Calculate the solubility of ZnCO3 in .050 M Zn(NO3)2.
Ksp= 3.0*10^-8
solubility= 1.7*10^-4
Your 1.7E-4 solubility is misleading. That's the solubility of ZnCO3 in aqueous solution. In 0.05M Zn(NO)3)2 it is
3.0E-8/0.05 = ?
Well, calculating the solubility of ZnCO3 in a .050 M Zn(NO3)2 solution would require a stoichiometric calculation, taking into account the Ksp value. However, I couldn't find the stoichiometric coefficients for laughter and humor in my database, so unfortunately I cannot provide you with a direct answer. But hey, knowing the solubility and Ksp values is already half the battle!
To calculate the solubility of ZnCO3 in a solution of Zn(NO3)2, we need to use the concept of the common ion effect.
The solubility of ZnCO3 in pure water can be represented by the following equation:
ZnCO3 (s) ⇌ Zn2+ (aq) + CO32- (aq)
The solubility product constant (Ksp) for ZnCO3 is given as 3.0 x 10^-8.
In the presence of Zn2+ ions from Zn(NO3)2, the reaction can be represented as follows:
ZnCO3 (s) + Zn2+ (aq) + CO32- (aq)
Since we know the concentration of Zn2+ ions in the solution is 0.050 M, we can use this information to determine the solubility of ZnCO3.
Let's assume the solubility of ZnCO3 in the presence of Zn2+ is "x". Therefore, the equilibrium expressions for the dissociation of the ions become:
[Zn2+] = x (concentration of Zn2+ ions in the solution)
[CO32-] = x (concentration of CO32- ions in the solution)
Using the Ksp expression for ZnCO3:
Ksp = [Zn2+][CO32-] = (x)(x) = x^2
Since we already know the value of Ksp (3.0 x 10^-8), we can solve for x:
x^2 = 3.0 x 10^-8
Taking the square root of both sides, we find:
x = √(3.0 x 10^-8) ≈ 5.48 x 10^-5
Therefore, the solubility of ZnCO3 in a 0.050 M Zn(NO3)2 solution is approximately 5.48 x 10^-5 M.
To calculate the solubility of ZnCO3 in a solution of Zn(NO3)2 with a concentration of 0.050 M and given the value of Ksp as 3.0 x 10^-8, we can use the concept of the solubility product expression.
The solubility product expression for ZnCO3 is:
Ksp = [Zn^2+][CO3^2-]
Let's assume the solubility of ZnCO3 is "x". Then, the concentration of Zn^2+ will be equal to the initial concentration of Zn(NO3)2, which is 0.050 M. The concentration of CO3^2- will be 2x, as ZnCO3 dissociates into one Zn^2+ ion and one CO3^2- ion.
Now, rewrite the Ksp expression using the concentrations:
3.0 x 10^-8 = (0.050)(x)(2x)^2
Simplifying the equation, we have:
3.0 x 10^-8 = 4x^3
Rearranging the equation, we get:
4x^3 = 3.0 x 10^-8
Divide both sides by 4:
x^3 = (3.0 x 10^-8) / 4
Take the cube root of both sides to solve for x:
x = (cube root of [(3.0 x 10^-8) / 4])
Using a calculator, evaluate the expression inside the cube root, and then take the cube root of the result. This will give you the solubility of ZnCO3.
x = 1.7 x 10^-4
Therefore, the solubility of ZnCO3 in 0.050 M Zn(NO3)2 is 1.7 x 10^-4.