The reaction between hydrochloric acid HCl and sodium thiosulphate Na2S2O3 can be represented by the following balanced equation:2HCl aq + Na2S2O3 aq 2NaCl aq + H2O l + SO2 g + S s In this reaction, the reaction intermediates are the species that are formed and consumed during the reaction but do not appear in the overall balanced equation. The concentration of these intermediates can affect the rate of the reaction.The reaction between HCl and Na2S2O3 proceeds through a series of steps, involving the formation of reaction intermediates. One of the intermediates in this reaction is the thiosulfate ion S2O3^2- , which reacts with HCl to form the tetrathionate ion S4O6^2- , sulfur, and water. The tetrathionate ion can further react with HCl to form sulfur dioxide SO2 and more sulfur.The rate of the reaction depends on the concentration of the reactants and the reaction intermediates. According to the law of mass action, the rate of a reaction is directly proportional to the product of the concentrations of the reactants raised to the power of their stoichiometric coefficients. In this case, the rate of the reaction can be represented as:Rate = k[HCl]^m[S2O3^2-]^nwhere k is the rate constant, m and n are the reaction orders with respect to HCl and S2O3^2-, respectively.As the concentration of the reaction intermediates such as S2O3^2- increases, the rate of the reaction may increase or decrease, depending on the reaction mechanism and the role of the intermediate in the reaction. In some cases, the intermediate may act as a catalyst, speeding up the reaction, while in other cases, it may act as an inhibitor, slowing down the reaction.In the case of the reaction between HCl and Na2S2O3, the concentration of the reaction intermediates can affect the rate of the reaction by altering the availability of the reactants and the reaction pathway. However, the exact effect of the concentration of reaction intermediates on the rate of this reaction would require further investigation and experimentation to determine the reaction mechanism and the role of the intermediates in the reaction.