Problem: Ag+(aq) + e- → Ag(s)                       E° = +0.800 VAgBr(s) + e- → Ag(s) + Br-(aq)         E° = +0.071 VBr2(l) + 2 e- → 2 Br-(aq)                   E° = +1.066 VUse some of the data above to calculate Ksp at 298K for AgBr.a. 2.13x10-12b. 29.72c. 4.70x10-13d. 48.16e. not enough information is given

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We are asked to calculate for the calculate Ksp of AgBr at 298 K.


Recall that the Nernst Equation relates the concentrations of compounds and cell potential.

E°cell=RTnFln K

E°cell = cell potential, V
R = gas constant = 8.314 J/(mol
·K)
T = temperature, K
n = mole e- transferred
F = Faraday’s constant, 96485 C/mol e-
K = equilibrium constant


Since the AgBr is an ionic compound, it will form ions when dissociating in water. The dissociation of AgBr in water is as follows:

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Problem Details

Ag+(aq) + e- → Ag(s)                       E° = +0.800 V

AgBr(s) + e- → Ag(s) + Br-(aq)         E° = +0.071 V

Br2(l) + 2 e- → 2 Br-(aq)                   E° = +1.066 V

Use some of the data above to calculate Ksp at 298K for AgBr.

a. 2.13x10-12
b. 29.72
c. 4.70x10-13
d. 48.16
e. not enough information is given

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