A 25.00-mL aliquot of 0.100 M sodium acetate (pKb = 9.244) is titrated with 0.125 M HCl. Calculate the pH after 10.00 mL of 0.125 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−.

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.

_________________ is a process in which the sample is thermally decomposed in the absence of added O2.

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.

You need to prepare 1.00 L of a pH 5.00 propionic acid buffer with a total concentration of 50 mM. Calculate the millimoles of propionic acid and sodium propionate needed to prepare the buffer. Ka = 1.34 × 10−5 for propionic acid. Hint: Set millimoles of propionate equal to x and millimoles of propionic acid equal to 50 − x. Insert into the Henderson-Hasselbalch equation and solve for x. X mmol sodium propionate; Y mmol propionic acid (Report 1 decimal place) Answer setup:  X; Y

Calculate pPb2+ when 25.00 mL of 0.100 M is titrated with 21.00 mL of 0.100 M Pb2+. Ksp = 7.4 × 10−14 for PbCO3.

Calculate the pH of a 0.200 M H2A− solution. K1 = 1.00 × 10−4, K2 = 1.00 × 10−8 and K3 = 1.00 × 10−12.

A buffer is prepared by mixing 200.0 mL of 0.150 0 M NaOH with 200.0 mL of 0.200 0 M CH3CO2H (Ka = 1.75 × 10−5) in a 1-L volumetric flask, and then diluting to volume with deionized water. Calculate the pH of the buffer.

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.