A certain weak acid, HA, with a Ka value of 5.61 x 10 6, is titrated with NaOH. Part A A solution is made by titrating 7.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ΑΣφ ? pH = Part B More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 36.0 mL ? Express the pH numerically to two decimal places. ΑΣφ ? pH =

You are titrating 90.0 mL of a weak base solution (A-) with a concentration of 0.0515 M, using an HCl solution with a concentration of 0.0662 M. Note that the Ka Value for the conjugate acid , HA, is 5.6 x 10-10 . a) What is the pH of the initial weak base solution? b) What is the pH of the solution at the equivalence point? c) What is the pH of the solution when an additional 10 mL of HCl solution is added after reaching the equivalence point?

The Ka of hydrocyanic acid (HCN) is 4.0 × 10-10.  Determine the pH of a 0.300 mol/L solution of hydrocyanic acid. [3 T]                1. What is the pH at the equivalence point if 25.00 mL of the                 hydrocyanic acid is titrated with 0.300 mol/L NaOH.

A solution is made by combining 10.0 mL of 17.5 M acetic acid with 5.56 g of sodium acetate and diluting to a total volume of 1.50 L. Part A Calculate the pH of the solution. Express your answer using two decimal places Hν ΑΣφ ? pH =