what is the net ionic equation for NaOH + H2SeO3?
Molecular equation is
2NaOH + H2SeO3 ==> Na2SeO3 + 2H2O
Net ionic
Strong electrolytes written as ions.
Weak electrolytes as molecules.
Cancel ions common to both sides and the net ionic equation results.
yes but is SeO3 Soluble? i do not know if it can break apart, it is not on the chart
To determine the net ionic equation for the reaction between NaOH (sodium hydroxide) and H2SeO3 (selenous acid), we need to first write the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction can be written as follows:
2NaOH + H2SeO3 -> Na2SeO3 + 2H2O
Now, let's break down this equation into its ionic forms:
2Na+(aq) + 2OH-(aq) + H2SeO3(aq) -> Na2SeO3(aq) + 2H2O(l)
Next, we need to determine which ions are present in both the reactants and the products and cancel out any spectator ions that appear on both sides of the equation. The spectator ions are the ones that do not participate in the reaction.
In this case, the spectator ions are Na+(aq) and OH-(aq) because they appear unchanged on both sides of the equation.
Therefore, the net ionic equation for the reaction between NaOH and H2SeO3 is:
H2SeO3(aq) -> Na2SeO3(aq) + 2H2O(l)
In the net ionic equation, we only include the species that are directly involved in the reaction.