The pH of the half-titrated solution is 4.70, the concentration of acetic acid is 1.00 M and the C2H3O2 is 1.00 M. Calculate the Ka for the solution. 5.01 x 104 O 5.01 x 103 O2x 10-5 O 2.0 x 104

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.580 moles of a monoprotic weak acid (Ka = 2.5 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? PH =

Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid.  The Kb for hydrazine is 3.00x10-6. 9.39 3.32 4.80 9.60 4.70 3.22

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka = 5.3 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?