A 25.00-mL aliquot of 0.100 M KOH is titrated with 0.065 2 M HCl. Calculate the pH after 40.00 mL of 0.065 2 M HCl has been added.

Calculate pBa2+ after 35.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100 M Ba2+ in the presence of 0.100 M nitrilotriacetate. The solution is buffered at pH 10. = 1.48 × 10−4. = 0.30 at pH 10. Kf = 7.59 × 107 for BaY2−.

The Ka value for CH3CH2NO2 is 2.7 × 10−9. Calculate Kb for . Ans= x 10^

Calculate the pH of a 0.150 M maleic acid solution. pK1 = 1.92 and pK2 = 6.27 for maleic acid.

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.