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Chemistry > Acids and bases > Flashcards

Acids and bases Flashcards

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1
Q

States the acid, bases, and there conjugates of this equation.
HCl + H2O <=> H3O+ + Cl-

A

HCl(acid) + H2O(base) <=> H3O+(acid) + Cl-(Base)

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2
Q

State the meaning for pH.

A

-log10[H+]

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3
Q

State the definition of a Strong Acid.

A

A Strong Acid completely dissociates into ions in an aqueous solution.

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4
Q

State the definition of a Weak Acid.

A

A Weak Acid partially dissociates into ions in an aqueous solution and is in equilibrium.

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5
Q

State the definition of a Strong Base.

A

A Strong Bases completely dissociate into ions in an aqueous solution.

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6
Q

State the definition of a Weak Base.

A

weak bases partially dissociation react with water to give ions in an aqueous solution.

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7
Q

State the equation for the relative strength of dissociation of a weak acid.

A 
Ka = ([H+][A-]) / ([HA])
pKa = -log10Ka
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8
Q

State the equilibrium which defines the dissociation of a weak acid.

A

[HA] <=> [H+] + [A-]

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9
Q

State the definition of Kb

A

The relative strength of dissociation of a base.

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10
Q

State the equilibrium which defines the dissociation of a weak base.

A

[Base] + [H+] <=> [HB+]

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11
Q

State the definition of the dissociation of water.

A

H2O <=> H+ + OH-

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12
Q

State the Ionic product of water.

A

Kw = [H+][OH] at 27oC Kw=10^-14

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13
Q

State one assumption made with Kw.

A

The concentration of H2O is so large compared to the concentration of [H+] or [OH-] it is regarded as constant combined with kc to make Kw.

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14
Q

What are the units for Kw.

A

mol2dm-6

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15
Q

State the definition of a neutral solution.

A

a solution consisting of equal concentrations of H+ and OH- ions.

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16
Q

What are the Bronsted Lowery definitions of an acid and a base?

A

An Acid is a proton donor and a Base is a proton acceptor

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17
Q

What is the conjugate acid of NH3?

A

NH4+

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18
Q

What is the conjugate base of CH3COOH?

A

CH3COO-

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19
Q

What is the conjugate acid of HNO3?

A

H2NO3+

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20
Q

Names the Acid Base conjugate pairs in this reaction H3O+ + HSO4- → H2SO4 + H2O

A

H3O+ Acid H2O Base. HSO4- Base H2SO4 acid.

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21
Q

Give the formula of Hydroxonium Ion

A

H3O+

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22
Q

Describe the bonding in the Hydroxonium Ion

A

Covalent and Dative Covalent Bonding

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23
Q

Define a strong acid

A

An acid that completely dissociates in aqueous solution

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24
Q

Define a weak acid

A

An acid that partially dissociates in aqueous solution.

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25
Q

What is the pH of a solution with a [H+] of 1.23x10-4 mol dm-3

A

3.91

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26
Q

What is the pH of a solution with a [H+] of 7.89 x10-15 mol dm-3

A

14.1

27
Q

Rearrange the definition of pH to make [H+(aq)] the subject

A

[H+(aq) = 10-pH

28
Q

What is the [H+(aq)] of a solution with a pH of 9.2?

A

6.31x10-10 moldm-3

29
Q

Calculate the pH of the solution formed by adding of 250 cm3 of water to 50 cm3 of 0.200 mol dm-3 HNO3

A

1.48

30
Q

Calculate the pH of the following solution 100 g dm-3 H2SO4

A

-0.31

31
Q

What is the formula of the ionic prodcut of water Kw

A

Kw = [H+][OH-]

32
Q

What is the relationship between pH and pOH?

A

pH + pOH = 14

33
Q

Calculate the pH of the following solution: 0.20 mol dm-3 Ba(OH)2

A

13.6

34
Q

Calculate the pH of the solution formed by the addition of 100 cm3 of water to 25 cm3 of 0.100 mol dm-3 NaOH

A

12.3

35
Q

Write a general equation for the dissociation of a weak acid

A

“HA(aq) → A¯(aq) + H+(aq)

“

36
Q

What are the two assumptions one makes when calculating the pH of a weak acid?

A

“The amount of HA at equilibrium is equal to the amount of HA put into the solution and [H+(aq)]= [A¯(aq)]
“

37
Q

What does the general formula for the acid dissociation constant become when these two assumptions are applied?

A

“Ka = [H+(aq)]2/[HA(aq)]

“

38
Q

Write the fomula you use to calculate the pH of a weak acid.

