In addition to redox indicators and the starch-iodine complex, the equivalence point for a redox titration can be determined using a Gran plot. Which statement is NOT true for a Gran plot?

Which is NOT a property of buffers?

A 50.00-mL aliquot of 0.100 M HNO3 is titrated with 0.075 0 M NaOH. Calculate the pH after 40.00 mL of 0.075 0 M NaOH has been added.

A 100.0-mL sample of a solution containing copper(II) (FM 63.546) is treated with excess sodium carbonate (FM 105.988 8) to precipitate 3.605 5 g of copper(II) carbonate (FM 123.55). What is the molarity of the solution?

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