Question

Solubility product of. AgCl is 2.0x10-10 mol2 dm 6
Maximum concentration of Agions in the solution is:​

Answer 1

Answer:

Explanation:

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Answer 2

Concept:

The ability of a substance, known as a solute, to dissolve in a solvent to form a solution is known as solubility. Ionic compounds that separate into cations and anions in water have a wide range of solubilities.

Given:

Solubility product of AgCl (Ksp) = 2.0 x 10⁻¹⁰ mol² dm⁻⁶

Find:

The solubility product of AgCl is 2.0 x 10⁻¹⁰ mol² dm⁻⁶. The maximum concentration of Ag⁺¹ ions in the solution is?

Solution:

AgCl exist in equilibrium as:

               AgCl  ⇄  Ag⁺ + Cl⁻

The solubility product can be calculated as:

              Ksp = [Ag⁺][Cl⁻]

Let the concentration of silver ions and chloride ions be x.

2.0 x 10⁻¹⁰ mol² dm⁻⁶ = x * x

2.0 x 10⁻¹⁰ mol² dm⁻⁶ = x²

square root of(2.0 x 10⁻¹⁰ mol² dm⁻⁶) = x

1.414 * 10⁻⁵ mol dm⁻³ = x

Therefore, the concentration of silver ions and chloride ions is 1.414 * 10⁻⁵ mol dm⁻³.

Hence, the solubility product of AgCl is 2.0 x 10⁻¹⁰ mol² dm⁻⁶. The maximum concentration of Ag⁺¹ ions in the solution is 1.414 * 10⁻⁵ mol dm⁻³.

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