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Chemistry > Acids, Bases and pH > Flashcards

Acids, Bases and pH Flashcards

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1
Q

What is an alkali

A

a soluble base

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2
Q

What is a bronsted-lowry acid

A

a proton donor

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3
Q

What is a bronsted-lowry base

A

a proton acceptor

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4
Q

What is a conjugate acid base pair

A

contains 2 species that can be interconverted by transfer of a proton

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5
Q

What is a monobasic acid

A

there is 1 hydrogen ion in the acid that can be replaced per molecule in an acid-base reaction

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6
Q

What is a dibasic acid

A

there are 2 hydrogen ions in the acid that can be replaced per molecule in an acid-base reaction

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7
Q

What is a tribasic acid

A

there are 3 hydrogen ions in the acid that can be replaced per molecule in an acid-base reaction

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8
Q

What is pH

A

-log[H+(aq)]

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9
Q

How to work out H+ concentration from pH

A

10^-pH

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10
Q

A change of 1 pH number is equal to how many times difference

A

x10

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11
Q

What is a strong acid

A

completely dissociates in aqueous solution

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12
Q

What is a weak acid

A

partially dissociates in aqueous solution

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13
Q

What is Ka

A

the acid dissociation constant used for acid base equilibria

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14
Q

What is the Ka formula

A

[H+][A-] /[HA]

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15
Q

What can cause Ka to change

A

Temperature

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16
Q

What does a large Ka mean

A

Further equilibrium is to the right. The greater the disassociation/strength of acid

17
Q

How do you convert Ka to pka

A

-log(ka)

18
Q

How do you convert pka to ka

A

10^-pka

19
Q

What is the purpose of pka

A

makes values more manageable than ka and it is much easier to compare relative acid strengths using pka

20
Q

The stronger the acid…

A

larger the ka and the smaller the pka

21
Q

the weaker the acid…

A

the smaller the ka and the larger the pka

22
Q

What does [H+] depend upon

A

concentration of acid and the acid dissociation constant

23
Q

What approximations are made when calculating pH of acids

A
  1. HA dissociates to produce equilibrium concentrations of H+ and A- that are equal.
  2. the equilibrium concentration of HA is smaller than the undissociated concentration.
24
Q

How can Ka be calculate used equilibrium concentrations

A

[H+]eqm[A-]eqm/[HA]eqm or [H+]2/[HA]

25
Q

How to solve pH of a weak acid using Ka

A

[H+] = square root of (Ka x [HA])

26
Q

What can the ka of a weak acid be determined by

A

preparing a standard solution of a weak acid of a known concentration. Measuring the pH of the standard solution using a pH meter.

27
Q

What approximations are made involving weak acids

A
  1. Assumes that the dissociation of water is negligible.

2. The concentration of acid is much greater than the H+ concentration at equilibrium.

28
Q

What is kw

A

the ionic product of water

29
Q

What is the kw formula

A

[H+][OH-] = 1x10-14

30
Q

What is the importance of kw

A

controls the concentrations of H+ and OH- in aqueous solutions

31
Q

How do you calculate H+ and OH- concentrations in aqueous solution when given pH

A
  1. 10^-pH = [H+]

2. Kw/[H+] = [OH-]

32
Q

What is a strong base

A

an alkali that completely dissociates in solution

33
Q

What is a monoacidic base

A

each mole of a base releases one mole of OH-(aq) ions e.g.NaOH

34
Q

How do you calculate the pH of a solution of a strong base

A
  1. concentration of base = [OH-]
  2. kw/[OH-] = [H+]
  3. -log[H+] = pH
35
Q

What is a weak base

A

partially dissociates in solution so one mole of a base releases far less than one mole of [OH-]. e.g.NH3

36
Q

How do you find pka form a titration curve

A

Find volume needed to reach the end point (steep part of the curve). Divide the volume by 2 and use your graph to find the pH. pka=pH

Chemistry (24 decks)

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