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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.
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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 CACB • NH3 + H2O --> NH4+ + OH- • Base Acid CA CB
Lewis Acid/Base • Acid: Electron Acceptor • Base: Electron Donor
Lewis Acid/Base • H3N: + 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
Amphoterism • Can act like an acid or a base • Can donate or accept protons
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
Name & give the formula for at least 4 each of strong acids & strong bases
Binary Acids • Acids containing only 2 elements • HCl Hydrochloric acid • H2S Hydrosulfuric acid
Ternary Acids • Acids containing 3 elements • H2SO4 Sulfuric acid • H2SO3 Sulfurous acid • HNO3 Nitric acid
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. • LiOH Lithium 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)
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 • MAVA = MBVB for monoprotics
Standard Solution • A solution with known concentration
Titration • When titrating acids against bases, the end point of the titration is at the equivalence point
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
Equivalence Point • The point where the H+ concentration is equal to the OH- concentration
Indicator • An organic dye that changes color when the pH changes
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 Formula • NAVA = NBVB • Elliott’s Rule: • #HMAVA = #OHMBVB
Make Calculations • Calculate the molarity of 30.0 mL H2CO3 when it’s titatrated 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 titatrated 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:1) [H+] = 0.040 M2) [HCl] = 0.0025 M3) [HBr] = 0.080 M
Calculate the pOH of: 1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-5 M
Titration Curve:Strong acid vs strong base; then weak acid vs strong base