Calculate the pH at each of the following points for the titration of 100 mL of 0. 6 M dl-Histidine with the following volumes of 1.20 M sodium hydroxide. H3His + H* + H2His Ka1 = 3.98x103 H2His + H* + HHis2- Ka2 = 9.12x10-7 HHİS2- + H* + His3- Ka3 = 4.67x10-10 Vol. of NaOH Calculated pH 135mL 150mL 175mL

Calculate the pH at 0, 10, 25, 50, and 60mL of titrant in the titration of 50ml, 0.1M HCOOH with 0.1M NaOH. ka= 1.80x10-4

Which acid as shown is most appropriate for preparation of a buffer solution with a pH of 3.1? Explain your choice.

Consider the titration of 50.0 mL of 1.00 M H3ASO4(Ka1 = 5.6\times 10-3, Ka2 = 1.7\times 10-7, Ka3 = 4.0\times 10-12) with 1.00 MKOH. Calculate the pH after the addition of each of the following volumes of base. A) 25 mL B) 50 mL C) 75 mL D) 100 mL

Given a 0.100 M solution of anserine at its isoelectric point and ready access to 0.200 M HCl, 0.200 M NaOH and distilled water, describe the preparation of 1 L of 0.0300 M anserine buffered solution, pH 7.20.   Volume of stock solution needed = ? mL   Volume of HCl needed to adjust the imidazole group = ? mL   Volume of HCl needed to titrate the amino group = ? mL   Total HCl needed = ? mL

Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH₂CH₂COOH additions of titrant. (a) 10.00 mL: pH = (b) 20.10 mL: pH (c) 25.00 mL: pH = (Ka 1.54 × 10¯), with 0.1000 M NaOH solution after the following =