   Chapter 17, Problem 114SCQ

Chapter
Section
Textbook Problem

Which of the following barium salts should dissolve in a strong acid such as HCl: Ba(OH)2, BaSO4, or BaCO3?

Interpretation Introduction

Interpretation: The barium salt out of Ba(OH)2 BaSO4 and BaCO3 will dissolve in a strong acid such as HCl has to be predicted.

Concept introduction: The solubility of insoluble salts containing anions (conjugate base of a weak acid) such as hydroxide, acetate, carbonate, phosphate and sulfide increases in the presence of strong acid than in pure water. Whereas the solubility of insoluble salts containing anions (conjugate base of a strong acid) such as chlorides decreases in the presence of strong acid than in the pure water.

Explanation

Ba(OH)2 dissociates as,

Ba(OH)2(s)Ba2+(aq)+2OH(aq) (1)

The hydroxide ion is a strong conjugate base of weak acid H2O and therefore reacts with hydrochloric acid. The reaction of OH with strong hydrochloric acid decreases the concentration of the hydroxide ions in the solution and as a result, the reaction equilibrium in equation (1) shifts to right-hand side increasing the solubility of Ba(OH)2 This is the reason Ba(OH)2 is soluble in HCl.

OH(aq)+HCl(aq)H2O(l)+Cl(aq)

BaCO3 dissociates as,

BaCO3(s)Ba2+(aq)+CO32(aq) (2)

Carbonate ion is a strong conjugate base of weak carbonic acid. It reacts with strong hydrochloric acid to form weak carbonic acid. This decreases the concentration of the carbonate ions in the solution and as a result, the reaction equilibrium in equation (2) shifts to right-hand side increasing the solubility of BaCO3. This is the reason BaCO3 is soluble in HCl

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