2. You are to analyze an unknown acid sample found at a crime scene to determine whether nitric acid (HNO3) was used to spike a sample of Kool-Aid. Law enforcement has a suspect and obtained his lab notes. The notes show a pH for the sample of Kool-Aid as 1.622. You need to verify this pH value and have at your lab pure sodium hydroxide (NaOH) pellets and recall that sodium hydroxide will react with acids as follows: (11marks) a. What is the balanced neutralization equation? b. Determine the molarity for the NaOH solution if a mass of 5.678g was dissolved to prepare 1000.0mL of the titrant solution. c. You titrate 50.00mL of this spiked Kool-Aid with the prepared NaOH solution from b). Several drops of the indicator are added to this solution, and a titrant is added until the endpoint is observed. The data for the NaOH titrant volume as read from the burette is recorded as follows: What is the volume used for the titration? Volume final (Vf): 23.45mL Volume initial(Vi): 0.32mL d. Calculate the concentration of nitric acid found in the Kool-Aid. e. Based on your acid-base titration results, what is the pH of this Kool-Aid? Was the Kool-Aid tainted with nitric acid? [YES or NO] Circle