1. During the titration of an HcIO4 solution with 0.1032 M NaOH, quantitative analysis student Alcohol became distracted and overshot the end point. A fellow student, I. M. Smart, suggested that he simply record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.00 ml, the volume of NaOH added was 28.06 ml, and it took 3.47 ml of 0.1094 M HCl to back titrate the naOH, calculate the molar concentration of the original HclO4 solution.

You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1379 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 mL. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 13.88 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution? Concentration = A 60.00 mL solution of 0.4500 M AgN03. was added to a solution of AsO43-. Ag3AsO4 precipitated and was filtered off. Fe3+ was added and the solution was titrated with 0.2400 M KSCN. After 36.90 mL of KSCN solution had been added, the solution turned red. What mass of ASO43- was in the original solution?