Standardized solutions of KBrO3 are frequently used in redox titrations. The necessary solution can be made by dissolving KBrO3 in water and then titrating it with an As(III) solution. What is the molar concentration of a KBrO3 solution if 28.55 mL of the solution is needed to titrate 1.550 g of As2O3? See Problem 4.128 for the balanced equation. (As2O3 dissolves in aqueous acid solution to yield H3AsO3: As2O3 + 3 H2OS 2 H3AsO3.)

Key Concepts

Redox Reactions

Redox reactions involve the transfer of electrons between two species, resulting in changes in oxidation states. In the context of titrations, one reactant is oxidized while the other is reduced. Understanding the oxidation states of the elements involved, such as arsenic in As2O3 and bromine in KBrO3, is crucial for determining the stoichiometry of the reaction and calculating concentrations.

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant to a solution until a reaction endpoint is reached, often indicated by a color change. In this case, the volume of KBrO3 solution required to completely react with a known mass of As2O3 allows for the calculation of the molarity of the KBrO3 solution.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (mol/L). To find the molarity of the KBrO3 solution, one must first calculate the moles of As2O3 used in the titration and then use the volume of KBrO3 solution to determine its concentration, applying the stoichiometry from the balanced chemical equation.