Changing the concentration of reactants does not affect the equilibrium constant K for a chemical reaction. The equilibrium constant is a ratio of the concentrations of products to reactants raised to their respective stoichiometric coefficients at equilibrium, and it is a constant value for a given reaction at a specific temperature.However, changing the concentration of reactants can affect the position of the equilibrium, which is the actual concentrations of reactants and products at equilibrium. If the concentration of a reactant is increased, the system will shift towards the side of the products to re-establish equilibrium according to Le Chatelier's principle . Conversely, if the concentration of a reactant is decreased, the system will shift towards the side of the reactants.To measure the effect of changing the concentration of reactants on the equilibrium experimentally, you can follow these steps:1. Set up the reaction in a controlled environment, such as a closed container, and allow it to reach equilibrium.2. Measure the initial concentrations of reactants and products at equilibrium using appropriate analytical techniques e.g., spectrophotometry, titration, etc. .3. Calculate the initial equilibrium constant K using the initial concentrations of reactants and products.4. Change the concentration of one of the reactants by adding or removing a known amount of it.5. Allow the system to re-establish equilibrium.6. Measure the new concentrations of reactants and products at the new equilibrium.7. Calculate the new equilibrium constant K using the new concentrations of reactants and products.If the temperature remains constant during the experiment, you should observe that the equilibrium constant K remains the same, even though the concentrations of reactants and products have changed. This demonstrates that the equilibrium constant is not affected by changes in the concentration of reactants.