Question

solubility rules

1. compounds containing group 1 alkali metals or ammonium (nh₄⁺) are soluble.
2. nitrates (no₃⁻), chlorates (clo₃⁻), perchlorates (clo₄⁻), and acetates (c₂h₃o₂⁻) are soluble.
3. chlorides (cl⁻), bromides (br⁻), and iodides (i⁻) are soluble, except for compounds containing silver (ag⁺), mercury(i) (hg₂²⁺), and lead (pb²⁺).
4. sulfates (so₄²⁻) are soluble, except for compounds containing calcium (ca²⁺), strontium (sr²⁺), barium (ba²⁺), and lead (pb²⁺).
5. hydroxides (oh⁻), carbonates (co₃²⁻), and phosphates (po₄³⁻) are insoluble, except for compounds containing

use the solubility rules and the periodic table to predict the product that will precipitate out in the reaction.
k₂so₄(aq) + ba(no₃)₂(aq) → ?

a. kno₃
b. ba(no₃)₂
c. k₂so₄
d. k₂ba
e. baso₄

Explanation:

Step1: Identify the reaction type

This is a double - displacement reaction. The general form of a double - displacement reaction is \(AB + CD=AD + CB\). For the reaction \(K_{2}SO_{4}(aq)+Ba(NO_{3})_{2}(aq)\), the ions involved are \(K^{+}\), \(SO_{4}^{2 -}\), \(Ba^{2+}\), and \(NO_{3}^{-}\). So the possible products are \(KNO_{3}\) and \(BaSO_{4}\).

Step2: Apply solubility rules to each product

• For \(KNO_{3}\): According to solubility rule 2, nitrates (\(NO_{3}^{-}\)) are soluble, and \(K^{+}\) is a group 1 alkali metal ion. So \(KNO_{3}\) is soluble in water.
• For \(BaSO_{4}\): According to solubility rule 4, sulfates (\(SO_{4}^{2 -}\)) are soluble except for compounds containing \(Ba^{2+}\) (among others like \(Ca^{2+}\), \(Sr^{2+}\), \(Pb^{2+}\)). Since \(BaSO_{4}\) contains \(Ba^{2+}\) and \(SO_{4}^{2 -}\), it is insoluble and will precipitate out.

• Option B (\(Ba(NO_{3})_{2}\)) is a reactant, not a product. Option C (\(K_{2}SO_{4}\)) is a reactant, not a product. Option D (\(K_{2}Ba\)) is not a valid product of this reaction.

Answer:

E. \(BaSO_{4}\)