Hg2I2(s) ⇄ Hg2 2+(aq) + 2 I−(aq) Ksp = [Hg2 2+][I−]^2 A saturated solution of Hg2I2 is at equilibrium at 25°C as represented by the equation above. If [I−] = 4.6 × 10^−10 M at equilibrium, which of the following gives the correct molar solubility, S, and Ksp for Hg2I2 ?

Explanation:

Hg₂I₂ ⇆ Hg₂⁺² + 2I⁻¹

2[I⁻¹ ] = 4.6 x 10⁻¹⁰

[I⁻¹ ] = 2.3 x 10⁻¹⁰ M

[Hg₂⁺²] = 2.3 x 10⁻¹⁰ M

Molar solubility = 2.3 x 10⁻¹⁰ moles / liter

Ksp =  [Hg₂⁺²] x [2I⁻¹ ]²

= 4 x 2.3 x 10⁻¹⁰ x (2.3 x 10⁻¹⁰)²

= 48.67 x 10⁻³⁰ .

answer: a chemical reaction

explanation:

im not wrong

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%