Consider a galvanic cell that operates at 298 K and is based on the following redox reaction: Fe(s) + Sn2+(aq) → Fe2+(aq) + Sn(s) E° = 0.30 V If the cell is initially at standard conditions ([Sn2+] = [Fe2+] = 1.00 M), what are the concentrations of Sn2+ and Fe2+ when the cell potential has fallen 10% to 0.27 V?

Answer asap need to be answered by wednesday morning explain how a buffer works, using an ethanoic acid / sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.