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CH302: Chemistry > ACID/BASE EQUILIBRIA > Flashcards

ACID/BASE EQUILIBRIA Flashcards

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1
Q

What is an acid?

A

An acid is a proton (H+) donor

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2
Q

What is a base?

A

A base is a proton {H+) acceptor

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3
Q

What is Kw for water at room temperature?

A

Kw - [H+] [OH-] = 10E-14

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4
Q

Strong acids:

A

HCl

HBr

HClO4

HClO3

H2SO4

HNO3

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5
Q

Strong bases:

A

LiOH

NaOH

KOH

RbOH

CsOH
Ca(OH)2

Sr(OH)2

Ba(OH)2

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6
Q

How is K written for strong acids?

A

Very large

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7
Q

How is K writen for weak acids?

A

Ka

The larger the Ka, the stronger the base

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8
Q

How is K written for a weak base?

A

Kb

The larger the Kb the stronger the base

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9
Q

What is the formula for [H+]?

A

[H+] = √Ka(Ca)

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10
Q

What is the formula for [OH-]?

A

[OH-] = √Kb(Cb)

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11
Q

How are Ka and Kb of its conjugate base related?

A

The larger the Ka, the smaller the Kb of its conjugate base

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12
Q

What forms when acids and bases react and are neuralized?

A

Salts

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13
Q

What is a buffer?

A

A buffer is a solution that contains sustantial amounts of a compound in both its protonate and deprotonated forms, which male it resistant to changes in pH

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14
Q

How do you calculate pH of a buffer?

A

pH = pKa + log[A-/HA]

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15
Q

How do you calculate pOH of a buffer?

A

pOH = pKb + log[BH+/B]

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16
Q

What is a titration?

A

A titration is the procedure in which a strong acid or base of acccurate concentration is added stepwise in small amounts to incrementally neutralize the solution

17
Q

What is an analyte?

A

An analyte is the “unknown” solution for which you would like to know either the concentration or K value of

18
Q

What is a titrant?

A

A titrant is the “known” solution which has a percise and accurate concentration

19
Q

What is the equivalence point?

A

The equivalence point is the point at which the number of moles of added base are equal to the number of moles of analyte solution

20
Q

What is the half-equivalence point?

A

The half-equivalence point is the point at which half of the original analyte has been neutralized

21
Q

How do you convert between Ka and Kb?

A

1E-14 = [Ka][Kb]

22
Q

How do you convert Ka to pKa (of Kb to pKb)?

A

pKa = -log[Ka] (or pKb = -log[Kb])

23
Q

What species dominates at the equivalence point?

A

100% A- (conjugate base to strong acid)

24
Q

Explain what is happening at the half-equivalence point?

A

Moles HA = moles A-

25
Q

What is the protonated state?

A

pH < pka

26
Q

What is the deprotonated state?

A

pH > pKa

27
Q

What is needed for an indicator to effectively indicate the endpoint of the titration?

A

pKa needs to be close to the pH of the equivalence point of the titration

CH302: Chemistry (7 decks)

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