To determine the acid in the given reaction:
[tex]\[ \text{HBr} + \text{KOH} \rightarrow \text{KBr} + \text{H}_2\text{O} \][/tex]
Let's break down the process step-by-step:
1. Identify the reactants and products:
- Reactants: HBr and KOH
- Products: KBr and H₂O
2. Understand the nature of each reactant:
- HBr (Hydrobromic acid): This is a strong acid, as it completely dissociates in water to give H⁺ (proton) and Br⁻ (bromide ion).
[tex]\[ \text{HBr} \rightarrow \text{H}^+ + \text{Br}^- \][/tex]
- KOH (Potassium hydroxide): This is a strong base, as it completely dissociates in water to give K⁺ (potassium ion) and OH⁻ (hydroxide ion).
[tex]\[ \text{KOH} \rightarrow \text{K}^+ + \text{OH}^- \][/tex]
3. Understand the products formed:
- KBr (Potassium bromide): This is a salt formed from the neutralization reaction between the acid (HBr) and the base (KOH).
[tex]\[ \text{K}^+ + \text{Br}^- \rightarrow \text{KBr} \][/tex]
- H₂O (Water): It is formed from the reaction between H⁺ (proton) from the acid and OH⁻ (hydroxide ion) from the base.
[tex]\[ \text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} \][/tex]
4. Determining the acid:
- From the reactants, HBr is the compound that donates a proton (H⁺) in the reaction.
- This ability to donate H⁺ indicates that HBr is the acid in this reaction.
Thus, in the reaction [tex]\( \text{HBr} + \text{KOH} \rightarrow \text{KBr} + \text{H}_2\text{O} \)[/tex], the acid is:
[tex]\[ \boxed{\text{HBr}} \][/tex]
