Calculate the solubility of Cu(oh)2 in grams per liters of solution if Ksp for Cu(OH)2 IS 4.8X 10^-20
To calculate the solubility of Cu(OH)2 in grams per liters of solution, we need to use the solubility product constant (Ksp) and the stoichiometry of the reaction.
The balanced equation for the dissolution of Cu(OH)2 can be written as follows:
Cu(OH)2(s) ↔ Cu^2+(aq) + 2OH^-(aq)
The Ksp expression for this equation is:
Ksp = [Cu^2+][OH^-]^2
Given that Ksp for Cu(OH)2 is 4.8×10^-20, we can assume that the equilibrium concentrations of Cu^2+ and OH^- are both equal because of the 1:2 stoichiometric ratio.
Let's assume that the concentration of Cu^2+ and OH^- at equilibrium is represented by 'x', then:
[Cu^2+] = x (M)
[OH^-] = 2x (M)
Applying this information to the Ksp expression, we have:
Ksp = x * (2x)^2
4.8×10^-20 = 4x^3
Solving for x:
4x^3 = 4.8×10^-20
x^3 = (4.8×10^-20) / 4
x^3 = 1.2×10^-20
x = (1.2×10^-20)^(1/3)
x ≈ 9.68×10^-7 M
Now we can convert the concentration to grams per liter by considering the molar mass of Cu(OH)2, which is 97.56 g/mol.
To convert from molarity (M) to grams per liter (g/L), we can multiply the molarity by the molar mass.
Converting the solubility to grams per liter:
Solubility = (9.68×10^-7 M) * (97.56 g/mol) = 9.44×10^-5 g/L
Therefore, the solubility of Cu(OH)2 in grams per liter of solution is approximately 9.44×10^-5 g/L.
To calculate the solubility of Cu(OH)2 in grams per liter (g/L) of solution, you need to use the solubility product constant (Ksp) and set up an equilibrium expression.
The solubility product constant (Ksp) is an equilibrium constant that represents the equilibrium between a solid compound dissolving and the ions in the solution. In this case, the equation is:
Cu(OH)2(s) ⇌ Cu2+(aq) + 2OH-(aq)
The Ksp expression for this reaction is:
Ksp = [Cu2+][OH-]^2
Where [Cu2+] represents the concentration of Cu2+ ions in the solution and [OH-] represents the concentration of OH- ions in the solution.
Given the value of Ksp as 4.8 × 10^-20, you can set up the equation like this:
4.8 × 10^-20 = [Cu2+][OH-]^2
Since Cu(OH)2 dissociates into 1 Cu2+ ion and 2 OH- ions, let's assume the solubility of Cu(OH)2 as "x" moles. Therefore, the concentration of Cu2+ ([Cu2+]) in the solution will be "x" moles per liter (mol/L), and the concentration of OH- ([OH-]) will be "2x" moles per liter (mol/L).
Now, substitute these values into the Ksp expression:
4.8 × 10^-20 = [x][2x]^2
4.8 × 10^-20 = 4x^3
Rearrange the equation to solve for x:
x = ∛(4.8 × 10^-20 / 4)
x ≈ 5.84 × 10^-7 mol/L
Finally, to find the solubility in grams per liter (g/L), you need to multiply the molar mass of Cu(OH)2 by the concentration in moles per liter:
Molar mass of Cu(OH)2 = 63.55 g/mol (Cu) + 2 * (1.01 g/mol (H) + 16.00 g/mol (O)) = 97.55 g/mol
Solubility = Concentration (moles/L) * Molar mass (g/mol)
Solubility = 5.84 × 10^-7 mol/L * 97.55 g/mol
Therefore, the solubility of Cu(OH)2 is approximately 5.69 × 10^-5 g/L.
Cu(OH)2 ==> Cu^+2 + 2OH^-
Ksp = (Cu^+2)(OH^-)^2
Set up an ICE chart and solve for solubility.