Question

Identify the ions that exist in each aqueous solution, and specify the concentration of each ion. (a) 0.12 M BaCl2

a) Ba²+ (0.12 M), Cl⁻ (0.24 M)
b) Ba²+ (0.24 M), Cl⁻ (0.12 M)
c) Ba²+ (0.12 M), Cl⁻ (0.12 M)
d) Ba²+ (0.24 M), Cl⁻ (0.24 M)

Answer 1

The correct answer is that in a 0.12 M solution of BaCl2, the ions present are Ba2+ with a concentration of 0.12 M and Cl- with a concentration of 0.24 M.

Step-by-step explanation:

The question involves identifying the ions present in an aqueous solution of BaCl2 and their concentrations. When dissolved in water, BaCl2 dissociates into one Ba2+ ion and two Cl- ions. Therefore, for every mole of BaCl2, there is one mole of Ba2+ ion and two moles of Cl- ions.

Given a 0.12 M solution of BaCl2, the concentration of Ba2+ will remain at 0.12 M because there is one Ba2+ ion for each formula unit of BaCl2. However, the concentration of Cl- will be twice that of Ba2+ because there are two Cl- ions for each formula unit of BaCl2, resulting in a concentration of 0.24 M for Cl-.