What is the minimum silver ion concentration required to initiate the precipitate of silver bromate from 0.01 M potassium bromate
KBrO3 is a salt soluble in water that ionizes 100%; ie.,
..........KBrO3==> K^+ + BrO3
I.........0.01.....0......0
C........-0.01....0.01....0.01
E..........0......0.01....0.01
.........AgBrO3 --> Ag^+ + BrO3^-
I........solid......0......0.01
C........solid......x.......x
E........solid......x.....0.01+x
Then Ksp AgBrO3 = (Ag^+)(BrO3^-)
Look up Ksp and substitute the E line into Ksp expression and solve for x = (Ag^+).
To determine the minimum silver ion concentration required to initiate the precipitate of silver bromate from 0.01 M potassium bromate, we need to understand the concept of solubility product constant (Ksp).
The solubility product constant (Ksp) is an equilibrium constant that describes the solubility of a sparingly soluble compound in a solvent. It represents the product of the concentration of the ions in a saturated solution, each raised to the power of its stoichiometric coefficient.
In the case of silver bromate (AgBrO3), it dissociates into silver ion (Ag+) and bromate ion (BrO3-):
AgBrO3(s) ⇌ Ag+(aq) + BrO3-(aq)
The solubility product constant expression for this reaction can be written as:
Ksp = [Ag+][BrO3-]
Given that the concentration of potassium bromate (KBrO3) is 0.01 M, we need to find the minimum silver ion concentration ([Ag+]) at which the product of its concentration and the bromate ion concentration will exceed the Ksp value.
First, we need to find the concentration of bromate ions ([BrO3-]) in the solution. Since potassium bromate dissociates into one bromate ion for each potassium bromate molecule, the concentration of bromate ions is the same as the concentration of potassium bromate: 0.01 M.
Now, we need to solve for the silver ion concentration ([Ag+]) using the Ksp expression:
Ksp = [Ag+][BrO3-]
To find the minimum silver ion concentration, we take the square root of Ksp and divide it by the concentration of bromate ions:
[Ag+] = (Ksp/[BrO3-])^(1/2)
Substituting the values, we get:
[Ag+] = (Ksp/0.01)^(1/2)
Please note that the value of Ksp for silver bromate would need to be provided in order to calculate the minimum silver ion concentration.