Chapter 17 - Additional Aspects of Aqueous Equilibria Flashcards
What is the common-ion effect? (Lengthy)
The extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.
What is a buffer?
A buffer is an aqueous solution that has a highly stable pH.
How can you change the pH of a buffer?
You can’t really do that, as adding bases/acids/water won’t change the pH (or change it very little).
What is buffer capacity?
It is the quantitative measure of how much a buffer will resist changes to pH from strong acids or bases.
What is the Henderson-Hasselbalch equation?
What is a pH titration curve?
A graphic representation of how one substance is titrated into a solution and the effect it has on pH.
What is the solubility-product constant? (Ksp)
The equilibrium constant that expresses quantitatively the extent to which the compound dissolves.
How is solubility affected by the common-ion effect?
The solubility of a slightly soluble ionic compound is decreased by the presence of a second solute that has a common ion.
Example: If you dump salt (NaCl) into a glass of saltwater, not much of it will dissolve.
What is a complex ion?
A complex ion has a metal ion at its center with a number of other molecules or ions surrounding it.
How do you get an amphoteric oxide or hyrdoxide to dissolve more in water?
On their own, amphoteric oxides and hydroxides are only slightly soluble, but when an acid or base is added to the solution, they dissolve significantly more.
Regarding Q (reaction quotient) and Ksp, when will a precipitate form?
Precipitates form when Q > Ksp.