A

[H+(aq)] = √ [HA(aq)] Ka

39
Q

Calculate the pH of the following weak acid: 0.200 mol dm-3 butanoic acid (Ka = 1.51 x 10-5 mol dm-3)

A

2.76

40
Q

Calculate the Ka value for phenylethanoic acid given that a 0.100 mol dm-3 solution has a pH of 2.66

A

4.79 x 10-5 mol dm-3

41
Q

Write the seven steps for the calculation of the pH of a solution formed by the reactions between a weak acid and a strong base if the acid is in excess.

A

Calculate moles HA (it is still HA and not H+ as it is a weak acid), Calculate moles OH, Calculate moles XS HA, Calculate moles HA left and A- formed, Calculate [HA] leftover and [A-] formed, Use Ka to find [H+], Find pH

42
Q

Write the six steps for the calculation of the pH of a solution formed by the reactions between a weak acid and a strong base if the OH- is in excess.

A

Calculate moles HA (it is still HA and not H+ as it is a weak acid), Calculate moles OH, Calculate moles XS OH, Calculate [OH-], Use Kw to find [H+], Find pH

43
Q

Calculate the pH of the solution formed when 50 cm3 of 0.500 mol dm-3 ethanoic acid (pKa = 4.76) is added to 50 cm3 of 0.250 mol dm-3 KOH

A

4.76

44
Q

What is a titration?

A

” a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete.
“

45
Q

What is the equivalence point of a titration?

A

“the point at which the titration reaction is complete

“

46
Q

Define what types of substances are suitable to be indicators

A

They are weak acids whose conjugate base is a different colour to the acid.

47
Q

How do you select a suitable indicator for a particular type of titration.

A

The pH range of the suitable indicator fits within the vertical section of the titration curve.

48
Q

“Methyl Orange has a pH range of 3.1-4.4 for what types of titration Is it suitable?
“

A

Strong acid, Strong base. Strong acid, Weak Base

49
Q

“Phenolpthalein has a pH range of 8.3-10.0 for what types of titration Is it suitable?
“

A

Strong acid, Strong base. Weak acid, Strong Base

50
Q

What is the typical equivalence point of a strong acid strong base titration?

A

7

51
Q

What is the typical equivalence point of a strong acid weak base titration?

A

5

52
Q

What is the typical equivalence point of a weak acid strong base titration?

A

9

53
Q

What is the typical pH range of the vertical section of a strong acid strong base titration curve?

A

3 to 10

54
Q

What is the typical pH range of the vertical section of a weak acid strong base titration curve?

A

7 to 11

55
Q

What is the typical pH range of the vertical section of a strong acid weak base titration curve?

A

3 to 7

56
Q

Explain how one can use a titration curve to calculate Ka of a weak acid.

A

“Half way to the equivalence point [HA(aq)] = [A¯ (aq) ], so pKa = pH

”

57
Q

Define what is a buffer solution

A

“Solutions which resist changes in pH when small quantities of acid or alkali are added.
“

58
Q

Describe the most common way of making a buffer solution.

A

“A buffer solution is made from a weak acid and the salt of the weak acid.
“

59
Q

Describe an additional way of making a buffer solution

A

“Adding a measured amount of hydroxide ions to a weak acid

“

60
Q

What are the two assumption we make when calculate the pH of a buffer solution.

A

“All the A- ions come from the salt, Almost all the HA molecules put into the buffer remain unchanged

”

61
Q

What does the general formula for the acid dissociation constant become when the assumptions for a buffer solution are applied?

A

” Ka = [H+(aq)] x [salt]/ [acid]

“

62
Q

“What happens if an acidic substance is added to a buffer?

“

A

“Any rise in [H+(aq)] disturbs the equilibrium. Some A-(aq) ions from the salt react with the extra H+(aq) ions to form HA(aq) and water. A significant fall in pH is prevented.
“

63
Q

Calculate the pH of the following buffer solutions made by mixing 50.0 cm3 of 1.00 mol dm-3 methanoic acid (Ka = 1.78 x 10-4 mol dm-3 with 20.0 cm3 of 1.00 mol dm-3 sodium methanoate

A

3.35

64
Q

“Calculate the pH of the following buffer solution made by mixing 100 cm3 of 1.00 mol dm-3 ethanoic acid (Ka = 1.78 x 10-4 mol dm-3 ) is mixed with 50.0 cm3
of 0.8000 mol dm-3 sodium hydroxide.”

A

3.57

Chemistry (21 decks)

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