Chapter 15 (one five) fifteen - Acid-Base Equilibria

Question 1

rate this chapter

Answer 1

bad

Question 2

Can you ever put “partners” on the same side of an equilibrium reaction equation?

Answer 2

No

Question 3

What things must a buffer have>

Answer 3

1. A weak acid
2. A partner within a factor of 10 of the WA (has to be an ionic salt)

Question 4

What are “partners?”

Answer 4

Partners are the same molecule with a difference in one H+ ion (ex. NH3 weak base and NH4 conjugate acid)

Question 5

What is a buffer?

Answer 5

Substance that resists change in pH

Question 6

What units can you work with in buffer questions?

Answer 6

moles or mmol

Question 7

WHen is the only time the Henderson-Hasselbach Equation applies?

Answer 7

In the case of a buffer (WA or WB + partner, either or and you get nothing)

Question 8

What proportion of partners is the ideal buffer?

Answer 8

1:1

Question 9

What are the units of the H-H equation’s A-/HA?

Answer 9

Moles, put in molarity it just cancels to moles, H-H equation uses proportion

Question 10

What is pH a measure of? How do higher and lower pH sol’ns react?

Question 11

How do you calculate % dissociation?

Question 12

Is OH- a strong or weak base?

Question 13

Is H2O a strong or weak acid?

Question 14

H-H equation for bases

Question 15

Why aren’t spectator ions included?

Question 16

What unit do you need of a substance for a -log pH calculation?

Answer 16

Mol/L

Question 17

Why do weak-base titrations have a lower equivalence than strong-base titrations?

Answer 17

Because as the reactants neutralize each other 100% (strong acid/base reacts with weak acid/base), the remaining salt hydrolyzes and creates either H+ or OH-

Question 18

Define titrate

Answer 18

Add a reagent/titrant until substance being measured is exactly fully reacted