The Ksp of mercury(II) hydroxide, Hg(OH)2, is 3.60 × 10-26. Calculate the solubility of this compound in g/L.

Gf of H2CO3 = -616.1 KJ/mol
Gf of H20 = -237.1 KJ/mol
Gf of CO2 = - 394.4 KJ/mol
3.

To calculate the solubility of mercury(II) hydroxide (Hg(OH)2), you need to use the concept of Ksp (solubility product constant). The Ksp is a measure of the equilibrium between the dissolved ions and the solid compound in a saturated solution.

The general equation for the dissolution of Hg(OH)2 can be written as:

Hg(OH)2(s) ⇌ Hg2+(aq) + 2OH-(aq)

The Ksp expression for this reaction is:

Ksp = [Hg2+][OH-]^2

Given that the Ksp of Hg(OH)2 is 3.60 × 10^-26, we can assume that x is the solubility of Hg(OH)2 in mol/L. As there is stoichiometry involved, the concentration of Hg2+ will be also x, while the concentration of OH- will be 2x.

Substituting these values into the Ksp expression:

Ksp = (x)(2x)^2
3.60 × 10^-26 = 4x^3

Solving for x:

x^3 = (3.60 × 10^-26) / 4
x^3 = 9.00 × 10^-27
x = (9.00 × 10^-27)^(1/3)
x ≈ 1.30 × 10^-9 mol/L

Now, to determine the solubility of Hg(OH)2 in g/L, you need to use the molar mass of Hg(OH)2. The molar mass of Hg = 200.59 g/mol, and the molar mass of OH = 17.01 g/mol.

The molar mass of Hg(OH)2 = (200.59 g/mol) + 2 × (17.01 g/mol)
Molar mass of Hg(OH)2 = 234.61 g/mol

To convert the solubility from mol/L to g/L, multiply the solubility (in mol/L) by the molar mass of Hg(OH)2:

Solubility (g/L) = (1.30 × 10^-9 mol/L) × (234.61 g/mol)
Solubility (g/L) ≈ 3.04 × 10^-7 g/L

Therefore, the solubility of mercury(II) hydroxide (Hg(OH)2) is approximately 3.04 × 10^-7 g/L.

To calculate the solubility of mercury(II) hydroxide, Hg(OH)2, in g/L, we need to use the Ksp (solubility product constant) and the molar mass of Hg(OH)2.

First, let's write the balanced chemical equation for the dissociation of Hg(OH)2:
Hg(OH)2(s) ⇌ Hg2+(aq) + 2OH-(aq)

The Ksp expression can be written as:
Ksp = [Hg2+][OH-]^2

Since the stoichiometric coefficients are 1 for Hg2+ and 2 for OH-, we can assume that the concentrations of Hg2+ and OH- are equal.

Let's represent the solubility of Hg(OH)2 as "s". Therefore, the concentration of Hg2+ and OH- would be "s". Substituting these values into the Ksp expression:
Ksp = s * s^2 = s^3

Given that the Ksp of Hg(OH)2 is 3.60 × 10^-26, we can set up the equation:
3.60 × 10^-26 = s^3

To solve for "s", let's take the cube root of both sides:
s = (3.60 × 10^-26)^(1/3)
s ≈ 3.40 × 10^-9 M

Now, we need to convert the solubility from moles per liter (M) to grams per liter (g/L). To do this, we need to multiply the molar mass of Hg(OH)2, which can be calculated using the atomic masses of the elements:
molar mass of Hg(OH)2 = (1 * atomic mass of Hg) + (2 * atomic mass of O) + (2 * atomic mass of H)
molar mass of Hg(OH)2 = (1 * 200.59 g/mol) + (2 * 15.999 g/mol) + (2 * 1.0078 g/mol)
molar mass of Hg(OH)2 ≈ 34.023 g/mol

Now, we can calculate the solubility in g/L:
solubility = (s * molar mass of Hg(OH)2)
solubility ≈ (3.40 × 10^-9 * 34.023) g/L
solubility ≈ 1.16 × 10^-7 g/L

Therefore, the solubility of mercury(II) hydroxide, Hg(OH)2, is approximately 1.16 × 10^-7 g/L.