please show work for question #2 **Section: Objective #12:** Students can distinguish between strong and weak acids and bases in terms of definitions and properties, and perform basic acid-base reactions with the stoichiometry.1. **Explain how KCl, HBr, HCN, and C₂H₅₂O₁₁ behave differently at the particle level when they are dissolved in water.** You can draw pictures or write reactions if it helps your explanation.---2. **Identify each of the following solutions, as acidic, basic, or neutral:** (And only for the ones with "explain", briefly explain your choice) a. \( \text{H}_3\text{C}_6\text{O}_7 (\text{aq}) \) **______________________** b. A solution with [H₃O⁺] = [OH⁻] **______________________** c. A substance with a pH of 4.5 at 25°C **______________________** **Explain:** d. A covalent compound that ionizes with water and accepts an H⁺ from the water. **______________________**---3. **In the following reactions, identify the conjugate acid-base pairs.** \( \text{C}_2\text{H}_3\text{O}_2^- + \text{H}_2\text{O} \leftrightarrow \text{HC}_2\text{H}_3\text{O}_2 + \text{OH}^- \) \( \text{HClO}_4 + \text{H}_2\text{O} \leftrightarrow \text{H}_3\text{O}^+ + \text{ClO}_4^- \)---4. **What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H₂SO₄ solution is required to neutralize a 25.0-mL sample of the NaOH solution?** \( 2\text{NaOH (aq)} + \text{H}_2\text{SO}_4 (\text{aq}) \rightarrow \text{Na}_2\text{SO}_4 (\text{aq}) + 2\text{H}_2\text{O (l)} \)---5

Hello. There are multiple subparts in the question. The first three subparts have been solved. To receive solutions for the remaining subparts, please resubmit the whole question and mention the subparts to be solved. The nature of each of the given solutions has been identified below.HC2H3O2 (aq) acidic b. A solution with [H3O+] = [OH-] neutral When the concentration of hydronium ions and hydroxide ions in a solution are equal, then, the solution will be neutral as one hydroxide ion can neutralize one hydronium ion. c. A substance with a pH of 4.5 at 25⁰C acidic Determining the acidity of a solution by calculating the concentration of hydronium ions/ protons is not an easy process in every case. A pH scale has been established to give a measure of acidity. At room temperature, below a pH of 7, the solution is said to be acidic. Therefore, if a substance has a pH of 4.5, it is acidic in nature.