Only number 3 please
2 answers:
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Answer:
.
Explanation:
<h3>Ionic Equation for this reaction</h3>Rewrite only the species that exist as ions. Those species typically include:
- soluble salts,
- strong acids, and
- soluble bases.
In this reaction, both and
are salts. The state symbol "
" suggests that both of these salts are soluble. Hence, both of these salts exist as ions and should be rewritten:
- Each
formula unit would exist as one
and
. Notice how there are twice as many
ions as
ions.
- Each
formula unit would exist as one
and one
.
Similarly, the state symbol "" suggests that the base
is also soluble:
- Each
formula unit would exist as one
.
On the other hand, the state symbol "" suggests that the base
is a precipitate and is not soluble. Rather, the bonds within
stay mostly intact, and this species would not exist as ions. Hence, do not rewrite
when deriving the ionic equation for this reaction.
Hence, the ionic equation for this reaction would be:
.
Eliminate species that are present on both sides of the ionic equation to obtain the net ionic equation. A species should be eliminated if only if an equal number of this species are found on both sides of the ionic equation. Otherwise, subtract from the side with a larger number of that species.
For this reaction, the net ionic equation would be:
.