Answer :
Sure, let's predict the balanced products of the given reaction step-by-step.
The given reaction is: [tex]\( CaCl_2 (aq) + 2 AgNO_3 (aq) \)[/tex]
1. Identify the types of reactions:
- This is a double displacement reaction, which is typical for ionic compounds like the ones given. In a double displacement reaction, the cations and anions of the reactants switch partners.
2. Predict the products:
- The cation of [tex]\( CaCl_2 \)[/tex] is [tex]\( Ca^{2+} \)[/tex]
- The anion of [tex]\( CaCl_2 \)[/tex] is [tex]\( Cl^- \)[/tex]
- The cation of [tex]\( AgNO_3 \)[/tex] is [tex]\( Ag^+ \)[/tex]
- The anion of [tex]\( AgNO_3 \)[/tex] is [tex]\( NO_3^- \)[/tex]
By swapping the ions, we get:
- [tex]\( Ca^{2+} \)[/tex] pairs with [tex]\( NO_3^- \)[/tex] to form [tex]\( Ca(NO_3)_2 (aq) \)[/tex]
- [tex]\( Ag^+ \)[/tex] pairs with [tex]\( Cl^- \)[/tex] to form [tex]\( AgCl (s) \)[/tex]. Note that silver chloride [tex]\( AgCl \)[/tex] is insoluble in water and precipitates out as a solid.
3. Write the products including the states:
- [tex]\( Ca(NO_3)_2 (aq) \)[/tex] — Calcium nitrate is soluble in water.
- [tex]\( 2 AgCl (s) \)[/tex] — Silver chloride is insoluble in water and forms a precipitate.
4. Balance the equation:
- The given reaction equation is already balanced, with one [tex]\( CaCl_2 \)[/tex], two [tex]\( AgNO_3 \)[/tex], one [tex]\( Ca(NO_3)_2 \)[/tex], and two [tex]\( AgCl \)[/tex].
The balanced equation is:
[tex]\[ CaCl_2 (aq) + 2 AgNO_3 (aq) \rightarrow Ca(NO_3)_2 (aq) + 2 AgCl (s) \][/tex]
So, the products are:
[tex]\[ Ca(NO_3)_2 (aq) \][/tex]
[tex]\[ 2 AgCl (s)\][/tex]
The given reaction is: [tex]\( CaCl_2 (aq) + 2 AgNO_3 (aq) \)[/tex]
1. Identify the types of reactions:
- This is a double displacement reaction, which is typical for ionic compounds like the ones given. In a double displacement reaction, the cations and anions of the reactants switch partners.
2. Predict the products:
- The cation of [tex]\( CaCl_2 \)[/tex] is [tex]\( Ca^{2+} \)[/tex]
- The anion of [tex]\( CaCl_2 \)[/tex] is [tex]\( Cl^- \)[/tex]
- The cation of [tex]\( AgNO_3 \)[/tex] is [tex]\( Ag^+ \)[/tex]
- The anion of [tex]\( AgNO_3 \)[/tex] is [tex]\( NO_3^- \)[/tex]
By swapping the ions, we get:
- [tex]\( Ca^{2+} \)[/tex] pairs with [tex]\( NO_3^- \)[/tex] to form [tex]\( Ca(NO_3)_2 (aq) \)[/tex]
- [tex]\( Ag^+ \)[/tex] pairs with [tex]\( Cl^- \)[/tex] to form [tex]\( AgCl (s) \)[/tex]. Note that silver chloride [tex]\( AgCl \)[/tex] is insoluble in water and precipitates out as a solid.
3. Write the products including the states:
- [tex]\( Ca(NO_3)_2 (aq) \)[/tex] — Calcium nitrate is soluble in water.
- [tex]\( 2 AgCl (s) \)[/tex] — Silver chloride is insoluble in water and forms a precipitate.
4. Balance the equation:
- The given reaction equation is already balanced, with one [tex]\( CaCl_2 \)[/tex], two [tex]\( AgNO_3 \)[/tex], one [tex]\( Ca(NO_3)_2 \)[/tex], and two [tex]\( AgCl \)[/tex].
The balanced equation is:
[tex]\[ CaCl_2 (aq) + 2 AgNO_3 (aq) \rightarrow Ca(NO_3)_2 (aq) + 2 AgCl (s) \][/tex]
So, the products are:
[tex]\[ Ca(NO_3)_2 (aq) \][/tex]
[tex]\[ 2 AgCl (s)\][/tex]