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Advanced Reaction Patterns: Mastery Test

Two solutions are mixed, bringing together ions of [tex]\( \text{Na}^{+} \)[/tex], [tex]\( \text{PO}_4^{3-} \)[/tex], [tex]\( \text{V}^{3+} \)[/tex], and [tex]\( \text{Cr} \)[/tex]. Use the solubility rules to identify the composition of the salt that precipitates out of the solution.

A. [tex]\( \text{VPO}_4 \)[/tex]
B. [tex]\( \text{Na}_3\text{PO}_4 \)[/tex]
C. [tex]\( \text{VCl}_3 \)[/tex]
D. [tex]\( \text{NaCl} \)[/tex]

Sagot :

GinnyAnswer
Let's identify which salt precipitates out of the solution when ions [tex]\( Na^+ \)[/tex], [tex]\( PO4^{3-} \)[/tex], [tex]\( V^{3+} \)[/tex], and [tex]\( Cr \)[/tex] are mixed based on solubility rules.

1. Sodium Ion ([tex]\( Na^+ \)[/tex]): Salts containing sodium ions are generally soluble in water. This includes [tex]\( NaCl \)[/tex] and [tex]\( Na3PO4 \)[/tex].

2. Phosphate Ion ([tex]\( PO4^{3-} \)[/tex]): Phosphates are generally insoluble in water except for those of Group 1 (alkali metals like sodium, potassium) and ammonium. This means that salts such as [tex]\( VPO4 \)[/tex] (Vanadium(III) phosphate) can be insoluble.

3. Vanadium(III) Ion ([tex]\( V^{3+} \)[/tex]): Vanadium(III) salts need specific consideration. While chlorides like [tex]\( VCl3 \)[/tex] are typically soluble, phosphates of other metals generally are not.

4. Chromium ([tex]\( Cr \)[/tex]): Chromium alone in its elemental form will not form any salts directly from this context.

Evaluating the options:

A. [tex]\( VPO4 \)[/tex]: Vanadium(III) phosphate. Given that phosphates are generally insoluble except for those of alkali metals and ammonium, [tex]\( VPO4 \)[/tex] is expected to be insoluble and hence can precipitate out of the solution.

B. [tex]\( Na3PO4 \)[/tex]: Sodium phosphate. This is soluble because sodium salts are generally soluble.

C. [tex]\( VCl3 \)[/tex]: Vanadium(III) chloride. Chlorides are generally soluble except for a few exceptions like AgCl, PbCl2, and Hg2Cl2, making [tex]\( VCl3 \)[/tex] soluble in water.

D. [tex]\( NaCl \)[/tex]: Sodium chloride. This is soluble as sodium salts are generally soluble.

Therefore, the salt that will precipitate out of the solution is:
A. [tex]\( VPO4 \)[/tex]

This results from the fact that of the given ions, the combination of [tex]\( V^{3+} \)[/tex] and [tex]\( PO4^{3-} \)[/tex] will form an insoluble compound.

Final answer:

A. [tex]\( VPO4 \)[/tex]
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