Chapter 15 - The Nature of Acids and Bases

Question 1

anions tend to form either neutral or (basic/acidic) solutions

Answer 1

basic

Question 2

cations tend to form either neutral or (basic/acidic) solutions

Answer 2

acidic

Question 3

an anion that is the conjugate base of a weak acid is itself a (weak/strong) base

Answer 3

weak

Question 4

an anion that is the conjugate base of a strong acids is itself pH-_________

Answer 4

neutral

Question 5

small, highly charged metal cations such as Al3+ and Fe3+ form weakly (acidic/basic) solutions

Answer 5

acidic

-the smaller and more highly charged the cation, the more acidic its behavior

Question 6

When an H atom is bonded to another atom, the charge on the H must be (positive/negative) in order for the solution of the compound to be acidic

Answer 6

positive

b/c acids release H+ ions

Question 7

the stronger the bond, the (weaker/stronger) the acid

Answer 7

weaker

-because the acid wont dissolve entirely when it is held by stronger bonds

Question 8

the more oxygen atoms bonded to Y (any element), the more (acidic/basic) the compound gets

Answer 8

acidic

-O draws electron density away from Y, further weakening and polarizing it, leading to increasing acidity

Question 9

electron pair acceptor

Answer 9

lewis acid

Question 10

electron pair donor

Answer 10

lewis base

Question 11

Stuff to know:

Answer 11

• we can determine the [H3O+] of a polyprotic acid by considering on the first ionization step
• acid strength decreases with increasing bond energy
• acid strength increases with increasing bond polarity