1A + 2B 1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. K c = 2.0 x 10 -10.

1A + 2B 1C + 1DCalculate the equilibrium

concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. Kc = 2.0 x 10-10

Drill:1A + 2B 1C + 1D

Calculate the equilibrium concentrations of each

species when a solution is made with 1.0 M A &

1.0 M B. Kc = 2.0 x 10-12

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

Common Names· H+ Hydrogen ion

· H3O+ Hydronium ion

· H- Hydride ion

· OH- Hydroxide ion

· NH3 Ammonia

· NH4+ Ammonium ion

Amphiprotism·Can act like an acid or a base

·Can donate or accept protons

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

·Weak acids or bases ionize <100 % in solution

Drill: Name each of the following:

KOH HBrAl(OH)3 H2CO3

HClO4 NH3

Naming Acids· All acids are H-anion

· If the anion is:

· -ides hydro___ic acids

· -ates ___ic acids

· -ites ___ous acids

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

Binary Acids·Acids containing only 2 elements

·HCl Hydrochloric acid

·H2S Hydrosulfuric acid

Ternary Acids· Acids containing 3 elements

·H2SO4 Sulfuric acid

·HNO3 Nitric acid

Monoprotic Acids·Acids containing only one ionizable hydrogen

·HBr Hydrobromic acid

·HC2H3O2 Acetic acid

Diprotic Acids·Acids containing 2 ionizable hydrogens

·H2SO4 Sulfuric acid

·H2CO3 Carbonic acid

Triprotic Acids·Acids containing 3 ionizable hydrogens

·H3PO4 Phosphoric acid

·H3AsO4 Arsenic acid

Polyprotic Acids· Acids containing more than

one ionizable hydrogens

·H4SiO4 Silicic acid

·H2CO2 Carbonous acid

Monohydroxic Base

·A base containing only one ionizable hydroxide

·NaOH Sodium hydroxide

·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)

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) [H+] = 0.040 M2) [HCl] = 0.0025 M 3) [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 10-7 M

Standard Solution

·A solution with known

concentration

Drill: Identify: acid, base, CA, & CB HCO3

- + H2O

H2CO3 + OH-

Titration·A method of determining the concentration of one solution by reacting it with a standard solution

Titration Formula for monoprotic solutions

MAVA = MBVB

Titration FactWhen titrating acids

against bases, the end

point of the titration is

at the equivalence point

Equivalence Point

·The point where the concentrations of the two solutions in the titration are equal

Acid/Base Equivalence PointThe point where the H+

concentration is equal to

the OH- concentration

Titration Fact 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

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

Titration Formula for monoprotic solutions

MAVA = MBVB

Dilution Formula

M1V1 = M2V2

·Calculate the mL of 16.0 M HNO3 it takes to make 4.0 L of 0.100 M HNO3

Make Calculations·Calculate the mL of 12.5 M HCl required

to make 2.5 L of 0.200 M HCl

Molarity

·Moles of solute per liter of solution

(M)

Normality·Number of moles of hydrogen or hydroxide ions per liter of solution (N)

Titration Formulafor Acid/Base

·NAVA = NBVB

·Elliott’s Rule:

·#HMAVA = #OHMBVB

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

Titration Curve:Strong acid vs

strong base

Titration Curve:Strong acid vs

strong base; then weak acid vs strong base

Titration Curve:Strong base vs

strong acid; then weak base vs strong acid

3.2 g HI is dissolved in a

1250 mL aqueous solution.

Calculate its pH.

Calculate the volume of 0.10 M H3PO4 that

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

equivalence point

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.