Question

Part A: Watch the animation and observe the titration process of a standard 0.100 M sodium hydroxide solution with 50.0 \rm ml of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titration are correct.Check all that apply.a - The titration process is based on a chemical reaction.b - The \rm pH of the solution at the equivalence point is 7.c - At the endpoint, the \rm pH of solution is 10 and the color of solution is pink.d - At the beginning of the titration process, the \rm pH of the solution increases rapidly.e - The chemical reaction involved in an acid-base titration is a neutralization reaction.f - Before any base is added to the solution, the \rm pH of the solution is high.g - In a titration process, the endpoint is reached before the equivalence point.h - The \rm pH of the solution changes very slowly at the equivalence point.Part B: 100 \rm mL of 1.00 M HCl solution is titrated with 1.00 M~ \rm NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint.Drag the appropriate items to their respective bins10.0mL of 1.00 M NaOH150 mL of 1.00 M NaOH5.00 mL of 1.00 M NaOH50.0 mL of 1.00 M NaOH200 mL of 1.00 M NaOHBINS:Before equivalent pointAt equivalent pointAfter equivalent pointPart C:A volume of 90.0 mL of a 0.400 M HNO3 solution is titrated with 0.470 M KOH. Calculate the volume of KOH required to reach the equivalence point.