The solubility product constant (Ksp) for the dissolution of Cu(OH)2 as represented by the chemical equation is 2.6 x 10-19.
Cu(OH)2 (s) Cu2+ (aq) + 2 OH- (aq)
Calculate the moles of Cu(OH)2 that dissolves in 1900 mL of water.
i know how to do it when its one to one but for these i always get confused on the (1/2) and x^2 and what you do with it.
Cu(OH)2 ==> Cu^2+ + 2OH^-
....x........x.......2x
Ksp = (Cu^2+)(OH^-)2
Ksp = (x)(2x)2
Ksp = 4x3
x = ?
4.0 x 10^-7
To calculate the moles of Cu(OH)2 that dissolve in 1900 mL of water, we first need to find the concentration of Cu2+ and OH- ions in the solution.
Let's assume that 'x' moles of Cu(OH)2 dissolve in water. As per the balanced chemical equation, 1 mole of Cu(OH)2 yields 1 mole of Cu2+ and 2 moles of OH- ions.
Thus, the concentration of Cu2+ ions in the solution is also 'x' moles per liter, and the concentration of OH- ions in the solution is '2x' moles per liter.
Given that the volume of the solution is 1900 mL (or 1.9 L), the number of moles of Cu2+ ions and OH- ions present in the solution can be calculated as follows:
Number of moles of Cu2+ = x mol/L * 1.9 L = 1.9x
Number of moles of OH- = 2x mol/L * 1.9 L = 3.8x
Using the solubility product constant (Ksp), we can set up the following equation:
Ksp = [Cu2+][OH-]^2
2.6 x 10^(-19) = (1.9x)(3.8x)^2
Now, solve this equation for 'x' to find the moles of Cu(OH)2 that dissolves in 1900 mL of water.
To calculate the moles of Cu(OH)2 that dissolve in 1900 mL of water, we need to use the solubility product constant (Ksp) and the stoichiometry of the balanced equation.
The solubility product constant (Ksp) expression for the dissolution of Cu(OH)2 is given as follows:
Ksp = [Cu2+][OH-]^2
From the balanced equation, we can see that 1 mole of Cu(OH)2 produces 1 mole of Cu2+ and 2 moles of OH-. Therefore, we can write the relationship as:
[Cu2+] = [Cu(OH)2]
[OH-] = 2[Cu(OH)2]
Now let's assign a variable, let's say x, to the concentration of Cu(OH)2 that dissolves in water. By using this variable, we can write the concentrations of Cu2+ and OH- in terms of x:
[Cu2+] = x
[OH-] = 2x
Substituting these values into the expression for Ksp, we have:
Ksp = (x)(2x)^2 = 4x^3
Given that Ksp = 2.6 x 10^(-19), we can set up the equation:
2.6 x 10^(-19) = 4x^3
Now we can solve for x:
Divide both sides of the equation by 4:
(2.6 x 10^(-19))/4 = x^3
Take the cube root of both sides to isolate x:
x = (2.6 x 10^(-19)/4)^(1/3)
Evaluating the expression, we find that x ≈ 1.08 x 10^(-7) M.
Now that we have the concentration of Cu(OH)2 in terms of moles per liter (M), we can calculate the moles of Cu(OH)2 that dissolve in 1900 mL of water (1.9 L).
moles of Cu(OH)2 = concentration (M) × volume (L)
moles of Cu(OH)2 = (1.08 x 10^(-7) M) × (1.9 L)
Calculating this expression, we find that the number of moles of Cu(OH)2 that dissolves in 1900 mL of water is approximately 2.05 x 10^(-7) mol.