1A + 1B 1C + 1DCalculate the equilibrium

concentrations of each species when 150 ml 2.0 M A is mixed with 100.0

ml 2.0 M B. Kc = 0.25

Acid/Base

Properties of Acids·Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts

Properties of Bases·Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts

Arrhenius·Acids: release H+ or H3O+ in solution

·Bases: release OH- in solution

Arrhenius·Acid: HA --> H+ + A-

·HCl --> H+ + Cl-

·Base: MOH --> M+ + OH-

·NaOH -->Na+ + OH-

Bronsted-Lowry·Acid: Proton donor

·Base: Proton

Acceptor

Bronsted-Lowry· HA + H2O --> H3O+ + A-

· HI + H2O --> H3O+ + I-

· Acid Base CA CB

· NH3 + H2O --> NH4+ + OH-

· Base Acid CA CB

Lewis Acid/Base·Acid: Electron

Acceptor

·Base: Electron Donor

Lewis Acid/BaseH3N: + BF3 --> H3N-BF3

Base Acid Neutral

Drill:•List 3 properties

each of both acids & bases

Common Names· H+ Hydrogen ion

· H3O+ Hydronium ion

· H- Hydride ion· OH- Hydroxide ion

· NH3 Ammonia

· NH4+ Ammonium ion

Define acids & bases by each of

the three methods

Naming Bases·Almost all bases are metal hydroxides

·Name by normal method

·Ammonia (NH3) as well as many amines are bases

Strong Acids or Bases·Strong acids or bases ionize 100 % in solution

·Weak acids or bases ionize <100 % in solution

Strong Acids· HClO4 Perchloric acid

· H2SO4 Sulfuric acid

· HNO3 Nitric acid

· HCl Hydrochloric acid· HBr Hydrobromic acid· HI Hydroiodic acid

Strong Bases· All column I hydroxides

· Ca(OH)2 Calcium hydroxide

· Sr(OH)2 Strontium hydroxide

· Ba(OH)2 Barium hydroxide

Strong Acid/BaseIonizes 100 % (1 M)

HA H+ + A-

1 M – all 1 1

Monoprotic Acids·Acids containing only one ionizable hydrogen

·HBr Hydrobromic acid

·HCN Hydrocyanic acid

·HC2H3O2 Acetic acid

Diprotic Acids·Acids containing 2 ionizable hydrogens

·H2SO4 Sulfuric acid

·H2SO3 Sulfurous acid

·H2CO3 Carbonic acid

Triprotic Acids·Acids containing 3 ionizable hydrogens

·H3PO4 Phosphoric acid

·H3PO3 Phosphorus acid

·H3AsO4 Arsenic acid

Polyprotic Acids· Acids containing more than one ionizable hydrogens

·H2SO4 Sulfuric acid

·H4SiO4 Silicic acid

·H2CO2 Carbonous acid

Monohydroxic Base·A base containing only one ionizable hydroxide

·NaOH Sodium hydroxide·KOH Potassium hydro.·LiOHLithium hydroxide

Neutralization Rxn· A reaction between an acid

& a base making salt & H2O

·HA(aq) + MOH(aq)

MA(aq) + H2O(l)

Neutralization Rxn

HCl(aq) + NaOH(aq)

NaCl(aq) + H2O(l)

Titration·When titrating acids against bases, the end point of the titration is at the equivalence point

Equivalence Point

·The point where the H+ concentration is equal

to the OH- concentration

Equivalence Point• [ H+] = [OH-]

•Molarity (M)acid

=Molarity(M)base

Titration No changes will be observed when titrating acids against bases; thus, one must use an indicator to see changes

Indicator·An organic dye that changes color when the pH changes

Make Calculations·Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH

Make Calculations·Calculate the mL of 12.5 M HCl required

to make 2.5 L of 0.200 M HCl

Drill: ·Calculate the mL of 16.0 M HNO3 it takes

to make 4.0 L of 0.100 M HNO3

Molarity

·Moles of solute per liter of solution

(M)

Make Calculations·Calculate the molarity of 30.0 mL H2CO3 when it’s titrated to its equivalence point with 75.0 mL 0.200 M NaOH

Make Calculations·Calculate the molarity of 40.0 mL H3PO4 when it’s titrated to its equivalence point with 30.0 mL 0.20 M Ba(OH)2

Calculate the volume of 0.250 M HCl

needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point

Calculate the molarity 25.0 mL H3PO4 that

neutralizes 50.00 mL 0.200 M Ca(OH)2 to its equivalence point

Drill: Calculate the volume of 0.10 M

H3PO4 that neutralizes 50.00 mL 0.200 M

Ca(OH)2 to its equivalence point

pH·The negative log of the hydrogen or hydronium ion concentration

·pH = -log[H+]

·pOH = -log[OH-]

Calculate the pH of each of the following:1) [HCl] = 0.0025 M 2) [H+] = 0.040 M3) [HBr] = 0.080 M

Calculate the pOH of each of the following:

1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-12 M

Drill: Calculate the molarity of 25.00 mL of H3PO4 that was titrated to its equivalence point

with 75.00 mL of0.125 M Ba(OH)2.