What is the molar solubility of brucite crystal, Mg(OH)2, in pure water. Ksp = 7.1 × 10−12 for brucite crystal, Mg(OH)2. Ans= x 10^

How many milliliters of 0.105 M HCl should be added to 200.0 mL of 0.010 9 M triethylamine to give a buffer with a pH of 10.20? The Kb of triethylamine is 5.26 × 10−4. Hint: Calculate the millimoles of triethylamine. Set the millimoles of the triethylammonium ion equal to x and the millimoles of triethylamine equal to the initial number of moles minus x. Calculate pKa from the Kb, insert the values into the Henderson-Hasselbalch equation, and solve for x, which is equal to the millimoles of HCl needed. Use the concentration of the HCl solution to calculate the volume. (Report to 1 decimal places)

Strong bases consist of alkali metal hydroxides and alkaline earth metal hydroxides, although the latter are far less soluble. Which statement is NOT true for strong bases?

Calculate the pH of a 0.002 50 M hemimellitic acid solution. pK1 = 2.86, pK2 = 4.30, and pK3 = 6.28 for hemimellitic acid.

Calculate the pH of 0.005 0 M phenylacetic acid. The Ka for phenylacetic acid is 4.90 × 10–11. Hint: Solve the weak-acid equilibrium problem, ignoring the change in the formal concentration of phenylacetic acid.

___________ expresses the margin of uncertainty associated with a measurement.

Calculate the pH of a 0.033 M Na2SO3 solution. pK1 = 1.66 and pK2 = 6.85 for sulfurous acid.

Calculate the percent dissociation for a 0.010 0 M HCN solution. Ka = 6.2 × 10−10 for HCN. (Report at least 3 decimal places) Hint: Solve the weak-acid equilibrium for , ignoring the change in the formal concentration of HCN. Divide the concentration of the cyanide ion by the formal concentration and multiply by 100.

Which of the following compounds is NOT an aprotic solvent?

Calculate pPb2+ at the equivalence point when 25.00 mL of 0.120 M  is titrated with 0.120 M Pb2+. Ksp = 7.4 × 10−14 for PbCO3.