The compound M2X3 has a molar solubility of 0.0190 M. What is the value of Ksp for M2X3?
Here are the choices:
1. 3.52 × 10^-6
2. 4.12 × 10^-5
3. 8.91 × 10^-8
4. 2.48 × 10^-9
5. 2.67 × 10^-7
Well, it looks like we've stumbled upon some chemistry. Don't worry, I'm here to clown around and help you out! To find the value of the solubility product constant (Ksp), we need to use the molar solubility of the compound M2X3.
Ksp is the product of the concentrations of the products raised to the power of their stoichiometric coefficients. In this case, the stoichiometry is 1:1 between M2X3 and its dissociated ions, so the balanced equation would be:
M2X3 ⇌ 2M^3+ + 3X^-
The molar solubility of M2X3 is given as 0.0190 M. Since the compound dissociates into 2M^3+ ions and 3X^- ions, the concentration of the ions would be twice the molar solubility for M^3+ ions and three times the molar solubility for X^- ions.
Using the given molar solubility, the concentration of M^3+ ions would be 2 * 0.0190 M = 0.0380 M, and the concentration of X^- ions would be 3 * 0.0190 M = 0.0570 M.
Now, to find Ksp, we multiply the concentrations of the products raised to the power of their stoichiometric coefficients:
Ksp = [M^3+]^2 * [X^-]^3
= (0.0380 M)^2 * (0.0570 M)^3
Calculating the value gives us Ksp = 4.12152 × 10^-5.
So, the correct choice is 2. 4.12 × 10^-5.
To find the value of Ksp for M2X3, we need to use the given molar solubility.
Ksp represents the solubility product constant and is equal to the product of the concentrations of the ions raised to the power of their respective stoichiometric coefficients.
The compound M2X3 dissociates into 2 M+ ions and 3 X- ions.
So, the Ksp expression for M2X3 is:
Ksp = [M+]^2 * [X-]^3
Given that the molar solubility of M2X3 is 0.0190 M, the concentration of M+ ions and X- ions in the solution is also 0.0190 M.
Plugging these values into the Ksp expression:
Ksp = (0.0190)^2 * (0.0190)^3
Ksp = 0.0190^5
Ksp = 8.91 x 10^-8
Therefore, the value of Ksp for M2X3 is 8.91 x 10^-8.
So, the correct choice is option 3: 8.91 x 10^-8.
To find the value of Ksp for M2X3, we can start by writing the balanced equation for the dissolution of M2X3:
M2X3(s) ⇌ 2M3+(aq) + 3X3-(aq)
The equilibrium expression for the solubility product constant, Ksp, can be written by multiplying the concentrations of the products raised to the power of their stoichiometric coefficients:
Ksp = [M3+]^2 * [X3-]^3
Given that the molar solubility of M2X3 is 0.0190 M, we can use this information to determine the concentration of M3+ and X3- in terms of x, the molar solubility of M2X3:
[M3+] = 2x
[X3-] = 3x
Substituting these expressions into the Ksp equation, we get:
Ksp = (2x)^2 * (3x)^3 = 36x^5
Now, we can substitute the given molar solubility value into the equation:
Ksp = 36 * (0.0190)^5
Calculating this expression gives:
Ksp ≈ 8.91 × 10^-8
Therefore, the correct choice is option 3: 8.91 × 10^-8.
.........M2X3 ==> 2M^3+ + 3X^-2
I.......solid.....0........0
C.......solid.....2x.......3x
E.......solid.....2x.......3x
Ksp = (M^3+)^2(X^2-)^3
Ksp = (2x)^2(3x)^3
Substitute and solve for Ksp.