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My GenChem DAT Prep > Acid Base Equilibria and Titrations > Flashcards

Acid Base Equilibria and Titrations Flashcards

1
Q

What are the strong acids

A

HI
HBr
HCl
HClO3
HClO4
H2SO4
HNO3
(So I Brought No Clean Clothes)

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2
Q

What are the strong bases

A

Group 1 metal hydroxides
Mg(OH)2
Ca(OH)2
Sr(OH)2
Ba(OH)2

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3
Q

Creating an acidic buffer

A

Mixing a weak acid and its conjugate base in a 1:1 ratio

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4
Q

Creating an alkaline buffer

A

Mixing a weak base and its conjugate acid in a 1:1 ratio

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5
Q

Lewis acid

A

Species that can accept an electron pair

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6
Q

Lewis base

A

Species that can donate can electron pair

must contain a lone pair of electrons

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7
Q

What are some common Lewis acids?

A

Metal cations: K+, Mg2+, Ca2+, Fe3+
Neutral compounds of boron, aluminum
Other group 13 elements: BF3, AlCl3
Protons (H+)

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8
Q

What makes a good Lewis acid?

A

When the central atom can most readily accept an electron pair

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9
Q

Acid/base and conjugate acid/base relationship:

A

The stronger the acid = the weaker the conjugate base
The weaker the acid = the stronger the conjugate base
The stronger the base = the weaker the conjugate acid
The weaker the base = the stronger the conjugate acid

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10
Q

As pKa/pKb goes down, Ka/kb _______ and acid/base strength ________
As pka/pkb goes up, Ka/kb __________ and acid/base strength _________

A

Increases, increases
Decreases, decreases

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11
Q

Metal oxides produce ________ solutions in water

A

Basic

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12
Q

Non-metal oxides produce ________ solutions in water

A

Acidic

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13
Q

General trend for acidity for oxyacids

A
  • The more oxygen atoms, the more acidic because there are more oxygens for the electrons to spread out onto in the conjugate base
  • for oxyacids with the same number of oxygen atoms, acid strength increases with electronegativity: HClO4 > HBrO4 > HIO4
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14
Q

the ______ is placed in an Erlenmeyer flask during a titration

A

analyte

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15
Q

the _______ is placed in a burrette during a titration

A

titrant

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16
Q

what is the equivalence point in an acid-base titration?

A

the point at which the moles of H+ ions in solution is equal to the moles of OH- ions
usually the steepest part of the titration curve

17
Q

what titrations involve a half-equivalence point?

A

titrations involving weak acid/strong base or a weak base/strong acid

18
Q

what is the half-equivalence point in a titration curve?

A

the midpoint of the buffering region, the part of the curve where the pH of the solution is not drastically affected

19
Q

what is the process of an acid-base titration?

A

the concentration of an analyte is determined by gradually adding small volumes of a solution with a known concentration (the titrant). titrant is added until the reaction completes at a certain equivalence point, which can be viewed by color changes or on a graph

20
Q

at the equivalence point, what formula can be used to determine the concentration of the analyte?

A

NaVa = NbVb (using normality) or MaVa = MbVb (molarity)

21
Q

strong acid + strong base = equivalence point at pH

A

= 7

22
Q

strong acid + weak base = equivalence point at pH

A

< 7

23
Q

weak acid + strong base = equivalence point at pH

A

> 7

24
Q

all monoprotic strong acid and strong base titrations will have an equivalence point at pH ______

A

7

25
Q

arrhenius acid

A

any species that dissolves in aqueous solution to produce H+ ions

arrhenius acids are bronsted-lawry acids –> both release protons

26
Q

arrhenius base

A

any species that dissolves in aqueous solution to produce OH- ions

27
Q

formula for calculating pH:

A

pH = -log[H+]

28
Q

formula for calculating pOH:

A

pOH = -log[OH-]

29
Q

what is the pH of water?

A
  • 7
  • it contains the same number of hydrogen ions and hydroxide ions
  • [H+][OH-] = (1 x 10-7 M)
30
Q

what is the constant kw of water?

A
  • water dissociates to produce H+ and OH-
  • the constant kw = [H+][OH-] = (1 x 10-7 M)2 = 1 x 10-14
31
Q

strength of binary acids:

A
  • binary acids: HCl, HBr, HI
  • HCl > HBr > HI
  • HI is the strongest because it has the largest atomic radius which causes the bond length to become longer and the bond strength to be weaker
32
Q

neutralization reaction:

A
  • when a strong acid reacts with a strong base to form salt and water
  • all protons (H+) and hydroxide ions (OH-) present in the solution combine to form water and the reaction goes to completion
  • the salt produced is neutral
33
Q

reaction that form salts may occur between:

A
  • strong acid and a strong base
  • strong acid and a weak base
  • weak acid and a strong base
34
Q

reaction between a strong acid and a weak base:

A
  • results in an acidic salt
  • the conj. base of the strong acid is considered to be neutral
  • the conj. acid of the weak base is considered to be acidic
  • ex: HCl + NH3 -> NH4Cl
35
Q

reaction between a weak acid and a strong base:

A
  • results in a basic salt
  • the conjugate base of the weak acid is basic
  • the conjugate base of the strong base is neutral
36
Q

what formula is used to calculate the pH of a buffer solution?

A
  • Henderson-Hasselbalch equation:
  • pH = pKa + log([A-]/[HA])
  • [A-] = concentration of conj. base
  • [HA] = concentration of weak acid

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