Find the pH of the two equivalence points and the volume (mL) of 0.0400 M KOH needed to reach them in the titration of 17.3 mL of 0.130 M H2CO3.

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.62 M NH3 with 0.20 M HCl. Kb(NH3)= 1.8 x 10^-5

Find the pH and the volume (mL) of 0.527 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5H5N, Kb = 1.7 ×10−9)

Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use a BCA table to detrmine the moles of reactant and product after the reaction of the acid and base. Ignore the amount of liquid water. Then, set up an ICE table to identify the unknown. Then figure the pH.

Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl.  The Ka of HN3 is 2.2 x 10–5.   What is the pH at the equivalence point?

Acid-Base Titrations. What type of chemical substances are present at the half-equivalence point in a weak acid-strong base titration when pH=pKa?

Calculate the pH at the equivalence point for the titration of 0.230 M methylamine (CH 3 NH 2 ) with 0.230 M HCI. The Kb of methylamine is 5.0 * 10 ^ - 4

Consider the titration of 25.0 mL of 0.766 M KOH with 1.25 M HBr. Calculate the pH after the addition of 17.64mL of HBr

Do all titrations of a strong base with a strong add have the same PH at the equivalence point?

25.0 mL of 0.200 M  HNO2 is titrated to its equivalence point with 1.00 M  NaOH. What is the pH at the equivalence point?