Consider the titration of 100.0 ml of 0.250 M HA (K = 5.0 x 10% pk, = 3.30) with 0.250 M NaOH. Determine the pH at the equivalence point. 4 7.00 5.80 C 11.59 8.35 9.86

A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box

What is a pH at the equivalence point when exactly 25.00 mL of 0.1000 M (CH3)2NH is titrated with 0.1000 M HBr? Kb((CH3)2NH) = 5.100e-4.  3.292    6.004  10.708  7.996

16.0mL of a 0.750M solution of H>COz are titrated with a 1.0OOM solution of KOH. At what volume of base will the equivalence point be reached? 42.7 mL 12.0 mL O24.0 mL 20.0 mL 21.3 mL