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 H 3 O + 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 + H 2 O --> H 3 O + + A - ·HI + H 2 O --> H 3 O + + I - ·Acid Base CA CB ·NH 3 + H 2 O --> NH OH - ·Base Acid CA CB
Lewis Acid/Base ·Acid: Electron Acceptor ·Base: Electron Donor
Lewis Acid/Base ·H 3 N: + BF 3 --> H 3 N-BF 3 ·Base Acid Neutral
Common Names ·H + Hydrogen ion ·H 3 O + Hydronium ion ·H - Hydride ion ·OH - Hydroxide ion ·NH 3 Ammonia ·NH 4 + Ammonium ion
Amphoterism ·Can act like an acid or a base ·Can donate or accept protons
Define acids & bases by each of the three methods
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 (NH 3 ) 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 ·HClO 4 Perchloric acid ·H 2 SO 4 Sulfuric acid ·HNO 3 Nitric acid ·HClHydrochloric acid ·HBrHydrobromic acid ·HIHydroiodic 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 ·HClHydrochloric acid ·H 2 SHydrosulfuric acid
Ternary Acids ·Acids containing 3 elements ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·HNO 3 Nitric acid
Monoprotic Acids ·Acids containing only one ionizable hydrogen ·HBr Hydrobromic acid ·HCNHydrocyanic acid ·HC 2 H 3 O 2 Acetic acid
Diprotic Acids ·Acids containing 2 ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·H 2 CO 3 Carbonic acid
Triprotic Acids ·Acids containing 3 ionizable hydrogens ·H 3 PO 4 Phosphoric acid ·H 3 PO 3 Phosphorus acid ·H 3 AsO 4 Arsenic acid
Polyprotic Acids ·Acids containing more than one ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 4 SiO 4 Silicic acid ·H 2 CO 2 Carbonous acid
Monohydroxic Base ·A base containing only one ionizable hydroxide ·NaOHSodium hydroxide ·KOHPotassium hydro. ·LiOHLithium hydroxide
Neutralization Rxn ·A reaction between an acid & a base making salt & H 2 O ·HA (aq) + MOH (aq) MA (aq) + H 2 O (l)
Neutralization Rxn HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l)
Drill: Identify: acid, base, CA, & CB HCO H 2 O H 2 CO 3 + OH -
Work problems 1 – 6 on page 395
Titration ·A method of determining the concentration of one solution by reacting it with a standard solution ·M A V A = M B V B 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 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 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 ·N A V A = N B V B ·Elliott’s Rule: ·# H M A V A = # OH M B V B
Make Calculations ·Calculate the molarity of 30.0 mL H 2 CO 3 when it’s titatrated to its equivalence point with 75.0 mL M NaOH
Make Calculations ·Calculate the molarity of 40.0 mL H 3 PO 4 when it’s titatrated to its equivalence point with 30.0 mL 0.20 M Ba(OH) 2
Calculate the volume of M HCl needed to titrate mL M NaOH to its equivalence point
Calculate the molarity 25.0 mL H 3 PO 4 that neutralizes mL M Ca(OH) 2 to its equivalence point
Drill: Calculate the volume of 0.10 M H 3 PO 4 that neutralizes mL 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 + ] = M 2) [HCl] = M 3) [HBr] = M
Calculate the pOH of: 1) [OH - ] = M 2) [KOH] = M 3) [NaOH] = 4.0 x M
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