[Geddoe]

Each of the following salts can be prepared from an acid and a base. Write the balanced molecular
equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products
[(aq), (s), (l)]. Review solubility rules if necessary to determine the solubility of the reactants.
(a) Ba(ClO4)2 (aq) (b) CsCH3CO2 (aq) (c) Sr(ClO4)2 (aq)

(a)
Ba(OH)2(aq) + 2HClO4(aq) -----> Ba(ClO4)2(aq) + 2H2O(l)

net: 2OH-(aq) + 2H+(aq) -----> 2H2O(l)

(b)
CsOH(aq) + CH3COOH(aq) ----> CsCH3COO(aq) + H2O(l)

net:
OH-(aq) + CH3COOH(aq) ----> CH3COO-(aq) + H2O(l)

(c)  Sr(OH)2(aq) + 2 HClO4(aq) = Sr(ClO4)2(aq) + 2 H2O(l)
net: 2OH-(aq) + 2H+(aq) ---> 2H2O(l)

Correct?

[UG]

I (think) you have to write the net ionic for the formation of the SALT, ie, Ba²⁺ + 2ClO4^- Ba(ClO4)

[Borek]

Ba²⁺ + 2ClO4^- Ba(ClO4)

That would be strange, as technically there is no reaction taking place - correctly written it is

Ba²⁺(aq) + 2ClO4^-(aq) Ba²⁺(aq) + 2ClO4^-(aq)

No idea what will be accepted as a correct answer.

Geddoe: last one doesn't have smallest possible coefficients.

[UG]

Oh, that's funny, why do they not react?

[Geddoe]

The logic of writing the net ionic equations here is leaving what is left after crossing out the spectator ions, correct? They don't react per solubility rules.

Borek: Smallest possible coeff is 2 isn't it? Thus...  Sr(OH)2(aq) + 2 HClO4(aq) => Sr(ClO4)2(aq) + 2 H2O(l) right?

[Geddoe]

Ah or are you referring to the net ionic...

 OH-(aq) + H+(aq) => H2O(l)


would that be correct?

[Borek]

OH-(aq) + H+(aq) => H2O(l)

Yes.

[sjb]

Oh, that's funny, why do they not react?

It's not a case of not reacting per se, but barium perchlorate is soluble in water, so the net ionic is different say, compared to the case of barium sulfate, where the product is insoluble.