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 = 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:
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.
e. not enough information is given
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