Acids, Bases And PH

Question 1

What is the equation for pH of strong acids?

Answer 1

PH = -Log [H+]

Question 2

How to calculate [H+] of strong acids?

Answer 2

[H+] = 10 ^pH

Question 3

What is a Bronsted-Lowry base?

Answer 3

A proton acceptor

Question 4

What is a Bronsted-Lowry acid?

Answer 4

A proton donor

Question 5

What is the Arrhenius model of an acid?

Answer 5

Dissociate and release H+ ions in aqueous solutions

Question 6

What is the Arrhenius model of an base?

Answer 6

Dissociate to release OH- ions in aqeuous solutions

Question 7

What is a conjugate acid base pair?

Answer 7

An acid/base pair that can be interconverted by transfer of a proton

Question 8

What is Ka?

Answer 8

Acid dissociation constant

Question 9

What does a Ka equation look like?

Answer 9

Ka = [H+][A-]
[HA]

Question 10

How do you calculate pKa?

Answer 10

PKa = -logKa

Question 11

How do you calculate Ka?

Answer 11

Ka = 10^ -pKa

Question 12

What does pH + pOH = ?

Answer 12

14

Question 13

What is the equation for Kw?

Answer 13

Kw = [H+][OH-]

Question 14

How do we calculate pOH?

Answer 14

POH = -Log [OH -]

Question 15

How to calculate [H+] using kw and [OH-] for strong bases

Answer 15

[H+] = Kw / [OH-]

Question 16

How to calculate [H+] using Ka and [HA] for weak acids

Answer 16

Square root of Ka x [HA] = [H+]

Question 17

What are the limitations of Ka?

Answer 17

1. Ignored dissociation of H2O in very weak acids
2. Value of [HA] does not decrease despite the partial dissociation of weak acids