HClO2(aq)+NaOH(aq)⟶H2O(l)+NaClO2(aq) net ionic equation

Answer 1

When finding the net ionic equation, you must first split up all ionic compounds in the equation. Not sure what this means? Let's dive into it.

1. Original equation : HClO₂ (aq) + NaOH (aq) -----> H₂O (l) + NaClO₂(aq)
2. Which compounds in this equation can be split?
3. Aqueous compounds can be split : HClO₂, NaOH, and NaClO₂
4. Liquid / solids cannot be split : H₂O cannot be split
5. Splitting the compounds
6. HClO2 (aq)
7. splits into H+ and ClO₂^-
8. if you were unsure about the charge for ClO₂^- , remember that the H+ and ClO₂ must equal out to a neutral charge, since this compound has zero charge overall. So since H+ has a positive charge of +1, ClO₂ must have a -1 charge to equal zero total charge.
9. You may also find it helpful to memorize the polyatomic ion charges for your future chemistry classes: https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_(CK-12)/07%3A_Chemical_Nomenclature/7.09%3A_Polyatomic_Ions
10. NaOH
11. splits into Na+ and OH-
12. NaClO₂
13. Splits into Na+ and ClO₂^-
14. Rewrite equation with split compounds
15. H⁺ + ClO₂^- + Na⁺ + OH^- -----> H₂O (l) + Na⁺ + ClO₂^-
16. Cross out like terms from both sides (just like in algebra!)
17. H⁺ + ClO₂^- + Na⁺ + OH^- -----> H₂O (l) + Na⁺ + ClO₂^-
18. What you are left with is your net ionic equation:
19. ANSWER: H⁺+ OH^-------> H₂O (l)

Answer 2

Hey there Lexie! The formula you gave is sometimes referred to as a molecular equation, in which all the substances are written as though they exist as molecules, even though they might actually exist as separate ions in aqueous solution.

HClO₂(aq) + NaOH(aq) ⟶ H₂O(l) + NaClO₂(aq)

The complete ionic equation for the above looks like this:

H⁺(aq) + ClO₂^–(aq) + Na⁺(aq) + OH^–(aq) ⟶ H₂O(l) + Na⁺(aq) + ClO₂^–(aq)

The complete ionic equation shows us that, in aqueous solutions, the compounds HClO₂, NaOH, and NaClO₂ exist not as connected molecular compounds, as the molecular equation indicated, but rather in their dissolved form as individual hydrogen (H⁺), chlorite (ClO₂^–) hydroxide (OH^–) and sodium ions (Na⁺). The (aq) symbol next to these compounds in the molecular equation is an indication that they actually exist, in aqueous solution, as these independent, freely moving ions. By contrast, water, which is written as H₂O(l), is actually a single covalent compound in liquid form; it is not split into different ions.

The net ionic equation is a way of indicating which species are actually participating in the reaction at hand. Notice, in the complete ionic equation, that chlorite (ClO₂^–) and sodium (Na⁺) appear the same in the left- and right-hand sides of the reaction; they undergo no chemical change. Ions that appear in the complete ionic equation, but do not actually participate in the chemical reaction, are called spectator ions. The net ionic equation eliminates spectator ions to show only the species that actually participate in the reaction.

So your net ionic equation is:

H⁺(aq) + OH^–(aq) ⟶ H₂O(l)