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### Solubility Rules

1. Compounds containing group 1 alkali metals or ammonium [tex]\((NH_4^+)\)[/tex] are soluble.
2. Nitrates [tex]\((NO_3^-)\)[/tex], chlorates [tex]\((ClO_3^-)\)[/tex], perchlorates [tex]\((ClO_4^-)\)[/tex], and acetates [tex]\((C_2H_3O_2^-)\)[/tex] are soluble.
3. Chlorides [tex]\((Cl^-)\)[/tex], bromides [tex]\((Br^-)\)[/tex], and iodides [tex]\((I^-)\)[/tex] are soluble, except for compounds containing silver [tex]\((Ag^+)\)[/tex], mercury(1) [tex]\((Hg_2^{2+})\)[/tex], and lead [tex]\((Pb^{2+})\)[/tex].
4. Sulfates [tex]\((SO_4^{2-})\)[/tex] are soluble, except for compounds containing calcium [tex]\((Ca^{2+})\)[/tex], strontium [tex]\((Sr^{2+})\)[/tex], barium [tex]\((Ba^{2+})\)[/tex], and lead [tex]\((Pb^{2+})\)[/tex].

### Task

Two solutions are mixed, bringing together ions of [tex]\(Na^+, PO_4^{3-}, V^{3+},\)[/tex] and [tex]\(Cl^-\)[/tex]. Use the solubility rules to identify the composition of the salt that precipitates out of the solution.

A. [tex]\(VPO_4\)[/tex]

B. [tex]\(Na_3PO_4\)[/tex]

C. [tex]\(VCl_3\)[/tex]

D. [tex]\(NaCl\)[/tex]



Answer :

GinnyAnswer
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]

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