Calculate [Cu^2+] in a 0.15 M CuSO4 solution that also 6.5 M in free NH3.

Cu^2+ + 4NH3 >>>>>> Cu(NH3)4

kf = 1.1 * 10^11.

thx

tell me the fromula for charles law

1.6 x 10^-17

To calculate [Cu^2+] in a solution that contains CuSO4 and NH3, we need to use the formation constant (kf) for the complex Cu(NH3)4 and the concentration of free NH3 (ammonia).

The formation equation is given as:
Cu^2+ + 4NH3 >>> Cu(NH3)4

First, we need to calculate the concentration of NH3 in terms of Cu(NH3)4. Since there are four NH3 molecules per one Cu(NH3)4 complex, we can calculate the concentration of NH3 as follows:

[Cu(NH3)4] = [NH3] / 4
[6.5 M] = [NH3] / 4
[NH3] = 6.5 M * 4
[NH3] = 26 M

Next, we use the formation constant (kf) to calculate the concentration of [Cu^2+]. The formation constant (kf) is a measure of the tendency of Cu^2+ to form the complex Cu(NH3)4. The equation for calculating [Cu^2+] is as follows:

kf = [Cu(NH3)4] / ([Cu^2+] * [NH3]^4)

Substituting the given values:
1.1 * 10^11 = [Cu(NH3)4] / ([Cu^2+]*[NH3]^4)
1.1 * 10^11 = (26 M) / ([Cu^2+]*((26 M)^4))

Simplifying:
1.1 * 10^11 = (26 M) / ([Cu^2+]*(456976 M^4))

Rearranging the equation:
[Cu^2+] = (26 M) / (1.1 * 10^11 * (456976 M^4))

Calculating the value:
[Cu^2+] = 5.84 * 10^-16 M

Therefore, the concentration of [Cu^2+] in the 0.15 M CuSO4 solution with 6.5 M free NH3 is 5.84 * 10^-16 M.