Determine whether a solid forms when solutions containing the follow salts are mixed. If so, write the ionic equation and the net ionic equation.
a: Na3PO4 and AgNO3
b: K2SO4 and Na2CO3
C: Pb(NO3)2 and Na2CO3
d: BaCl2 and KOH
Determine whether a solid forms when solutions containing the following salts are mixed. If so, write the ionic equation and the net ionic equation.
KCl and Na2S
To determine whether a solid forms when two solutions are mixed, we need to consider the possibility of a precipitation reaction occurring. A precipitation reaction occurs when two soluble salts react to form an insoluble precipitate.
To determine if a reaction occurs, we can use solubility rules, which provide information about the solubility of various salts in water. By consulting these rules, we can determine whether the resulting products are soluble or insoluble.
Let's analyze each pair of salts:
a) Na3PO4 and AgNO3:
- Na3PO4 is soluble in water according to the solubility rules.
- AgNO3 is also soluble in water according to the solubility rules.
Since both Na3PO4 and AgNO3 are soluble, no solid will form when they are mixed. Therefore, no ionic equation or net ionic equation can be written.
b) K2SO4 and Na2CO3:
- K2SO4 is soluble in water according to the solubility rules.
- Na2CO3 is also soluble in water according to the solubility rules.
Similar to the previous case, both K2SO4 and Na2CO3 are soluble salts, and no solid will form. Thus, there is no ionic equation or net ionic equation for this combination.
c) Pb(NO3)2 and Na2CO3:
- Pb(NO3)2 is soluble in water according to the solubility rules.
- Na2CO3 is also soluble, except when paired with some metal ions including Pb(2+).
Since Pb(NO3)2 is soluble and Na2CO3 can form an insoluble precipitate (PbCO3), a solid will form when these two solutions are mixed.
To write the ionic equation and net ionic equation, we first write the balanced molecular equation:
Pb(NO3)2 (aq) + Na2CO3 (aq) -> PbCO3 (s) + 2NaNO3 (aq)
Then, we can write the ionic equation by separating the soluble compounds into their respective ions:
Pb(2+) (aq) + 2NO3(-) (aq) + 2Na(+) (aq) + CO3(2-) (aq) -> PbCO3 (s) + 2Na(+) (aq) + 2NO3(-) (aq)
Finally, we can write the net ionic equation by removing the spectator ions (ions that appear on both sides unchanged):
Pb(2+) (aq) + CO3(2-) (aq) -> PbCO3 (s)
d) BaCl2 and KOH:
- BaCl2 is soluble in water according to the solubility rules.
- KOH is also soluble in water according to the solubility rules.
Since both BaCl2 and KOH are soluble salts, no solid forms when they are mixed. Therefore, no ionic equation or net ionic equation can be written for this combination.
You need to learn (read that memorize) the solubility rules. Here is a simplified set.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
For a I know that Ag3PO4 is insoluble.
The net ionic equation is
3Ag^+(aq) + PO4^-(aq) ==> Ag3PO4(s)
For b I know that K2CO3 and Na2SO4 are soluble.