Increasing the concentration of reactants in a chemical reaction typically leads to an increase in the reaction rate. This is because a higher concentration of reactants results in more frequent collisions between the reacting molecules, which in turn increases the probability of successful collisions that lead to the formation of products.In the reaction between potassium permanganate KMnO and oxalic acid HCO in an acidic medium, the reaction can be represented by the following balanced equation:2 KMnO + 5 HCO + 3 HSO KSO + 2 MnSO + 10 CO + 8 HOHere, potassium permanganate is reduced to manganese II sulfate MnSO , and oxalic acid is oxidized to carbon dioxide CO and water HO . The acidic medium is provided by sulfuric acid HSO , which remains unchanged throughout the reaction.If the concentration of either potassium permanganate or oxalic acid is increased, the reaction rate will increase due to the higher frequency of collisions between the reactant molecules. This will result in a faster formation of products MnSO, CO, and HO and a quicker consumption of the reactants KMnO and HCO . However, it is important to note that increasing the concentration of one reactant without changing the other may not lead to a proportional increase in the reaction rate, as the reaction rate is also dependent on the concentration of the other reactant.