Complete and balance each of the following half-reactions (steps 2–5 in half-reaction method):

(a) Cr2+(aq)⟶Cr3+(aq)
(b) Hg(l)+Br−(aq)⟶HgBr42−(aq)
(c) ZnS(s)⟶Zn(s)+S2−(aq)
(d) H2(g)⟶H2O(l (in basic solution)
(e) H2(g)⟶H3O+(aq) (in acidic solution)
(f) NO3−(aq)⟶HNO2(aq) (in acidic solution)
(g) MnO2(s)⟶MnO4−(aq) (in basic solution)
(h) Cl−(aq)⟶ClO3−(aq) (in acidic solution)

Calculate the ratio of h+ ions to oh– ions at a ph = 7. find the concentration of h+ ions to oh– ions listed in table b of your student guide. then divide the h+ concentration by the oh– concentration. record this calculated ratio in table a of your student guide. compare your approximated and calculated ratios of h+ ions to oh– ions at a ph = 7. are they the same? why or why not? record your comparison in table a. what is the concentration of h+ ions at a ph = 7? mol/l what is the concentration of oh– ions at a ph = 7? mol/l what is the ratio of h+ ions to oh– ions at a ph = 7? : 1