Write the net ionic equation for the following reaction: {eq}NaF(aq) + HClO_4(aq) \to {/eq}
Question:
Write the net ionic equation for the following reaction: {eq}NaF(aq) + HClO_4(aq) \to {/eq}
Ionic Equation:
A simple reaction equation defines an ionic equation during which some ions of individual chemical substance or some ions of chemical sub-compound participate and form a product. For example, water can form by the chemical reaction between hydrogen, and hydroxide ion. Its ionic equation is {eq}{{\text{H}}^{+}}+\text{O}{{\text{H}}^{-}}\to {{\text{H}}_{2}}\text{O} {/eq}.
Answer and Explanation: 1
The reaction is {eq}\text{NaF}\left( \text{aq} \right)+\text{HCl}{{\text{O}}_{4}}\left( \text{aq} \right)\to {/eq}.
Net ionic equation of the reaction equation is written below,
{eq}\begin{align} \text{NaF}\left( \text{aq} \right)+\text{HCl}{{\text{O}}_{4}}\left( \text{aq} \right) &\to \\ \text{NaF}\left( \text{aq} \right)+\text{HCl}{{\text{O}}_{4}}\left( \text{aq} \right) &\to \text{HF}\left( \text{l} \right)+\text{NaCl}{{\text{O}}_{4}}\left( \text{aq} \right) \\ \left[ \text{N}{{\text{a}}^{+}}\left( \text{aq} \right)+{{\text{F}}^{-}}\left( \text{aq} \right) \right]+\left[ {{\text{H}}^{+}}\left( \text{aq} \right)+\text{Cl}{{\text{O}}_{4}}^{-}\left( \text{aq} \right) \right] &\to \text{HF}\left( \text{l} \right)+\left[ \text{N}{{\text{a}}^{+}}\left( \text{aq} \right)+\text{Cl}{{\text{O}}_{4}}^{-}\left( \text{aq} \right) \right] \\ \text{N}{{\text{a}}^{+}}\left( \text{aq} \right)+{{\text{F}}^{-}}\left( \text{aq} \right)+{{\text{H}}^{+}}\left( \text{aq} \right)+\text{Cl}{{\text{O}}_{4}}^{-}\left( \text{aq} \right) &\to \text{HF}\left( \text{l} \right)+\text{N}{{\text{a}}^{+}}\left( \text{aq} \right)+\text{Cl}{{\text{O}}_{4}}^{-}\left( \text{aq} \right) \\ {{\text{F}}^{-}}\left( \text{aq} \right)+{{\text{H}}^{+}}\left( \text{aq} \right) &\to \text{HF}\left( \text{l} \right) \\ {{\text{H}}^{+}}\left( \text{aq} \right)+{{\text{F}}^{-}}\left( \text{aq} \right) &\to \text{HF}\left( \text{l} \right) \end{align} {/eq}
Thus, the net ionic equation is {eq}{{\text{H}}^{+}}\left( \text{aq} \right)+{{\text{F}}^{-}}\left( \text{aq} \right)\to \text{HF}\left( \text{l} \right) {/eq}.
Learn more about this topic:
from
Chapter 10 / Lesson 9Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.