acids and bases

Question 1

What is the arrhenius acid/base definition?

Answer 1

Acid: increases H+ concentration in water
Base: increases OH- concentration in water

Question 2

What is the lewis acid/base definition?

Answer 2

Acid = e- acceptor
Base = e- donor

Question 3

What is the Bronsted-Lowry acid/base definition?

Answer 3

Acid = H+ donor
Base = H+ acceptor

Question 4

What are conjugate acid/base pairs?

Answer 4

Acid/base pair that only differ by the presence of one H+ ion

Question 5

How is acid/base strength measured?

Answer 5

Ka / Kb

Question 6

What is the relationship bewteen Ka and Kb?

Answer 6

Ka = 1/Kb

Question 7

What is the relationship between conjugate acid strength and base strength

Answer 7

Stronger the acid/base, weaker the conjugate

Question 8

For acid HX, how does size of X affect acid strength

Answer 8

The larger the X, the stronger the acid

Question 9

For acid HX, how does electronegativity affect acid strength

Answer 9

The more electronegative X is, the weaker the acid

Question 10

For acid HXY, how does amount of Y affect acid strength?

Answer 10

the more Y bonded, the stronger acid

Question 11

What is the autoionization of water?

Answer 11

When water reacts with itself to form OH- and H+

Question 12

What is the acid dissociation constant for the autoionization of water at 25 degrees celsius ?

Answer 12

10^-14

Question 13

How do you calculate pH and pOH?

Answer 13

-log[H+], -log[OH-]

Question 14

What is the relationship between Kw, [H+] and [OH-]

Answer 14

Kw = [H+][OH-]

Question 15

How do you calculate pK?

Answer 15

-logK

Question 16

What is the relationship between pKw, pH and pOH

Answer 16

pKw = pH + pOH

Question 17

What is the relationship between pKa and acid strength?

Answer 17

The lower pKa, the stronger the acid

Question 18

What are the strong acids?

Answer 18

HCl, HI, HBr, HNO3, H2SO4, HClO4

Question 19

What are the strong bases?

Answer 19

LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2