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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
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
Bronsted-Lowry· HA + H2O H3O+ + A-
· HI + H2O H3O+ + I-
· Acid Base CA CB
· NH3 + H2O NH4+ + OH-
· Base Acid CA CB
Common Names· H+ Hydrogen ion
· H3O+ Hydronium ion
· H- Hydride ion
· OH- Hydroxide ion
· NH3 Ammonia
· NH4+ Ammonium ion
Strong Acids or Bases·Strong acids or bases ionize 100 % in solution
·Weak acids or bases ionize <100 % in solution
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
Monoprotic Acids·Acids containing only one ionizable hydrogen
·HBr Hydrobromic acid
·HC2H3O2 Acetic 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)
Calculate the pOH of each of the following:
1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-7 M
Titration·A method of determining the concentration of one solution by reacting it with a standard solution
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
Titration Fact No changes will be observed when titrating acids against bases; thus, one must use an indicator to see 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
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
Calculate the volume of 0.10 M H3PO4 that
neutralizes 50.00 mL 0.200 M Ca(OH)2 to its
equivalence point