Calculate the pH during the titration of 50.00 mL of 0.0500 M  NaOH with 0.1000 M HCl at 25°C after the addition of the  following volumes of reagent: (a) 24.50 mL, (b) 25.00 mL, (c) 25.50 mL

Calculate the pH during the titration of 150 mL of 0.17 M Benzoic acid(aq) with 0.34M NaOH(aq) – after the following additions of titrant (NaOH): 1)0 mL2)45 mL3)75 mL4)100 mL

Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO: after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 106. 3. 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH:(aq) H(aq) H2NNH3*(aq) -> Before (mol) Change (mol) After (mol) ↑

In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added.  Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker.  After 17.65 mL of NaOH is added to the beaker, the equivalence point is reached.  What is the concentration (M) of the NaOH solution?