Answer :
First, let's consider the solubility rules provided and the ions involved: [tex]$Na^{+}$[/tex], [tex]$PO_4^{3-}$[/tex], [tex]$V^{3+}$[/tex], and [tex]$Cl^{-}$[/tex].
1. Sodium Compounds: According to the first rule, compounds containing group 1 alkali metals (like sodium, [tex]$Na^{+}$[/tex]) are soluble. Therefore, any sodium compounds formed will be soluble.
- [tex]$Na_3PO_4$[/tex]: Sodium phosphate is soluble.
- [tex]$NaCl$[/tex]: Sodium chloride is soluble.
2. Chlorides: According to the third rule, chlorides ([tex]$Cl^{-}$[/tex]) are generally soluble, except for compounds containing [tex]$Ag^{+}$[/tex], [tex]$Hg_2^{2+}$[/tex], and [tex]$Pb^{2+}$[/tex], which are not present in this situation. Therefore, any chlorides formed will also be soluble.
- [tex]$VCl_3$[/tex]: Vanadium chloride should be considered for solubility based on this rule.
3. Phosphates: According to the solubility rules, phosphates ([tex]$PO_4^{3-}$[/tex]) are generally insoluble except when paired with group 1 metals (like sodium) or ammonium ([tex]$NH_4^+$[/tex]).
- [tex]$VPO_4$[/tex]: Vanadium phosphate would be insoluble because vanadium is not a group 1 metal or ammonium.
Given the information and applying the solubility rules, the compounds that can potentially form are:
1. [tex]$Na_3PO_4$[/tex] (sodium phosphate) – soluble.
2. [tex]$NaCl$[/tex] (sodium chloride) – soluble.
3. [tex]$VCl_3$[/tex] (vanadium chloride) – likely soluble, considering [tex]$Cl^{-}$[/tex] is generally soluble.
4. [tex]$VPO_4$[/tex] (vanadium phosphate) – insoluble.
Therefore, the insoluble compound that will precipitate out of the solution is:
A. [tex]$VPO_4$[/tex]
1. Sodium Compounds: According to the first rule, compounds containing group 1 alkali metals (like sodium, [tex]$Na^{+}$[/tex]) are soluble. Therefore, any sodium compounds formed will be soluble.
- [tex]$Na_3PO_4$[/tex]: Sodium phosphate is soluble.
- [tex]$NaCl$[/tex]: Sodium chloride is soluble.
2. Chlorides: According to the third rule, chlorides ([tex]$Cl^{-}$[/tex]) are generally soluble, except for compounds containing [tex]$Ag^{+}$[/tex], [tex]$Hg_2^{2+}$[/tex], and [tex]$Pb^{2+}$[/tex], which are not present in this situation. Therefore, any chlorides formed will also be soluble.
- [tex]$VCl_3$[/tex]: Vanadium chloride should be considered for solubility based on this rule.
3. Phosphates: According to the solubility rules, phosphates ([tex]$PO_4^{3-}$[/tex]) are generally insoluble except when paired with group 1 metals (like sodium) or ammonium ([tex]$NH_4^+$[/tex]).
- [tex]$VPO_4$[/tex]: Vanadium phosphate would be insoluble because vanadium is not a group 1 metal or ammonium.
Given the information and applying the solubility rules, the compounds that can potentially form are:
1. [tex]$Na_3PO_4$[/tex] (sodium phosphate) – soluble.
2. [tex]$NaCl$[/tex] (sodium chloride) – soluble.
3. [tex]$VCl_3$[/tex] (vanadium chloride) – likely soluble, considering [tex]$Cl^{-}$[/tex] is generally soluble.
4. [tex]$VPO_4$[/tex] (vanadium phosphate) – insoluble.
Therefore, the insoluble compound that will precipitate out of the solution is:
A. [tex]$VPO_4$[/tex]