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

If FeCl2, CuSO4, glucose (C6H12O6) and CaCr2O7 are thrown onto an icy road. Assuming they all can completely dissolve to form solutions of the same concentration in molality — which will decrease the freezing point of water more?

Balance the following redox reaction which happens in an acidic solution. What’s the coefficient of Fe3+? MnO4- + Fe2+ → Mn2+ + Fe3+

Is this map large scale or small scale? Why?

What is the latitude and longitude of the Football Stadium here in Jacksonville? List this in degrees, minutes, and seconds.