Calculate the saturation indices of this solution. Then classify as: undersaturated, supersaturated, or in equilibrium. Why? Saturation state with respect to: “Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM
Calculate the saturation indices of this solution.
Then classify as: undersaturated, supersaturated, or in equilibrium. Why?
Saturation state with respect to:
“Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM
![**Saturation State with Respect to Amakinite (Fe(OH)₂):**
- **Iron Concentration ([Fe²⁺]):** 0.1 mM
- **Hydroxide Concentration ([OH⁻]):** 0.0001 mM
This text describes the saturation state for the mineral "Amakinite," represented chemically as Fe(OH)₂. It specifies the concentrations of iron ions (Fe²⁺) and hydroxide ions (OH⁻) in the solution. Understanding these concentrations is essential for determining the solubility and precipitation conditions of the mineral in various environments.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50bf679e-c229-490b-91d0-8a5b8f84bb57%2F4d76c104-2681-4e15-962c-5c8caa521f49%2F78e62lo_processed.jpeg&w=3840&q=75)
Solution -
According to the question -
Given -
In order to determine if an ionic mixture is undersaturated, supersaturated or in equilibrium, we have to calculate the ionic product (Q) of the mixture and compare it with the Kps value of the system under analysis.
The ionic product of the system is the product of the concentrations of the ionic species elevated to their corresponding stoichiometric factors.
For Fe(OH)2
Kps for Fe(OH)2 is 4.87x10-17 so we are in an barely undersaturated situation.
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