Bell Ringer Have out lab from Monday. Join Kahoot at kahoot.it with PIN: 332825 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.”

Crash Course #8 Acid & Base Reactions https://www.youtube.com/watch?v=ANi709MYnWg Take notes about the acid/base definitions on your WS We will fill in “Lewis Acid/Base” together

Die Spongebob, Die! https://www.youtube.com/watch?v=PQ6IsCbNZAQ

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

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)

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.

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

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

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

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!

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+).

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

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

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

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

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

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

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+).

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+.

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.

HCl + NH3  NH4+ + 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

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

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.

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.