Calculate the equilibrium potential of a copper wire immersed in 0.0005 M CuSO4 solution. The standard electrode potential for t
he reaction Cu2+ + 2e- = Cu0 at 25°C is 0.34 V (NHE). Now, answer the following questions and enter your results (numerical number only). Calculate the ionic strength (M) of the solution.
1 answer:
Answer:
0.24V
Explanation:
First we must obtain the ionic strength of the solution I as shown in the image attached. This ionic strength can now be used to obtain the activity coefficient of the ions in solution by substitution of the value of the ionic strength obtained previously and the charge of the ion (Cu2+) into the equation for activity coefficient.
The activity of an ion is defined as the product of its activity coefficient and its concentration. This activity of copper II ion is now substituted into the Nernst equation to obtain the equilibrium potential required in the question.
You might be interested in
Answer:
pH = 2.46
Explanation:
Hello there!
In this case, since this neutralization reaction may be assumed to occur in a 1:1 mole ratio between the base and the strong acid, it is possible to write the following moles and volume-concentrations relationship for the equivalence point:
Whereas the moles of the salt are computed as shown below:
So we can divide those moles by the total volume (0.021L+0.0066L=0.0276L) to obtain the concentration of the final salt:
Now, we need to keep in mind that this is an acidic salt since the base is weak and the acid strong, so the determinant ionization is:
Whose equilibrium expression is:
Now, since the Kb of C6H5NH2 is 4.3 x 10^-10, its Ka is 2.326x10^-5 (Kw/Kb), we can also write:
Whereas x is:
Which also equals the concentration of hydrogen ions; therefore, the pH at the equivalence point is:
Regards!