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Equilibrium Constant from Nernst Equation

EMF of the ce...

Question

EMF of the cell, $A g | A g N O_{3} (0.1 M) | K B r (1 N), A g B r (s) | A g$ is $- 0.6 V$ at $298 K$
Calculate the $K_{s p}$ of $A g B r$ at $298 K$ .

K_{s p} = 4.0 \times 10^{- 12}

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K_{s p} = 3.5 \times 10^{- 12}

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K_{s p} = 4.8 \times 10^{- 12}

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K_{s p} = 3.8 \times 10^{- 12}

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Solution

The correct option is C $K_{s p} = 4.8 \times 10^{- 12}$
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Similar questions

A g | A g N O_{3} (0.1 M) | K B r (1 N), A g B r (s) | A g

- 0.6 V

298 K

K_{s p}

A g B r

298 K

A g | A g N O_{3} (0.1 M) | K B r (1 N), A g B r (s) | A g

- 0.6 V

298 K

K_{s p}

A g B r

298 K

A g B r (s)

5 \times 10^{- 13}

298 K

E_{B r^{-} | A g B r | A g}^{0}

0.07 V

E_{A g^{+} / A g}^{0}

A g (s)

A g N O_{3} (a q, 0.1 M)

C u (s)

C u S O_{4} (a q, 4 M)

298 K

E_{A g^{+} / A g}^{0} = 0.80 V

E_{C u^{2 +} / C u}^{0} = 0.34 V

The solubility product of a saturated solution of $A g_{2} C r O_{4}$ in water at 298 K will be................., if the EMF of the cell:

A g | A g^{\oplus} (s a t A g_{2} C r O_{4} s o l) | | A g (0.1 M) | A g

0.164 V

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