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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]$\left( C_2 H_3 O_2^{-}\right)$[/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(I) [tex]$\left( Hg_2^{2+}\right)$[/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].

Use the solubility rules and the periodic table to predict the product that will precipitate out in the reaction:
[tex]$
K_2SO_4(aq) + Ba(NO_3)_2(aq) \rightarrow \text{?}
$[/tex]

A. [tex]$KNO_3$[/tex]
B. [tex]$Ba(NO_3)_2$[/tex]
C. [tex]$K_2SO_4$[/tex]
D. [tex]$BaSO_4$[/tex]



Answer :

GinnyAnswer
To predict the products of the reaction:
[tex]\[ \text{K}_2\text{SO}_4(\text{aq}) + \text{Ba(NO}_3)_2(\text{aq}) \][/tex]

we need to perform a double displacement reaction, which involves swapping the cations and anions between the reactants. This results in the formation of two new products. Here are the steps:

1. Identify the cations and anions in the reactants:
- Potassium sulfate ([tex]\(\text{K}_2\text{SO}_4\)[/tex]):
- Cation: [tex]\( \text{K}^+ \)[/tex]
- Anion: [tex]\( \text{SO}_4^{2-} \)[/tex]
- Barium nitrate ([tex]\(\text{Ba(NO}_3)_2\)[/tex]):
- Cation: [tex]\( \text{Ba}^{2+} \)[/tex]
- Anion: [tex]\( \text{NO}_3^- \)[/tex]

2. Swap the cations and anions to form new products:
- Potassium will pair with nitrate to form potassium nitrate ([tex]\(\text{KNO}_3\)[/tex]).
- Barium will pair with sulfate to form barium sulfate ([tex]\(\text{BaSO}_4\)[/tex]).

3. Write the possible products:
[tex]\[ \text{K}_2\text{SO}_4(\text{aq}) + \text{Ba(NO}_3)_2(\text{aq}) \rightarrow 2\text{KNO}_3(\text{aq}) + \text{BaSO}_4(\text{s}) \][/tex]

4. Apply the solubility rules to determine the solubility of the products:
- According to Rule 1 and 2, nitrates ([tex]\( \text{NO}_3^- \)[/tex]) are always soluble. Therefore, potassium nitrate ([tex]\( \text{KNO}_3 \)[/tex]) will be soluble.
- According to Rule 4, most sulfates ([tex]\( \text{SO}_4^{2-} \)[/tex]) are soluble, except for those containing [tex]\( \text{Ba}^{2+} \)[/tex], among others. This means barium sulfate ([tex]\( \text{BaSO}_4 \)[/tex]) will be insoluble and form a precipitate.

Therefore, the reaction predicts:
- The precipitate product is barium sulfate ([tex]\( \text{BaSO}_4 \)[/tex]).
- The soluble product is potassium nitrate ([tex]\( \text{KNO}_3 \)[/tex]).

Conclusion:

The product that will precipitate out in the reaction is:
[tex]\[ \text{BaSO}_4 \][/tex]

The correct answer is:

A. [tex]\( \text{KNO}_3 \)[/tex]

This is a tricky question because actually there is no appropriate answer present.

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