Exam 17: Additional Aspects of Aqueous Equilibria

A 25.0-mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The K_a of hydrazoic acid is 1.9 × 10^-5.

Which of the following could be added to a solution of acetic acid to prepare a buffer?

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

In which aqueous system is Pbl₂ least soluble?

The molar solubility of __________ is not affected by the pH of the solution.

The Henderson-Hasselbalch equation is __________.

Which one of the following pairs cannot be mixed together to form a buffer solution?

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of __________.

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the __________ present in the buffer solution. The K_a of hydrazoic acid is 1.9 × 10^-5.

In general, the solubility of a slightly soluble salt is __________ by the presence of a second solute that furnishes a common ion.

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about __________ mol/L.