Using the Gibbs energy change, \DeltaG° = +63.3 kj, for the following reaction,
Ag2CO3 (s) \rightleftharpoons 2Ag+(aq) + \text{CO}_{3}^{2-}(\text{aq})

The Ksp of Ag2CO3(s) in water at 25oC is: (R = 8.314 J K-1 mol-1)

  • Option 1)

    3.2 x 10-26

  • Option 2)

    8.0 x 10-12

  • Option 3)

    2.9 x 10-3

  • Option 4)

    7.9 x 10-2

 

Answers (1)

As learnt in @9331

We have \Delta G^{\circ} = -2.303 \:RT\: \log \:Ksp

\Rightarrow 63.3 \times 10^{3} = -2.303 \times 8.314 \times 298 \log \:Ksp

\Rightarrow \log \: Ksp = -11.09

\Rightarrow Ksp = 8 \times 10^{-12}


Option 1)

3.2 x 10-26

This option is incorrect

Option 2)

8.0 x 10-12

This option is correct

Option 3)

2.9 x 10-3

This option is incorrect

Option 4)

7.9 x 10-2

This option is incorrect

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