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Chapter 8: Problem 132

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

Short Answer

Expert verified
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

01

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: \( 2HBr + Ba(OH)_2 \rightarrow BaBr_2 + 2H_2O \)
02

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.
03

Write the complete ionic equation

Using the ionic forms of the reactants and products, we can write the complete ionic equation: \(2H^+ (aq) + 2Br^- (aq) + Ba^{2+}(aq) + 2OH^- (aq) \rightarrow Ba^{2+}(aq) + 2Br^- (aq) + 2H_2O (l)\)
04

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.

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