Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add 100.0 mL of 1.0 M NaCl to that compartment. Ksp of AgCl is 1.6 x 10^-10 so the Qsp > Ksp and solid AgCl will precipitate out of solution. This silver chloride is in equilibrium with its ions according to the Ksp equilibrium. Calculate [Ag+] (HINT: it will be very small) and then use your result to calculate the cell potential to the hundredths (2 decimal places) with this concentration of [Ag+].
E (Ag+) = 0.80V
E (Cu2+) = 0.34V
Ksp of AgCl = [Ag+][Cl-]
Here, [Cl-] = [NaCl] = 100 mL * 1 M/(100+100) mL = 0.5 M
i.e. 1.6*10-10 = [Ag+] * 0.5 M
Therefore, [Ag+] = 3.2*10-10 M
Now, the cell potential (Eocell) = EoAg+/Ag - EoCu2+/Cu = 0.80 - 0.34 = 0.46 V
Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add...
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3 ques plz help thank you
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