To determine the products of the given replacement reaction:
[tex]\[ \text{BeSO}_4 + 2 \text{NH}_4\text{OH} \rightarrow \][/tex]
We need to analyze the reactants and apply the concept of double displacement reaction, where the cations and anions of the reactants switch places to form new compounds.
Let's break down the reaction:
1. Reactants:
- Beryllium sulfate ([tex]\(\text{BeSO}_4\)[/tex])
- Ammonium hydroxide ([tex]\(\text{NH}_4\text{OH}\)[/tex])
2. Double Displacement Reaction:
- Beryllium sulfate will dissociate into [tex]\(\text{Be}^{2+}\)[/tex] and [tex]\(\text{SO}_4^{2-}\)[/tex].
- Ammonium hydroxide will dissociate into [tex]\(\text{NH}_4^{+}\)[/tex] and [tex]\(\text{OH}^-\)[/tex].
3. Ion Combination:
- The beryllium ion ([tex]\(\text{Be}^{2+}\)[/tex]) will combine with the hydroxide ions ([tex]\(\text{OH}^-\)[/tex]) to form beryllium hydroxide ([tex]\(\text{Be(OH)}_2\)[/tex]).
- The ammonium ions ([tex]\(\text{NH}_4^{+}\)[/tex]) will combine with the sulfate ions ([tex]\(\text{SO}_4^{2-}\)[/tex]) to form ammonium sulfate ([tex]\(\left(\text{NH}_4\right)_2\text{SO}_4\)[/tex]).
Thus, the balanced chemical equation is:
[tex]\[ \text{BeSO}_4 + 2 \text{NH}_4\text{OH} \rightarrow \text{Be(OH)}_2 + \left( \text{NH}_4\right)_2 \text{SO}_4 \][/tex]
The products of this reaction are:
- Beryllium hydroxide ([tex]\(\text{Be(OH)}_2\)[/tex])
- Ammonium sulfate ([tex]\(\left( \text{NH}_4\right)_2 \text{SO}_4\)[/tex])
