Question

3. Write balanced net ionic equations for the following reactions from the spot tests in Part A. Include the states of components (e.g. (aq) if aqueous, (s) if solid) and the final colour of the solution or precipitate, if any. a) AgNO3+ HCI b) Pb(NO3)2+ K2CrO c) Fe(NO3)3 KSCN d) Ni(NOs)2 + H-DMG e) Ba(NO3)2 K2CrO4

Answer 1

a)

Ag+ and Cl- will form precipitate

Ag+(aq) + Cl-(aq) --> AgCl(s)

b)

Pb+2 and CrO4-2 are not soluble so

Pb+2(aq) + CrO4-2(aq) --> PBCrO4(s)

c)

Fe+3 and SCN- will form complex so

Fe+3(aq) + SCN-(aq) --> Fe(SCN)+2(aq)

d)

DMG stands for dimethylglyoxime

Ni2+ and MDG- forms the xopmles Ni(DMG)2

so

Ni(NO3)2 + 2 HDMG ---> Ni(DMG)2 + 2 HNO3

net ionic

Ni2+(aq) + 2DMG-(aq) =  Ni(DMG)2(aq)

e)

Ba+2 and CrO4-2 ions are not soluble

Ba+2(aq) + CrO4-2(aq) --> BaCrO4