Certainly! Let's solve the chemical reaction step by step.
1. Identify the reactants:
- Weak base: [tex]\( \text{CH}_3\text{NH}_2 \)[/tex] (methylamine)
- Strong acid: [tex]\( \text{HClO}_3 \)[/tex] (chloric acid)
2. Reaction type: This is a reaction between a weak base and a strong acid.
3. Ionic dissociation:
- The weak base [tex]\( \text{CH}_3\text{NH}_2 \)[/tex] does not fully dissociate in water, but it can accept a proton [tex]\( (\text{H}^+) \)[/tex].
- The strong acid [tex]\( \text{HClO}_3 \)[/tex] almost completely dissociates in water to give [tex]\( \text{H}^+ \)[/tex] (protons) and [tex]\( \text{ClO}_3^- \)[/tex] (chlorate ions).
4. Formation of products:
- The methylamine [tex]\( \text{CH}_3\text{NH}_2 \)[/tex] will accept a proton [tex]\( \text{H}^+ \)[/tex] from [tex]\( \text{HClO}_3 \)[/tex], forming the methylammonium ion [tex]\( \text{CH}_3\text{NH}_3^+ \)[/tex].
- The [tex]\( \text{ClO}_3^- \)[/tex] ion remains as the conjugate base.
5. Balanced chemical reaction:
- The balanced reaction can be written by combining these species:
[tex]\[
\text{CH}_3\text{NH}_2(\text{aq}) + \text{HClO}_3(\text{aq}) \rightarrow \text{CH}_3\text{NH}_3^+(\text{aq}) + \text{ClO}_3^-(\text{aq})
\][/tex]
So, the resulting acid is the methylammonium ion [tex]\( \text{CH}_3\text{NH}_3^+ \)[/tex] and the resulting base is the chlorate ion [tex]\( \text{ClO}_3^- \)[/tex].
Thus, the complete balanced chemical reaction is:
[tex]\[
\text{CH}_3\text{NH}_2(\text{aq}) + \text{HClO}_3(\text{aq}) \rightarrow \text{CH}_3\text{NH}_3^+(\text{aq}) + \text{ClO}_3^-(\text{aq})
\][/tex]
