Consider the possible acid-base reactions and answer the following question: Which buffer will have the greatest capacity upon the addition of limited amounts of bases?  

The molar solubility of the salt with generic formula AB3 is 8.87 × 10-3 M in pure water.  Calculate the Ksp for this salt.

Calculate the pH of the solution obtained by mixing 48.00 mL of 0.1110M NaOH and 52.00 mL of 0.0995M HCl

Which of the following pairs of substances will make aqueous buffer solutions (consider the products of acid-base reactions to get a correct answer)?  RbOH, HBr NaC2H3O2, HC2H3O2 KBr, HBr RbCl, HCl  NaClO, HNO3 HC2H3O2, NaOH  NaF, HF

Use the Henderson-Hasselbalch equation to calculate the pH of the solution prepared by dissolving  0.48 mol of NH3(Kb=1.77×10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution

If the pKa of HF is 3.14 and the pH of an HF/NaF solution is 3.04, then______________         

Which of the following salts has the highest molar solubility in pure water?   Salt Ksp 1 Ni(OH)2 2.0 x 10–15 2 Mn(OH)2 2.0 x 10–13 3 CaCO3   3.8 x 10–9 4 Fe(OH)2 8 x10–16 5 PbI2 6.5 x 10–9

Calculate the pH of the solution obtained by mixing 55.00 mL of 0.0954M HCl and 47.00 mL of 0.1095M NaOH.

The following is a solubility product expression for Ca3(PO4)2: Ksp=

Ka for HF is 6.8 x10–4.  Calculate Kb for F-?