A saturated aqueous solution of Ag2SO3 contains 3.2x10−5 M Ag+. What is the solubility-product equilibrium constant for Ag2SO3? A) 2.0x10−2 B) 1.6x10−2 C) 1.3x10−13 D) 1.6x10−14 E) 4.1x10−15

D) 1.6 x 10⁻¹⁴

Explanation:

The solubility-product equilibrium constant for  Ag₂SO₃ is given by the expression

Ksp = [Ag⁺]² [SO₃²⁻]

where  [Ag⁺] and [SO₃²⁻] are the concentration of the species dissolved in solution for the equlibrium

Ag₂SO₃ (s) ⇄    2 Ag⁺  +  SO₃²⁻

we are given the concentration of  Ag⁺ and from the stoichiometry of the equilibrium, the concentration of SO₃²⁻ is half that value, so

[Ag⁺]² = 3.2 x 10⁻⁵ M

[SO₃²⁻] = 3.2 x 10⁻⁵ M / 2 = 1.6 x 10⁻⁵ M

plugging these values into the solubility product constant equation we have

Ksp = (3.2 x 10⁻⁵)² x (1.6 x 10⁻⁵) = 1.6 x 10¹⁴

Therefore D is the correct answer.

3

explanation:

the food using pesticides in the future will harm you by giving you diseases like cancer or something since they have things that we should not eat in it like chemicals or pesticides. that is why organic food is more expensive because they take the time to make it right and healthy for you to eat.

explanation: