Solution- A) Ag2SO3 <--> 2Ag+(aq) + SO3-2 (aq) this is an equilibrium Ksp = [Ag+

Question

Solution- A)  Ag2SO3 <--> 2Ag+(aq) + SO3-2 (aq)

this is an equilibrium

Ksp = [Ag+]^2[SO3-2]

If ksp = 1.5x10^-15

Let us assume that s is the solublity, therefore there are 2x ag ions

[Ag+] = 2s

and 1:1 SO3 ions per mol of AG2SO3

[SO3-2] = s

Substitute in Ksp

KsP = (2s)^2 s

1.5x10-15 = 4s^3

s = 1.25*10^-16 mol per liter

B) Ksp = [Ag]²[SO3--]
For every x moles of Ag2SO3 that dissolves in a liter of water, the concentration of Ag+ is 2x Molar, and the concentration of SO3-- is x Molar. Therefore,
Ksp = (2x)²(x) = 4x³ = (4)(1.5 x 10^-15 M)³ = 1.35 x 10^-44 M³

Explanation / Answer

4 marks 4. Calculate the molar solubility of Ag SO, (Kup1.5 x 10-15) a. in a solution buffered to a pH of 6.50. b. in water.

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