a solution is made that is 1.5X10^-3M in Zn(NO3)2 and 0.130 M in NH3. the Kf for Zn(NH3)4^2+ is 2.0X10^9
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To find the concentration of Zn(NH3)4^2+ in the solution, you can use the concept of equilibrium constant (K) and the stoichiometry of the reaction. The equilibrium constant (K) is defined as the ratio of the concentration of the products to the concentration of the reactants, each raised to the power of their coefficients in the balanced chemical equation.
The balanced chemical equation for the formation of Zn(NH3)4^2+ from Zn(NO3)2 and NH3 is:
Zn(NO3)2 + 4NH3 ⇌ Zn(NH3)4^2+ + 2NO3^-
The expression for the equilibrium constant (Kf) for this reaction is:
Kf = [Zn(NH3)4^2+] / ([Zn(NO3)2] * [NH3]^4)
Given:
Kf = 2.0 × 10^9
[Zn(NO3)2] = 1.5 × 10^-3 M
[NH3] = 0.130 M
You can substitute the given values into the equation and solve for [Zn(NH3)4^2+]:
2.0 × 10^9 = [Zn(NH3)4^2+] / ((1.5 × 10^-3) * (0.130)^4)
To solve this equation, rearrange it to isolate [Zn(NH3)4^2+]:
[Zn(NH3)4^2+] = 2.0 × 10^9 * ((1.5 × 10^-3) * (0.130)^4)
Calculate the value to find the concentration of Zn(NH3)4^2+ in the solution.