Chemistry - Ch 17

Question 0

Buffered solutions (buffers)

Answer 0

solutions which contain a weak conjugate acid-base pair can resist drastic changes in pH upon the addition of small amounts of strong acid or strong base

Question 1

Common-Ion Effect

Answer 1

observation that whenever a weak electrolyte and a strong electrolyte contain a common ion, the weak electrolyte ionizes less than it would if it were alone in solution

Question 2

Henderson-Hasselbalch Equation

Answer 2

pH = pKa + log [base/acid]

Question 3

Buffer capacity

Answer 3

amount of acid or base the buffer can neutralize before the pH begins to change to an appreciable degree

Question 4

pH range

Answer 4

range over which a buffer acts effectively

Question 5

pH Titration Curve

Answer 5

a graph of the pH as a function of the volume of the added titrant

Question 6

Solubility-product constant (solubility product)

Answer 6

Ksp; equilibrium constant describing how soluble the solid is in water

Question 7

Complex ion

Answer 7

an assembly of a metal ion and the Lewis bases bonded to it

Question 8

Formation constant

Answer 8

Kf; for a metal ion complex, the equilibrium constant for formation of the complex from the metal ion and base species present in solution; it is a measure of the tendency of the complex to form

Question 9

Amphoteric oxides and hydroxides

Answer 9

substances capable of behaving as either an acid or base

Question 10

Qualitative analysis

Answer 10

determines only the presence of absence of a particular metal ion

Question 11

Quantitative analysis

Answer 11

determines how much of a given substance is present