1. Bell Ringer
Have out lab from Monday. Join Kahoot at kahoot.it with PIN: You have until 1 minute after the bell. This will be part of your lab grade. If you do not have access, get out a sheet of paper. While you’re waiting - “Son,” the father says, examining the broken petri dishes littered about the floor, “I’m not a mad scientists, I’m just a disappointed scientist.”

2. Crash Course #8 Acid & Base Reactions
Take notes about the acid/base definitions on your WS
We will fill in “Lewis Acid/Base” together

3. Die Spongebob, Die!

4. Acids and Bases Bronsted - Lowry Arrhenius Lewis pH
Acids produce hydrogen ions (H+) when dissociated in aqueous solution
Bases form hydroxide ions (OH-) when dissociated in water
Acids are proton (H+) donors
Bases are proton acceptors
Acids accept a pair of electrons
Bases donate a pair of electrons
Strengths of acids & bases
pH = -log [H+] pH

5. Arrhenius Definition acid: generates [H+] in solution
[H+] known as a hydrogen ion
can also be depicted as a hydronium ion [H3O+]
HA(aq) → H+(aq) + A-(aq)
base: generates [OH-] in solution
[OH-] known as a hydroxide ion
BOH(aq) → B+(aq) + OH-(aq)

6. Arrhenius Definition Acids produce hydrogen ions in aqueous solution.
Bases produce hydroxide ions when dissolved in water.
Limits to aqueous solutions.
Only one kind of base.
NH3 ammonia could not be an Arrhenius base.

7. Lewis Acids and Bases :N F H B F H F H Most general definition.
Acids are electron pair acceptors.
Bases are electron pair donors. F H B F :N H F H

8. Lewis Acids and Bases :N F H B F H F H
Boron triflouride wants more electrons. F H B F :N H F H

9. Lewis Acids and Bases F H F B N H F H
Boron triflouride wants more electrons.
BF3 is Lewis acid NH3 is a Lewis base. F H F B N H F H

10. Bronsted-Lowry Definition
Acid - any substance that donates a H+ (proton)
Base-any substance that accepts a H+ (proton).
Conjugate pairs- what is left after a proton is donated or accepted!

11. Acid (must contain at least 1 H+)
Bronsted-Lowry Acids
Acid - any substance that donates a H+ (proton)
Conjugate Base – acid’s anion left after the H+ was donated
Acid (must contain at least 1 H+)
Conjugate Base
HCl
HBr
H2PO4-
HCN
HSO4-
The only difference between an acid and its conjugate base is a proton (H+).

12. Plickers Check – get ready!
Hold up your answer card with the chosen answer choice at the top of the paper
Water acting as an acid

13. Base (must contain at least 1 H+)
Bronsted-Lowry Bases
Base-any substance that accepts a H+ (proton).
Conjugate Acid– base’s anion left after the H+ was accepted
Base (must contain at least 1 H+)
Conjugate Acid
HSO4-
OH-
HC2H3O2
HCO3-
NH3

14. Plickers Check – get ready!
Hold up your answer card with the chosen answer choice at the top of the paper
Water acting as a base

15. The Bronsted-Lowry model:
An acid is a proton donor (H+) and a base is a proton acceptor
HA (aq) + H2O (l)  H3O+ (aq) + A- (aq)
acid base
HCl (aq) H2O (l)  H3O+ (aq) + Cl- (aq)
acid base

16. The Bronsted-Lowry model:
An acid is a proton donor (H+) and a base is a proton acceptor
HA (aq) + H2O (l)  H3O+ (aq) + A- (aq)
acid base
HCl (aq) H2O (l)  H3O+ (aq) + Cl- (aq)
acid base

17. A base is proton acceptor
A- (aq) + H2O (l)  HA (aq) + OH- (aq)
base acid
NH3 (aq) + H2O (l)  NH4+ (aq) + OH- (aq)
base acid

18. Bronsted-Lowry Definition
The acid on one side reacts to become the base on the other side.
HCl + NH3 NH4+ + Cl-
Base 1 (Acceptor)
Acid 2 Donor CA
Base 2 (Acceptor) CB
Acid 1 Donor
Acid 1 (HCl) and Base 2 (Cl-) are
conjugate pairs
Acid 2 (NH4+) and Base 1 (NH3) are also conjugate pairs
The only difference between an acid and its conjugate base is a proton (H+).

19. Conjugate acid-base pairs
When you dissolve an acid in water, the acid donates a proton to a water molecule to form a new acid (conjugate acid) and a new base(conjugate base)
HA (aq) + H2O (l)  H3O+ (aq) + A- (aq)
acid base conjugate conjugate
acid base
The conjugate base is what is left over from the acid when it has lost its proton.
A conjugate acid-base pair, are the two substances related to each other by the loss and gain of protons.
This proton that is released by the acid forms a bond with water to form the hydronium ion, H3O+.

20. Which is the acid and which is the base in these equations?
HCl (aq) + H2O (l)  H3O+ (aq) + Cl- (aq)
NH3 (aq) + H2O (l)  NH4+ (aq) + OH- (aq)
base
Conjugate acid
Conjugate base
acid
Conjugate acid
Conjugate base
acid
base
Water can be an acid or a base. So water is amphoteric.

21. HCl NH3  NH Cl-
Acid Base conjugate conjugate
acid base
Acid / Base pair
Cl- is the conjugate base of the acid HCl
HCl / Cl-
NH4+ is the conjugate acid of the base NH3
NH4+ / NH3

22. Write conjugate base for the following:
a. HClO4
b. H3PO4
c. H2SO4
d. CH3NH3+
Which of the following are acid-base pairs?
a. H2O, H3O+
b. OH- ,HNO3
c. HC2H3O2 , C2H3O2-
d. H2SO4, SO4 2-
ClO4 -
H2PO4 -
HSO4 -
CH3NH2
Yes No

23. Die Spongebob/Acid Rain Reality: Label as True or False
H2SO4 (aq) + H2O(l)  _____ + _____ a)___ H2SO4 is acting as a base b)___ product HSO4- is acting as a conjugate acid c)___ H2O is acting as a base d)___ product H+ (aq) is acting as a conjugate acid e)___ The products of the reaction are in solution.

24. Die Spongebob/Acid Rain Reality: Label as True or False
H2SO4 (aq) + H2O(l)  HSO4- + H3O+ Acid base CB CA a)_F_ H2SO4 is acting as a base b)_F_ product HSO4- is acting as a conjugate acid c)_T_ H2O is acting as a base d)_T_ product H+ (aq) is acting as a conjugate acid e)_T_ The products of the reaction are in solution.