C2D3 has a solubility product constant of 9.14×10−9. What is the molar solubility of C2D3? Express your answer with the appropriate units.

To find the molar solubility of C2D3 (assuming it is a binary compound), we need to determine the concentration of C2D3 in a saturated solution. The solubility product constant (Ksp) can help us with this.

The solubility product constant (Ksp) expression for C2D3 is given as follows:
C2D3 ⇌ 2CD3^-

The Ksp expression can be written as:
Ksp = [CD3^-]²

Since the stoichiometric coefficient of CD3^- is 2, the concentration of CD3^- will be twice that of C2D3.

Let's denote the molar solubility of C2D3 as "s". Therefore, the concentration of C2D3 ([C2D3]) in a saturated solution will be equal to "s".

The concentration of CD3^- ([CD3^-]) is then 2s.

Substituting these values into the Ksp expression, we get:
Ksp = (2s)²

Now we can solve for "s".

Ksp = 9.14 × 10^(-9)
(2s)² = 9.14 × 10^(-9)

Taking the square root of both sides:
2s = √(9.14 × 10^(-9))
2s = 9.57 × 10^(-5)

Dividing both sides by 2:
s = (9.57 × 10^(-5)) / 2

s = 4.78 × 10^(-5) mol/L

Therefore, the molar solubility of C2D3 is 4.78 × 10^(-5) mol/L.

To find the molar solubility of C2D3, we need to understand the concept of a solubility product constant (Ksp). The Ksp is an equilibrium constant that measures the solubility of a compound in a solution.

For the compound C2D3, the solubility product constant (Ksp) is given as 9.14×10^−9.

The formula for the solubility product constant (Ksp) is Ksp = [C]^2[D]^3, where [C] and [D] represent the molar concentrations of the ions in the compound (in this case, C2D3).

Since the compound C2D3 is composed of two ions C and three ions D, we can write the general equation for its dissolution as:
C2D3(s) ⇌ 2C+(aq) + 3D-(aq)

Let's represent the molar solubility of C2D3 as "S". At equilibrium, the concentrations of C+ and D- ions will be the same, so we can substitute [C] with 2S and [D] with 3S in the solubility product expression.

Now, we can rewrite the solubility product expression as:
Ksp = (2S)^2 * (3S)^3

Simplifying the expression, we get:
Ksp = 36S^5

To find the molar solubility (S), we rearrange the equation:
S = (Ksp / 36)^(1/5)

Plugging in the given value of Ksp (9.14×10^−9), we can calculate the molar solubility as follows:

S = (9.14×10^-9 / 36)^(1/5)

S ≈ 5.49 × 10^−4 mol/L

Therefore, the molar solubility of C2D3 is approximately 5.49 × 10^−4 mol/L.

........C2D3 ==> 2C^3+ + 3D^2+

I.......solid.....0.......0
C.......solid.....2x......3x
E.......solid.....2x......3x

Ksp = (C^3+)^2(D^2+)^3
9.14E-9 = (2x)^2(3x)^3
Solve for x for solubility of C2D3.

Units: Technically the unit is "activity" since Ksp is a thermodynamic value and has no units. Your prof may want M or mols/L