Question

Write the complete ionic equation and net ionic equation for the neutralization reaction between aqueous hydrobromic acid and barium hydroxide.

Short answer

Complete ionic equation: \(2H^+ (aq) + 2Br^- (aq) + Ba^{2+}(aq) + 2OH^- (aq) \rightarrow Ba^{2+}(aq) + 2Br^- (aq) + 2H_2O (l)\) Net ionic equation: \( 2H^+(aq) + 2OH^-(aq) \rightarrow 2H_2O(l) \)

Step-by-step solution

Write the balanced chemical equation

The first thing we need to do is write the balanced chemical equation for the reaction between HBr and Ba(OH)₂. The general equation for a neutralization reaction is: Acid + Base → Salt + Water Hydrobromic acid (HBr) is an acid, and barium hydroxide (Ba(OH)₂) is a base. When they react, they will form a salt and water as products. In this case, the salt will be barium bromide (BaBr₂). Here's the balanced equation: \( 2HBr + Ba(OH)_2 \rightarrow BaBr_2 + 2H_2O \)

Break down the compounds into ions

Now, we need to break down the reactants and products into their respective ions: - Hydrobromic acid (\(HBr\)) \(-> H^+ + Br^-\) - Barium hydroxide (\(Ba(OH)_2\)) \(-> Ba^{2+} + 2OH^-\) - Barium bromide (\(BaBr_2\)) \(-> Ba^{2+} + 2Br^-\) - Water (\(H_2O\)) remains as \(H_2O\), as it does not dissociate.

Write the complete ionic equation

Using the ionic forms of the reactants and products, we can write the complete ionic equation: \(2H^+ (aq) + 2Br^- (aq) + Ba^{2+}(aq) + 2OH^- (aq) \rightarrow Ba^{2+}(aq) + 2Br^- (aq) + 2H_2O (l)\)

Write the net ionic equation

To find the net ionic equation, we can cancel out the spectator ions that appear on both sides of the complete ionic equation. In this case, the spectator ions are \(Ba^{2+}\) and \(2Br^-\). The net ionic equation is: \( 2H^+(aq) + 2OH^-(aq) \rightarrow 2H_2O(l) \) Thus, we have the complete ionic equation and the net ionic equation for the neutralization reaction between hydrobromic acid and barium hydroxide.

Key concepts

Complete Ionic Equation

In chemical reactions, particularly those occurring in aqueous solutions, it's essential to fully understand the transformation of reactants into products. The complete ionic equation is a way to express these reactions in detail. It provides a clear breakdown of all ions present in the solution before and after the reaction.
When hydrobromic acid (HBr) and barium hydroxide \(Ba(OH)_2\) react, the complete ionic equation demonstrates how these substances dissociate into their constituent ions.

• Hydrobromic acid dissociates into \(H^+\) and \(Br^-\) ions.
• Barium hydroxide dissociates into \(Ba^{2+}\) and \(2OH^-\) ions.
• The resulting products form barium bromide and water. Barium bromide dissociates into \(Ba^{2+}\) and \(2Br^-\), while water remains as \(H_2O(l)\).

In this reaction:\[2H^+ (aq) + 2Br^- (aq) + Ba^{2+}(aq) + 2OH^- (aq) \rightarrow Ba^{2+}(aq) + 2Br^- (aq) + 2H_2O (l)\]All ions should be present in their ionic form, except those that do not dissociate, such as water in this case. This detailed depiction helps in understanding which ions are actually involved in the chemical process and which remain unchanged.

Net Ionic Equation

The net ionic equation offers a simplified glimpse into the core changes occurring during a chemical reaction. While the complete ionic equation displays all ions present, the net ionic equation removes those unaltered spectator ions, focusing on the essential elements of the reaction.

In the neutralization reaction between hydrobromic acid and barium hydroxide, it's vital to identify which ions participate directly in forming new substances. Upon assessing the complete ionic equation, you'll find that the significant active participants are \(H^+\) and \(OH^-\) ions.

• These ions react to form water, \(2H_2O(l)\).
• Meanwhile, \(Ba^{2+}\) and \(2Br^-\) ions can be removed as spectators, because they do not participate in creating any new compounds.

The resulting net ionic equation, stripped of spectators, is:\[2H^+(aq) + 2OH^-(aq) \rightarrow 2H_2O(l)\]This concise expression highlights the transformation of hydrogen and hydroxide ions into water, making it easier to grasp the core reaction beyond the distractions of uninvolved ions.

Spectator Ions

Spectator ions are fascinating components of ionic reactions. Although they play no direct role in the reaction's outcome, they remain present, unchanged throughout the entire process. Understanding their role is crucial, as it helps to differentiate between active participants and passive bystanders in the chemical reaction.
In the example of hydrobromic acid reacting with barium hydroxide, the spectator ions identified from the complete ionic equation are \(Ba^{2+}\) and \(2Br^-\). These ions do not participate in the formation of the water product:

• \(Ba^{2+}\) remains dissolved in the solution as \(Ba^{2+}(aq)\).
• \(2Br^-\) also stays dissolved as \(2Br^-(aq)\).

Their presence is, however, critical to maintaining the charge balance of the solution. By recognizing spectator ions, chemists can focus on the ions directly engaged in the formation of new compounds, allowing for a clearer understanding of the reaction's essentials.