Final answer:
The calculation of the final concentration of iodate ions at equilibrium requires a specific balanced chemical equation, which was not provided.
Step-by-step explanation:
When considering the question of calculating the final concentration of iodate ions when the initial concentration is 0.15 M and the reaction reaches equilibrium with a K value of 2×10−8.
It is important to set up an ICE table (Initial, Change, Equilibrium) and apply the equilibrium constant expression corresponding to the reaction.
However, the question seems incomplete as it lacks the specific balanced chemical equation. We would need the balanced equation to determine the stoichiometric relationships between reactants and products in order to proceed with the calculations.
Changes in temperature can affect the equilibrium concentration of iodate ions, as increasing the temperature generally shifts the equilibrium position of an endothermic reaction to the right, increasing the concentration of products.
Whereas a decrease in temperature will favor the reactants in an exothermic reaction.Iodate ions play a major role in various chemical processes and industries, including acting as an oxidizing agent in the synthesis of organic compounds.
contributing to the iodination of table salt for health reasons, and being used in the manufacturing of dyes and disinfectants.A critical scenario involving the concentration of iodate ions could be in the treatment of water.
where a specific concentration of iodate is essential for proper disinfection without causing harm or undesired taste.