Answer:
A precipitate will form, AgI
Explanation:
When Ag⁺ and I⁻ ions are in an aqueous media, AgI(s), a precipitate, is produced or not based on its Ksp expression:
Ksp = 8.3x10⁻¹⁷ = [Ag⁺] [I⁻]
<em>Where the concentrations of the ions are the concentrations in equilibrium</em>
For actual concentrations of a solution, you can define Q, <em>reaction quotient, </em>as:
Q = [Ag⁺] [I⁻]
<em>If Q > Ksp, the ions will react producing BaCO₃, if not, no precipitate will form</em>.
Actual concentrations of Ag⁺ and I⁻ are:
[Ag⁺] = [AgNO₃] = 2.0x10⁻⁵ × (300mL / 500.0mL) = 1.2x10⁻⁵M
[I⁻] = [NaI] = 2.5x10⁻⁹ × (200mL / 500.0mL) = 1.0x10⁻⁹M
<em>500.0mL is the volume of the mixture of the solutions</em>
Replacing in Q expression:
Q = [Ag⁺] [I⁻]
Q = [1.2x10⁻⁵M] [1.0x10⁻⁹M]
Q = 1.2x10⁻¹⁴
As Q > Ksp
<h3>A precipitate will form, AgI</h3>
