acid-base equilibria

Question 1

What is degree of ionization?

Answer 1

quantity that dissociates/concentration before ionization

Question 2

What is the relationship between Kw, Ka and Kb

Answer 2

Kw = Ka*Kb

Question 3

What is a polyprotic acid?

Answer 3

An acid that can donate multiple protons

Question 4

How does Ka change from 1st ionization to 2nd ionization?

Answer 4

Ka decreases

Question 5

Under what conditions do only the first ionization affect pH?

Answer 5

When Ka differs 3 orders between ionizations

Question 6

If the cation/anion of a salt is conjugate of a strong acid/base, what does that mean?

Answer 6

The cation/anion is neutral

Question 7

If the cation of a salt is not conjugate of a strong acid/base, what does that mean?

Answer 7

The cation is acidic

Question 8

If the anion of a salt is not conjugate of a strong acid/base, what does that mean?

Answer 8

If it has no ionizable H, it is basic. If it has an ionizable H, it is amphiprotic

Question 9

What happens if the cation of a salt is acidic and the anion is basic?

Answer 9

The acidity is determined by which K is higher

Question 10

What happens if the cation in a salt is acidic and the anion is neutral?

Answer 10

The salt will be acidic

Question 11

What is the common ion effect?

Answer 11

When the equilibrium of an acid-base reaction is shifted by the addition of a salt with a common ion

Question 12

What is a buffer and what is its purpose?

Answer 12

A solution containing an acid and its conjugate, to resist pH

Question 13

What is the equation used to find the pH of buffers?

Answer 13

pH = pKa + log(HA/A)

Question 14

What is a titrant and an analyte?

Answer 14

Analyte: solution of unknown concentration
Titrant: reactant added to analyte via buret

Question 15

What is the equivalence point?

Answer 15

The point in a titration where titrant and analyte are present in stoichiometrically equal amounts

Question 16

How do you find the pH in a titration reaction?

Answer 16

set up ICF table w/ initial moles, determine limiting reagant that will go to 0, determine x from limiting reagant. if the remaining reactant is strong, then [H] or [OH] will equal concentration of the acid. If the remaining acid is weak, must use Ka to find [H] or [OH]