0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in mL, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 9.54.   acid/base pairs to use: Ka pKa HCO2H/NaHCO2 1.8×10-4 3.74 H2CO3/NaHCO3 4.2×10-7 6.38 HBO3/NaH2BO3 7.3×10-10 9.14 NaHCO3/Na2CO3 4.8×10-11 10.32

Consider how to prepare a buffer solution with pH = 2.97 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.418-M solution of weak acid with 0.351 M potassium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the potassium hydroxide solution would have to be added to the acid solution of your choice?

1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL pure water.

A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.