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.

The end point for the Volhard titration is indicated by

Which of the following compounds is NOT an aprotic solvent?

Use this space to provide feedback about the notes packet- was it useful? Was it easy to follow? Etc…

For the graphical equivalence point determination for a precipitation reaction, which statement(s) is/are TRUE? The steepest slope of the titration curve is the equivalence point. The equivalence point occurs where the first derivative of the titration curve reaches its largest value. The equivalence point occurs where the second derivative of the titration curve equals zero.