Question

What is the total molar concentration of all the ions in a 0.0250 M solution of the following salts in water?

Answer 1

The total molar concentration of all ions in a 0.0250 M solution of the given salts in water is 0.0500 M.

Step-by-step explanation:

In a solution of salts, each salt dissociates into its constituent ions when dissolved in water. The concentration of ions in the solution is twice that of the original salt concentration due to the dissociation of each salt into two ions. For example, for a salt represented as
`\(AB_2\)`, it dissociates into
`\(A^(2+)\) and \(2B^-\)` ions. Consequently, the molar concentration of ions is doubled.

Given a 0.0250 M solution, the effective concentration of ions is
`\(0.0250 M * 2 = 0.0500 M\)`. This is because each salt contributes to the molar concentration of both cations and anions. The ions act independently in solution, and their combined molar concentration is the sum of the concentrations of each individual ion. Therefore, for the specified solution, the total molar concentration of all ions is 0.0500 M.

It's important to note that this concept applies to all salts that dissociate completely in solution. The total molar concentration of ions is a key parameter in understanding the chemical behavior and reactivity of the solution, providing a basis for various applications in analytical chemistry and chemical processes.