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Solubility Rules:

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

Which substance is most likely to form in a precipitation reaction?

A. calcium nitrate
B. copper(I) nitrate
C. iron(I) chloride
D. iron(II) sulfide
E. potassium sulfate



Answer :

GinnyAnswer
To determine which substance is most likely to form in a precipitation reaction, we need to analyze each option using the provided solubility rules:

1. Calcium nitrate ([tex]$\text{Ca(NO}_3\text{)_2}$[/tex]):
- According to Rule 2, nitrates ([tex]$\text{NO}_3{^-}$[/tex]) are soluble regardless of the cation. Therefore, calcium nitrate is soluble.

2. Copper(I) nitrate ([tex]$\text{CuNO}_3$[/tex]):
- Again, Rule 2 states that nitrates ([tex]$\text{NO}_3{^-}$[/tex]) are soluble regardless of the cation. Therefore, copper(I) nitrate is soluble.

3. Iron(I) chloride ([tex]$\text{FeCl}$[/tex]):
- According to Rule 3, chlorides ([tex]$\text{Cl}^-$[/tex]) are generally soluble, except when combined with silver ([tex]$\text{Ag}^+$[/tex]), mercury(I) ([tex]$\text{Hg}_2^{2+}$[/tex]), and lead ([tex]$\text{Pb}^{2+}$[/tex]). Since iron is not one of these exceptions, iron(I) chloride is soluble.

4. Iron(II) sulfide ([tex]$\text{FeS}$[/tex]):
- Rule 1 and 2 do not apply here. According to general solubility rules for sulfides ([tex]$\text{S}^{2-}$[/tex]), they are usually insoluble except when paired with group 1 alkali metals or ammonium ([tex]$\text{NH}_4{^+}$[/tex]). Since iron does not fall into these exceptions, iron(II) sulfide is insoluble.

5. Potassium sulfate ([tex]$\text{K}_2\text{SO}_4$[/tex]):
- According to Rule 4, sulfates ([tex]$\text{SO}_4^{2-}$[/tex]) are soluble except with calcium ([tex]$\text{Ca}^{2+}$[/tex]), strontium ([tex]$\text{Sr}^{2+}$[/tex]), barium ([tex]$\text{Ba}^{2+}$[/tex]), and lead ([tex]$\text{Pb}^{2+}$[/tex]). Potassium is a group 1 metal, so potassium sulfate is soluble.

Among these options, the substance that is insoluble and thus most likely to form in a precipitation reaction is:

D. iron(II) sulfide

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