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Chemistry Kaplan MCAT > Ch. 10: Acids and Bases > Flashcards

Ch. 10: Acids and Bases Flashcards

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1
Q

Arrhenius Acids

A

Dissociate to produce an excess of hydrogen ions in soln

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2
Q

Arrhenius Bases

A

Dissociate to produce and excess of hydroxide ions in solution

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3
Q

Bronsted-Lowry Acids

A

Species that can donate hydrogen ions

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4
Q

Bronsted-Lowry Bases

A

Species that can accept hydrogen ions

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5
Q

Lewis Acids

A

Electron-pair acceptors

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6
Q

Lewis Bases

A

Electron-pair donors

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7
Q

Statements

A

All Arrhenius acids and bases are Bronsted-Lowry acids and bases, and all bronsted-lowry acids and bases are lewis acids ands and bases; however, the converse of these statements is not necesarily true

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8
Q

Amphoteric

A

Species which can behave as acids or bases

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9
Q

Amphiprotic

A

Species which can specifically behave as Bronsted lowry acids or bases

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10
Q

Water

A

Classic example of an amphoteric, amphiprotic species– it can accept a hydrogen ion to become a hydronium ion, or it can donate a hydrogen ion to become a hydroxide ion

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11
Q

Conjugate Species of Polyvalent acids and bases

A

Can also behave as amphoteric and amphiprotic species

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12
Q

Water Dissociation constant Kw

A

10^-14 at 298K. Like other equilibrium constants, Kw is only affected by changes in temp

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13
Q

pH and pOH

A

Can be calculated given the concentrations of H3O+ and OH- ions, respectively. In aqueous solns, pH+pOH=14 at 298K

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14
Q

Strong acids and bases

A

Completely dissociate in solution

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15
Q

Weak acids and bases

A

Do not completely dissociate in solution and have corresponding dissociation complexes (Ka and Kb)

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16
Q

Conjugate Acids and Bases

A

In the Bronsted-Lowry def, acids have conjugate bases that are formed when the acid is deprotonated. Bases have conjugate acids that are formed when the base is protonated

  • Strong acids and bases have very weak (inert) conjugates
  • Weak acids and bases have weak conjugates
17
Q

Neutralization reactions

A

From salts and (sometimes) water

18
Q

Equivalent

A

Defined as one mole of the species of interest

19
Q

Normality

A

In acid-base chemistry, normality is the concentration of acid or base equivalents in solution

20
Q

Polyvalent

A

Acids and bases that can donate or accept multiple electrons. The normality of a solution containing a polyvalent species is the molarity of the acid or base times the number of protons it can donate or accept.

21
Q

Titrations

A

Used to determine the concentration of a known reactant in a soln

22
Q

Titrant

A

Has a known concentration and is added slowly to the titrand to reach the equivalence point

23
Q

Titrand

A

Has an unknown concentration but a known volume

24
Q

Half-equivalence point

A

Midpoint of the buffering region, in which half of the titrant has been protonated (or deprotonated); thus, [HA] = [A-] and a buffer is formed

25
Q

Equivalence Point

A

Indicated by the steepest slope in a titration curve; it is reached when the number of acid eqivalents in the original soln equals the number of base equivalents added or vice versa

26
Q

pH values of acids and bases

A
  • Strong acid and strong base titrations have equivalence points at pH = 7
  • Weak acid and strong base titrations have equivalencce points at pH > 7
  • Weak base and strong acid titrations have equivalencce points at pH < 7
  • Weak acid and weak base titrations can have equivalence points above or below 7 depending on the relative strength of the acid and base
27
Q

Indicator

A

Chosen for a titration, should have a pKa close to the pH of the expected equivalence point

28
Q

Endpoint

A

When the indicator reaches its final color in a titration

29
Q

Polyvalent acid/base titrations

A

Multiple buffering regions and equivalence points are observed

30
Q

Buffer solutions

A

Consist of a mixture of a weak acid and its conjugate salt or a weak base its conjugate salt; they resist large fluctuations in pH

31
Q

Buffering capacity

A

Refers to the ability of a buffer to resist changes in pH; Maximal buffering capacity is seen within 1 pH point of the pKa of the acid in the buffer soln

32
Q

Henderson-Hasselbalch Equation

A

Quantifies the relationship between pH and pKa for weak acids and between pOh and pKb for weak bases; when a soln is optimally buffered, pH = pKa and pOH = pKb

Chemistry Kaplan MCAT (12 decks)

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