Consider the following chemical equilibrium: HCOOH(aq) + H_2O(aq) \rightleftharpoons HCOO^-(aq) + H_3O^+(aq). Which of the following graphs represents the perturbation on the system and the change of pH when water is evaporated from the container? **Chemical Equilibrium and pH Change** **Problem Statement:**Consider the following chemical equilibrium:\[ \text{HCOOH(aq) + H}_2\text{O(l) }\rightleftharpoons \text{ HCOO}^-(\text{aq}) + \text{ H}_3\text{O}^+(\text{aq}) \]Which of the following graphs represents the perturbation on the system and the change of pH when water is evaporated from the container?**Graphs Explanation:**The illustration contains four graphs labeled I through IV, each showing the change in a system’s equilibrium (Q) over time with respect to pH changes.- **Graph I:** - The equilibrium (Q) increases over time. - An upward arrow indicates an increase in pH.- **Graph II:** - The equilibrium (Q) decreases over time. - An upward arrow indicates an increase in pH.- **Graph III:** - The equilibrium (Q) decreases over time. - A downward arrow indicates a decrease in pH.- **Graph IV:** - The equilibrium (Q) increases over time. - A downward arrow indicates a decrease in pH.**Answer Choices:**Select the correct graph indicating how pH changes when water evaporates from the container:- a) I- b) II- c) III- d) IV**Instructions for Selection:**Use the up/down arrow keys to navigate and select your answer. When water evaporates, the concentration of ions increases, likely leading to a decrease in pH due to increased acidity in the solution. Select the graph that shows a decrease in pH over time.

In chemical systems, equilibrium describes a state where the forward and reverse reactions occur at equal rates, resulting in no net change in the concentration of reactants and products over time.For the weak acid dissociation equilibrium in question, formic acid (HCOOH) in water dissociates into formate ions (HCOO-) and hydronium ions (H3O+), but not completely, as it is a weak acid.When a system in equilibrium is disturbed, Le Chatelier's Principle predicts how the system will shift to re-establish equilibrium.Evaporating water from the system will increase the concentration of the acid and its ions due to the reduction of the solvent volume.The equilibrium will shift to oppose the concentration change, adhering to Le Chatelier's Principle, which in this case means the reaction will shift to the left, converting formate and hydronium ions back to formic acid and water.As the reaction shifts to the left, the concentration of hydronium ions decreases.A decrease in hydronium ion concentration means that the solution becomes less acidic, and thus the pH of the solution will increase.The graph that shows an increase in pH over time as a result of the decrease in hydronium ion concentration will correctly represent the system's response to water evaporation.Comparing the given graphs and applying the understood principles, the graph that shows an increase in pH over time—indicating a decrease in hydronium ion concentration—is the one that corresponds to the predicted shift in equilibrium.The correct graph will show the pH rising due to the reduction in hydronium ions as water evaporates from the container.The graph that correctly represents this behavior would be one that shows a decrease in Q (the quantity related to the concentration of hydronium ions) over time, coupled with an increase in pH.The graph that shows this pattern is graph II.