Chapter 18

Question 1

-mainly dealt with single solute in solution
- now deal with 2 solutes
- when you add ion that is in common with already dissolved species, you shift the equilibrium

Answer 1

common ion effect

Question 2

• solution that contains weak acid and its conjugate base
  OR
  -solution that contains weak base and its conjugate acid
• pH of blood must be maintained between 7.38 and 7.42
• resists changes in pH unless you add small amounts of strong acid or strong base
• presents in comparable amounts

Answer 2

Buffer

Question 3

how much acid or base can be absorbed before a buffer can no longer buffer the pH

Answer 3

capacity

Question 4

reaction of acid with base (neutralization)

Answer 4

titration

Question 5

one of known concentration

Answer 5

standard solution

Question 6

point when stochiometrically equivalent amounts of acid and base are present (moles of acid=moles of base)

Answer 6

equivalence point

Question 7

the point in the laboratory when the titration is stopped (often around the equivalence point)
- typically signaled by color change of an indicator

Answer 7

Endpoint

Question 8

the solution that is placed in the burette
- typically one of the known concentration

Answer 8

titrant

Question 9

pH vs. volume titrant (or moles of titrant) added

Answer 9

titration curve

Question 10

• reaction taking place (what is in the beaker) * most important
• moles of acid or base in beaker
• moles of acid or base in added from burette
• total volume

Answer 10

Items to keep track of during a titration