Silver (I) has a reduction potential of 0.799 V. If the solubility product of Ag2S is 6.0 x 10-51 (Ksp=[Ag+ ] 2 [S2-] )

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Silver (I) has a reduction potential of 0.799 V. If the
solubility product of Ag2S is 6.0 x 10-51 (Ksp=[Ag+ ] 2 [S2-] ) and
the pKa H2S is 7.05 and the pKa of HS- is 19. Estimate the
reduction potential for the following reaction using the data
provided above. Assume 25oC. You must show your calculation using
the above information
a. Ag2S(s)+H++2e- ↔ 2Ag(s)+HS
b. Write the appropriate Nernst equation for this half-cell.
c. A Silver/Silver Sulfide electrode is used with calomel
reference electrode with a half-cell voltage of 0.244 V. If the
high impedance meter reads -443 mV at a pH of 7.2 what is the
concentration of H2S, HS- and S-2?
Not sure where to start as the product is a solid