How does increasing the concentration of a species affect the equilibrium position?

When the concentration of a species in a chemical equilibrium is increased, the system responds according to Le Chatelier's Principle. This principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will shift in a direction that counteracts that change in order to restore a new equilibrium.

In this case, increasing the concentration of a particular species would result in the system adjusting to mitigate that increase. Specifically, the equilibrium will shift towards the reaction that consumes or removes that species, thus favoring the opposite reaction. For instance, if the equilibrium involves a reactant A forming products B and C, increasing A would cause the system to shift to the right, producing more B and C, and effectively reducing the concentration of A.

This response aligns with the notion that chemical systems tend to seek balance; thus, the correct understanding is that an increase in concentration of a species favors the reaction that removes or consumes that species from the system.