We are asked to calculate for the** **calculate K_{sp} of AgBr at 298 K.

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

$\overline{){\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{=}}\frac{\mathbf{RT}}{\mathbf{nF}}{\mathbf{ln}}{\mathbf{}}{\mathbf{K}}}$

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:*

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

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

Br_{2}(l) + 2 e^{-} → 2 Br^{-}(aq) E° = +1.066 V

Use some of the data above to calculate K_{sp} at 298K for AgBr.

a. 2.13x10^{-12}

b. 29.72

c. 4.70x10^{-13}

d. 48.16

e. not enough information is given

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Davis' class at UCF.