \times [4.932]$
$Solubility = \frac{[A g^{+}]}{2} = 10^{- 4} \times \frac{4.932}{2} = 10^{- 4} \times 2.46$

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Similar questions

Q. The solubility of

A g_{2} C_{2} O_{4}

in acidified water of

p H = 5

2.46 \times 10^{- x}

. The value of '

x

' is:

(Given: K a_{1} = 5 \times 10^{- 2}, K_{a_{2}} = 5 \times 10^{- 5} for oxalic acid

K_{s p} of A g_{2} C_{2} O_{4} = 5 \times 10^{- 11}, \sqrt[3]{120.004} = 4.93)

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The solubility of Ag2C2O4 in acidified water of pH=5 is 2.46×10−x. The value of 'x' is: (Given: Ka1=5×10−2,Ka2=5×10−5 for oxalic acid Ksp of Ag2C2O4=5×10−11,3√120.004=4.93)

The solubility of $A g_{2} C_{2} O_{4}$ in acidified water of $p H = 5$ is $2.46 \times 10^{- x}$ . The value of ' $x$ ' is:
$(Given: K a_{1} = 5 \times 10^{- 2}, K_{a_{2}} = 5 \times 10^{- 5} for oxalic acid$
$K_{s p} of A g_{2} C_{2} O_{4} = 5 \times 10^{- 11}, \sqrt[3]{120.004} = 4.93)$