Penn State CHEM 113Experiment 14 Part 1: Acid-Base EquilibriaRead through the experimental procedure in Chemtrek and watch the associated experiment videos inCanvas. In the provided spaces, write a lab goal, summarize the procedure, record your observations,and complete all questions included in this report sheet. Experiment Goal. Complete before lab.Be able to interpret conductivity experiments, investigate acid-base equilibria from bromocresol green,determine acid dissociation equilibrium constants, use a universal indicator as a color probe to sense pHand investigate various quantitative features of acid-base chem through titration curves.Procedure:Thompson, S. PSU Chemtrek: Expt. 14 Acid Base Equilibria; Keiser, J., Hayden-McNeilPublishing: Plymouth, MI, 2020, pp 14-1 to 14-39.Section A. Conductimetry and the Strength of Acids and BasesPre-lab data collection and observations. Complete before lab.Using a clean conductivity probe, 6 liquid solutions are tested. Between each the leads is rinsed withdistilled water. Record whether each solution got a reading, if yes, at what level out of 10?Table 1:conductivity of various solutionsSolution:DistilledwaterTap waterCH3COOH0.1MNH3/ NH4OH0.1MNaOH0.1MHCl 0.1MReading:N/A5 / 104 / 105 / 108 / 109 / 10Question 1: Arrange the six solutions tested from the lowest to the highest conductivity. Explain the order observed—i.e., why do solutions of the same concentration have different conductivities? If you cannotdifferentiate between them, explain why not. DI < acetic acid < tap = ammonia/ammonium < sodium hydroxide < hydrochloric acid. Conductivity of a solution is dependent on the amount of charge carriers/ions a solution has. Each ofthese solutions tested have different amounts of ions (except distilled water) despite being the sameconcentration.Question 2:The conductivity of an H2SO4solution was followed as it was titrated with the strong base Ba(OH)2.Predict the relative conductivities of: H2SO4 + Ba(OH)2 → BaSO4 + 2H2O(a)the starting solution Will be more acidic and have removable ions. Meaning it will be conductive.(b)the solution at the equivalence point The acidic will be completely reacted with the base at the equivalence point, creating water and aninsoluble salt. Water will not consist of ions, so will not be conductive.