What is the total molar concentration of ions in each of the following solutions? (b) A 0.225 M solution of HClO4

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Identify the dissociation reaction of HClO_4 in water: HClO_4 \rightarrow H^+ + ClO_4^-.

Recognize that HClO_4 is a strong acid and dissociates completely in solution.

Determine the concentration of each ion produced. Since the dissociation is complete, the concentration of H^+ ions is equal to the initial concentration of HClO_4, which is 0.225 M.

Similarly, the concentration of ClO_4^- ions is also 0.225 M because each molecule of HClO_4 produces one ClO_4^- ion.

Calculate the total molar concentration of ions by adding the concentrations of H^+ and ClO_4^- ions: 0.225 M + 0.225 M.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is a crucial concept in chemistry for quantifying how much of a substance is present in a given volume of solution, allowing for calculations involving reactions and properties of solutions.

Strong Acids and Ionization

Strong acids, like HClO4 (perchloric acid), completely dissociate in water, meaning that they release all of their hydrogen ions (H+) into the solution. This complete ionization is essential for determining the total molar concentration of ions, as each mole of a strong acid contributes an equivalent amount of H+ ions to the solution.

Total Molar Concentration of Ions

The total molar concentration of ions in a solution is the sum of the concentrations of all ions present. For a strong acid like HClO4, which dissociates into H+ and ClO4- ions, the total concentration is calculated by adding the concentration of H+ ions to that of ClO4- ions, providing a complete picture of the ionic composition of the solution.

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