The following is a solubility product expression for Bi(OH)3: Ksp=  

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?  

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

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

Which of the following salts has the highest molar solubility in pure water?   Salt Ksp 1 Cd(OH)2 5.3×10–15 2 PbCrO4 1.8x 10–14 3 Mn(OH)2 2.0 x 10–13 4 Ni(OH)2 2.0 x 10–15 5 AgBr 5.0 x 10–13

Consider a buffer solution that is 0.400M butanoic acid (CH3CH2CH2COOH) and 0.500M sodium butanoate. Ka (butanoic acid) = 1.61 x10-5 Calculate the [H+], [OH-], pH, and pOH for this buffer. (12 pts) Calculate the pH of this buffer after adding 22.0 mL of 2.2M NaOH to 1.0 L of the solution (Hint: 1.0 L + 22 mL = 1.0 L according to the rules of addition for s.f.). (2 pts) To receive full credit, show all work in handwriting or use the software showing calculations and units properly and clearly.

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

Use the Henderson-Hasselbalch equation to calculate the pH of the solution prepared by dissolving  0.55 mol of a weak acid (Ka=2.77×10-5) and 0.78 mol of its conjugate base in enough water to make 1.00L of buffer solution

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.

Which of the following pairs of substances will NOT make aqueous buffer solutions (consider the products of acid-base reactions to get a correct answer)? KF, HF KOH, HF KOH, HBr NaClO, HNO3 HC2H3O2, NaOH  NaOH, HNO3 KCl, HCl