Questions: Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and barium hydroxide are combined. (Use H^+ instead of H3O^+.)

Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and barium hydroxide are combined.
(Use H^+ instead of H3O^+.)

Transcript text: Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and barium hydroxide are combined. (Use $\mathrm{H}^{+}$instead of $\mathrm{H}_{3} \mathrm{O}^{+}$.)

Solution

Solution Steps

Step 1: Write the balanced molecular equation

First, we write the balanced molecular equation for the reaction between hydrobromic acid (HBr) and barium hydroxide (Ba(OH)₂):

\[ 2 \mathrm{HBr} (aq) + \mathrm{Ba(OH)}_2 (aq) \rightarrow \mathrm{BaBr}_2 (aq) + 2 \mathrm{H}_2\mathrm{O} (l) \]

Step 2: Write the complete ionic equation

Next, we write the complete ionic equation by dissociating all strong electrolytes into their ions:

\[ 2 \mathrm{H}^+ (aq) + 2 \mathrm{Br}^- (aq) + \mathrm{Ba}^{2+} (aq) + 2 \mathrm{OH}^- (aq) \rightarrow \mathrm{Ba}^{2+} (aq) + 2 \mathrm{Br}^- (aq) + 2 \mathrm{H}_2\mathrm{O} (l) \]

Step 3: Write the net ionic equation

To write the net ionic equation, we cancel out the spectator ions (ions that appear on both sides of the equation). In this case, the spectator ions are $\mathrm{Ba}^{2+}$ and $\mathrm{Br}^-$:

\[ 2 \mathrm{H}^+ (aq) + 2 \mathrm{OH}^- (aq) \rightarrow 2 \mathrm{H}_2\mathrm{O} (l) \]

Step 4: Simplify the net ionic equation

Finally, we simplify the net ionic equation by dividing all coefficients by 2:

\[ \mathrm{H}^+ (aq) + \mathrm{OH}^- (aq) \rightarrow \mathrm{H}_2\mathrm{O} (l) \]