What Is The Net Ionic Equation Of $Na^{+} + OH^{-} + H^{+} + Cl^{-} \rightarrow H_2O + Na^{+} + Cl^{-}$?A. $NaOH(aq) + HCl(aq) \rightarrow H_2O(\uparrow) + NaCl(aq)$B. \$Na^{+} + Cl^{-} \rightarrow NaCl$[/tex\]C.

Feb 27, 2025 by ADMIN 218 views

What is the Net Ionic Equation of a Chemical Reaction?

Understanding the Basics of Chemical Equations

Chemical equations are a fundamental concept in chemistry, representing the transformation of one or more substances into another. These equations are crucial in understanding the chemical reactions that occur in various processes. A chemical equation consists of reactants on the left side and products on the right side, separated by an arrow. The reactants are the substances that undergo a chemical change, while the products are the resulting substances after the reaction.

Writing the Complete Ionic Equation

To write the complete ionic equation, we need to break down the aqueous compounds into their respective ions. The given equation is:

Na^{+} + OH^{-} + H^{+} + Cl^{-} \rightarrow H_2O + Na^{+} + Cl^{-}

Breaking down the aqueous compounds into their respective ions, we get:

Na^{+}(aq) + OH^{-}(aq) + H^{+}(aq) + Cl^{-}(aq) \rightarrow H_2O(l) + Na^{+}(aq) + Cl^{-}(aq)

Identifying the Strong Electrolytes

Strong electrolytes are substances that completely dissociate into their respective ions in an aqueous solution. In the given equation, $NaOH(aq)$ and $HCl(aq)$ are strong electrolytes. They completely dissociate into their respective ions, which are $Na^{+}$ , $OH^{-}$ , $H^{+}$ , and $Cl^{-}$ .

Writing the Complete Ionic Equation with Strong Electrolytes

Substituting the strong electrolytes with their respective ions, we get:

Na^{+}(aq) + OH^{-}(aq) + H^{+}(aq) + Cl^{-}(aq) \rightarrow H_2O(l) + Na^{+}(aq) + Cl^{-}(aq)

Identifying the Weak Electrolyte

A weak electrolyte is a substance that only partially dissociates into its respective ions in an aqueous solution. In the given equation, $H_2O$ is a weak electrolyte. It partially dissociates into its respective ions, which are $H^{+}$ and $OH^{-}$ .

Writing the Complete Ionic Equation with Weak Electrolytes

Substituting the weak electrolyte with its respective ions, we get:

Na^{+}(aq) + OH^{-}(aq) + H^{+}(aq) + Cl^{-}(aq) \rightarrow H^{+}(aq) + OH^{-}(aq) + Na^{+}(aq) + Cl^{-}(aq)

Writing the Net Ionic Equation

The net ionic equation is obtained by removing the spectator ions from the complete ionic equation. Spectator ions are ions that do not participate in the chemical reaction. In the given equation, $Na^{+}$ and $Cl^{-}$ are spectator ions.

Removing the spectator ions, we get:

OH^{-}(aq) + H^{+}(aq) \rightarrow H_2O(l)

Conclusion

The net ionic equation of the given chemical reaction is:

OH^{-}(aq) + H^{+}(aq) \rightarrow H_2O(l)

This equation represents the actual chemical reaction that occurs between the hydroxide ion and the hydrogen ion to form water.

Answer

The correct answer is:

C. $OH^{-}(aq) + H^{+}(aq) \rightarrow H_2O(l)$

What is a Net Ionic Equation?

A net ionic equation is a simplified representation of a chemical reaction, showing only the ions that participate in the reaction. It is obtained by removing the spectator ions from the complete ionic equation.

Q: What are Spectator Ions?

A: Spectator ions are ions that do not participate in the chemical reaction. They are present in the solution but do not undergo any change during the reaction.

Q: How do I Identify Spectator Ions?

A: To identify spectator ions, look for ions that appear on both sides of the complete ionic equation. These ions are not involved in the chemical reaction and can be removed to obtain the net ionic equation.

Q: What is the Difference Between a Complete Ionic Equation and a Net Ionic Equation?

A: A complete ionic equation shows all the ions present in the solution, including spectator ions. A net ionic equation, on the other hand, shows only the ions that participate in the chemical reaction, with spectator ions removed.

Q: Why is it Important to Write a Net Ionic Equation?

A: Writing a net ionic equation helps to identify the actual chemical reaction that occurs between the reactants. It also helps to understand the role of each ion in the reaction.

Q: How do I Write a Net Ionic Equation?

A: To write a net ionic equation, follow these steps:

Write the complete ionic equation.
Identify the spectator ions.
Remove the spectator ions from the complete ionic equation.
Simplify the resulting equation to obtain the net ionic equation.

Q: What are Some Common Mistakes to Avoid When Writing a Net Ionic Equation?

A: Some common mistakes to avoid when writing a net ionic equation include:

Failing to identify spectator ions
Removing the wrong ions from the complete ionic equation
Not simplifying the resulting equation

Q: Can You Provide an Example of Writing a Net Ionic Equation?

A: Let's consider the following chemical reaction:

NaOH(aq) + HCl(aq) \rightarrow H_2O(l) + NaCl(aq)

To write the net ionic equation, we need to break down the aqueous compounds into their respective ions:

Na^{+}(aq) + OH^{-}(aq) + H^{+}(aq) + Cl^{-}(aq) \rightarrow H_2O(l) + Na^{+}(aq) + Cl^{-}(aq)

Identifying the spectator ions, we see that $Na^{+}$ and $Cl^{-}$ are present on both sides of the equation. Removing these ions, we get:

OH^{-}(aq) + H^{+}(aq) \rightarrow H_2O(l)

This is the net ionic equation for the given chemical reaction.

Conclusion

Writing a net ionic equation is an important step in understanding chemical reactions. By identifying spectator ions and removing them from the complete ionic equation, we can obtain a simplified representation of the reaction. This helps to identify the actual chemical reaction that occurs between the reactants and understand the role of each ion in the reaction.