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Biological Chemistry > Acid-base reactions > Flashcards

Acid-base reactions Flashcards

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1
Q

What is a bronsted - lowry acid

A

a proton donor e.g., NH4+, HCl, CH3COOH

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2
Q

What is a bronsted-lowry base

A

proton acceptor e.g., NH3, OH-, CH3COO-

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3
Q

What is the mass action law

A

the rate of any chemical reaction is proportional to the product of the masses of the reacting substances, with each mass raised to a power equal to the coefficient that occurs in the chemical equation

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4
Q

How to use mass action law to calculate k

A

k = [A][B]/[C][D]

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5
Q

Solubility reaction example

A

HgS(s) <-> Hg2+(aq) + S2- (aq)

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6
Q

Acid-base reaction example

A

CH3COOH +H2O <-> H3O+ + CH3COO-

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7
Q

Redox reaction example

A

Zn <-> Zn2+ + 2e-

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8
Q

Partitioning reaction example

A

FeCl3(aq) <-> FeCl3 (org)

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9
Q

What is the LeChatelier principle

A

when a change is imposed in equilibrium, equilibrium will shift to oppose the change

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10
Q

What are conjugate acid-base pairs

A

transfer of a proton between 2 species changes if the compound is an acid or a base e.g. NH4+ and NH3

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11
Q

What is the ionic product of water

A

[H+][OH-} 1x10^-14

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12
Q

What does a strong acid usually react with

A

a weak base

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13
Q

Kw formula

A

Ka x Kb

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14
Q

pKw formula

A

pKa + pKb = 14

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15
Q

strong base pH formula

A

pH = 14 - pOH = 14 + log c0

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16
Q

pH formula of a weak conjugate acid

A

pH = 1/2(14-pKb)-1/2(lo(c0))

17
Q

What is the ion product of water

A

[H3O+][OH-] = 10^-14

18
Q

pOH calculations for a weak base

A

1/2pKb - 1/2logc0

19
Q

How to calculate reaction involving a strong acid/base

A

there is no effect the pH = 7

20
Q

How to calculate the pH of a reaction involving strong acid/weak base

A

pH = 7-1/2pKb - 1/2 log(c0)

21
Q

How to calculate the pH of a reaction involving a weak acid/strong base

A

pH = 7 + 1/2pKa + 1/2 log(c0)

22
Q

Ampholyte pH calculation

A

(pKa1+ pKa2)/2

23
Q

What are the different types of ampholytes

A

salts of weak acid and weak bases, hydrogen salts or di/triprotic acids, compounds with acid and base functional group

24
Q

What are buffers

A

solution of a weak acid or base and its conjugate acid/base

25
Q

pH of buffers formula

A

pH = pKa + log([salt]/[acid])

26
Q

[H3O+] formula

A

[H3O+] = Ka ([acid]/[salt])

27
Q

How to calculate pKa from a buffer curve

A

When half added the base is added, the pH at that volume is equal to pKa

28
Q

What is the end point in a titration

A

the point where the indicator changes colour (verticle section)

29
Q

excess base on a buffer curve

A

pH = 14 - pOH = 14 - log[B]

30
Q

pH at end point formula

A

7 + 1/2pKa = 1/2 log[A-]0

31
Q

pH at the turning point formula

A

(pKa1+pKa2)/2

Biological Chemistry (12 decks)

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