Writing ionic equations, use only ions or species taking part in reaction and show aqeuos ions only.
eg.
H2SO4 + 2NaOH ---> Na2SO4 + H2O
WRITE IONIC EQUATION
2H+ + 2OH- ---> 2H2O
Do we not include the sodium because it has remained the same? (2Na ---> Na2)
And we don't include the SO4 because that has remained the same? (SO4 ---> SO4)
Is that right?
eg.
H2SO4 + 2NaOH ---> Na2SO4 + H2O
WRITE IONIC EQUATION
2H+ + 2OH- ---> 2H2O
Do we not include the sodium because it has remained the same? (2Na ---> Na2)
And we don't include the SO4 because that has remained the same? (SO4 ---> SO4)
Is that right?
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if you're writing an ionic equation, you break up all the ionic compounds into their individual ions.
so it would be H2SO4 + 2Na^+ + 2OH^- ---> 2Na^+ + SO4 ^2- + H2O
*and if you wanted the net ionic equation, you would cancel out any ions that are on oppisite sides of the arrow, so you would take out the 2Na^+
the second one- you can't write an ionic equation since it isn't an ionic equation
so it would be H2SO4 + 2Na^+ + 2OH^- ---> 2Na^+ + SO4 ^2- + H2O
*and if you wanted the net ionic equation, you would cancel out any ions that are on oppisite sides of the arrow, so you would take out the 2Na^+
the second one- you can't write an ionic equation since it isn't an ionic equation