Please correct answers from v to xi focus.

The titration solution in the cell below had a total volume of 50.0 mL and contained 0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00 S.C.E. || Zn(s) | titration solution Zn2+ + 2e- Zn(s) E = -0.762 V MgY2- : Kf = 6.2 108; 6.2 x 108; ZnY2-: Kf = 3.2 x 1016 What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: See Exercise 15-B.) v) Concentration of MgY2- in M mmoles of excess unreacted vi) Mg+2 vii) Concentration of Mg+2 in M viii) Concentration of EDTA (Y4-) in M ix) Total mmoles of Zn+2{1:NUMERICAL:%100%0.500:0.15) x) mole of ZnY2- in M xi) Concentration of ZnY2- in M xii) Concentration of Zn2+ in M xiii) Potential of the cell in voltage, Ecell={1:NUMERICAL-1.364:0.1}