1A + 1B 1C + 1D Calculate the equilibrium concentrations of each species when 150 ml 2.0 M A is mixed with ml 2.0 M B. K c = 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 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
Drill: List 3 properties each of both acids & bases
Common Names ·H + Hydrogen ion ·H 3 O + Hydronium ion ·H - Hydride ion ·OH - Hydroxide ion ·NH 3 Ammonia ·NH 4 + Ammonium ion
Define acids & bases by each of the three methods
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
Strong Acid/Base Ionizes 100 % (1 M) HAH + + A - 1 M – all1 1
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)
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 M NaOH
Make Calculations ·Calculate the mL of 12.5 M HCl required to make 2.5 L of M HCl
Drill: ·Calculate the mL of 16.0 M HNO 3 it takes to make 4.0 L of M HNO 3
Molarity ·Moles of solute per liter of solution (M)
Make Calculations ·Calculate the molarity of 30.0 mL H 2 CO 3 when it’s titrated 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 titrated 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 each of the following: 1) [HCl] = M 2) [H + ] = M 3) [HBr] = M
Calculate the pOH of each of the following: 1) [OH - ] = M 2) [KOH] = M 3) [NaOH] = 4.0 x M
Drill: Calculate the molarity of mL of H 3 PO 4 that was titrated to its equivalence point with mL of M Ba(OH) 2.