Consider the titration of a 20.0-ml sample of 0.105 m hc2h3o2 with 0.125 m naoh. determine each quantity. a. the initial ph b. the volume of added base required to reach the equivalence point c. the ph at 5.0 ml of added base d. the ph at one-half of the equivalence point e. the ph at the equivalence point f. the ph after adding 5.0 ml of base beyond the equivalence

Percent ionization for a weak acid (ha) is determined by the following formula: percent ionization=[ha] ionized[ha] initial×100%for strong acids, ionization is nearly complete (100%) at most concentrations. however, for weak acids, the percent ionization changes significantly with concentration. the more diluted the acid is, the greater percent ionization.a certain weak acid, ha, has a ka value of 9.4×10? 7.part acalculate the percent ionization of ha in a 0.10 m solution.part bcalculate the percent ionization of ha in a 0.010 m solution