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Savatey [412]
3 years ago
8

Will a precipitate (ppt) form when 300. mL of 2.0 × 10 –5 M AgNO 3 are added to 200. mL of 2.5 × 10 –9 M NaI? Answer yes or no,

and identify the precipitate if there is one
Chemistry
1 answer:
Vsevolod [243]3 years ago
8 0

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>

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