Balanced equation for salts prepared from acid or base

[Mitchtwitchita]

Hey Guys, I seem to be having some problem with this question. Can anybody help me out?

Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and net ionic equation for the preparation for each. Indicate states of the reactants and the products [(aq), (s), (l)]. Review solubility rules if necessary to determine the solubility of reactants.

(a) Fe(NO3)3 (aq) (b) LiBr (aq) (c) KHCO3 (aq)

For (a): 3HNO3 (aq) + Fe(OH)3 (s) > Fe(NO3)3 (aq) + 3H2O (l)
Ionic Equation: 3H2+(aq) + Fe(OH)3 (s) > Fe3+ (aq) + 3H2O (l)

For (b): HBr (aq) + LiOH (aq) > LiBr (aq) + H20 (l)
Ionic Equation: H2+ (aq) + OH- (aq) > H2O (l)

For (c): H2CO3 (aq) + KOH (aq) > KHCO3 (aq) +H2O (l)
Ionic Equation: H2+ (aq) + OH- (aq) > H2O (l)

I'm sure that these are incorrect, can anyone set me on the right path? Please.

 

[eli64]

For (a): 3HNO3 (aq) + Fe(OH)3 (s) > Fe(NO3)3 (aq) + 3H2O (l)
Ionic Equation: 3H2+(aq) + Fe(OH)3 (s) > Fe3+ (aq) + 3H2O (l)

QUOTE]

the dissociation of HNO3 in the ionic equation is H+(aq) + NO3-(aq)
in the net ionic should be 3H+ + Fe(OH)3 (s) etc...

- same for b)

- same for c) except...

H2CO3 is a weak acid, some books tell you not to dissociate it in the ionic equation because of this so
H2CO3(aq) + OH-(aq) ----> HCO3-(aq) + H2O (l)


however, experimentally, with a strong base like KOH, you would probably also get K2CO3too and have a mixture of products

H2CO3(aq) + 2KOH(aq) ----> K2CO3(aq) + H2O(l)
net ionic is...