Question

1. Solid silver bromide (AgBr) will disassociate slightly in water to produce Ag and Br. AgBr(s) +- Agtaq) + Braq) Ksp = 1.3 x 10-5 a. Calculate the equilibrium concentration of Ag if the solution if the solid AgBr is dissolved in pure water. Assume that the solution is behaving ideally (y = 1)

Please help me on this multistep problem

Answer 1

Part a.

Ksp = [Ag⁺][Br^-]

i.e. 1.3*10^-5 = s*s

Therefore, the equilibrium concentratin of Ag⁺ (s) = 3.6*10^-3 mol/L

Part b.

ln(k/k₀) = 1.02*Z₊*Z_-*($\mu$)^1/2

i.e. ln(k/k₀) = 1.02*1*(-1)*(0.1)^1/2

i.e. ln(k/k₀) = -0.32255

i.e. k/k₀ = e^-0.32255 = 0.7243

k - in the presence of salt, k₀ - in the absence of salt