Find the approximate percentage of chlorine,  bromine, and iodine in the original sample?

You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?

There is a solution containing two metal cations. The goal is to separate them by slowly and carefully adding a solution of an anion, until one mental cation precipitates as a compound with that anion, leaving the other metal cation still in solution. M+ is Ag+, M2+ is Ca2+, anion is SO4 2-, first Ksp is 1.2 x 10-5, second Ksp is 6.1 x 10-5, and the starting concentrations of M+ is 1.50 x 10-2 M and M2+ is 3.50 x 10-2M. Using these values, predict which metal will precipitate first and what concentration of anion the precipitation will begin.

Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?