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General Chemistry II
Test 1
17
Chemistry
Undergraduate 1
02/09/2009

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Term
Strong Acids
Definition

HI

HClO4 (Perchloric)

 HBr

HCl

H2SO4 (Sulfuric)

HClO3 (Chloric)

HNO3 (Nitric)

 

Term
Definition of a Strong Acid
Definition
  • A substance that reacts essentially, completely with water to produce H3O+.
  • The proton donating power of HA is greater than that of H3O+.
Term
Definition of a Weak Acid
Definition
  • A substance that is only partially deprotnated in water.
  • The proton donating ability of HA is weaker than that of H3O+
Term
Conjugate See-Saw
Definition
The observation that the stronger an acid/base is, the weaker it's conjugate base/acid will be.
Term
Definition of a Strong Base
Definition
  • A substance that reacts essentially completely with water to produce OH- - it is completely protonated in water.
  • The proton accepting power of A- is greater than that of OH-.
Term
Lewis Acid-Base Definition
Definition
  • Acid - Any species capable of donating an electron pair.
  • Base - Any species capable of donating a pair of electrons.
Term
Bronsted-Lowry Acid-Base Definition
Definition
  • Acid - A proton donator.
  • Base - A proton acceptor.

  • Can be viewed as a special case of Lewis definiton
Term
Arrhenius Acid-Base Definition
Definition
  • Acid - A compund that produces H3O+ (hydronium) when dissolved in water.
  • Base - A compound that produces OH- (hydroxide) in aqueous solution.
Term
Definition of a Weak Base
Definition
  • A substance that is only partially deprotonated in water.
  • The proton accepting power of A- is less than that of OH-.
Term
Levelling
Definition
  • H3O+ is the strongest acid that can exist in water and OH- is the strongest base that can exist in water.
  • An acid/base is strong if it is stronger than the conjugate acid/base of the solvent.
Term
Definition of a Buffer
Definition
  • A buffer solution is any solution that maintains an approximately constant pH despite small additions of acid/base or dilution
  • Typically, a buffer contains a weak acid and conjugate weak base in approximately equal concentrations
Term
Henderson-Hasselbeck Equation
Definition
  • pH = pKa - log10([HA]o/[A-]o)
  • pOH = pKb - log10([A-]o/[HA]o)
  • HA and A- represent conjugate acids and bases
  • Equation may be applied towards buffers and the early stages of titrations
Term
Definition of an Indicator
Definition
  • Typically, a weak acid that has sharply different colors in its associated and dissociated states.
  • When pH (of entire soln) = Kin, the concentrations of both states will be equal (both colors)
  • When pH>Kin, [In-]>[HIn]
  • When pH<Kin, [In-]<[HIn]
Term
Equivalence Point
Definition
  • Point in a titration when the acid/base has been completely neutralized by the base/acid.
  • CAVA=CBVB
Term
Endpoint
Definition
The point in a titration at which the color of the indicator changes.
Term
Half-Equivalence Point
Definition
  • The point in a titration at which exactly half the acid/base has been neutralized by the base/acid.
  • pH = pKa
  • pOH = pKb
Term
Amphiprotic pH
Definition
  • The pH of an amphiprotic salt solution is equal to the average of the pKa's of the salt and its conjugate acid.
  • pH = 1/2(pKa1+pKa2)

 

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