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Acids And Bases Flashcards

1
Q

Proton transfer

A

Nucleus of a h atom is transferred from acid to base

Electron stays behind on the acud.

Molecule hence has a negative ion form

Proton tramsfers to base

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2
Q

Common strong acids
Name and write the formula of common strong acids

A

Sulphuric acid. H2SO4
O
||
HO—S==O
|
OH
Hydro chloric acid HCl
*H—Cl

Nitric acid HN03
O
||
HO—N==O

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3
Q

Common weak acids

A

Sulphurous acid (greenhouse gas, sulphur dioxide, acid rain) H2SO3
O
||
HO——S——OH
Phosphoric acid H3PO for (Tangy taste of Coke)
O
||
HO——P——OH
|
OH
Carbonic acid H2CO3 ( fizz of sodas)
O
||
HO——-C———OH

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4
Q

Monoprotic acids
Examples and definition

A

HCl and HC3COOH
Acids which can donate one proton per acid molecule



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5
Q

Diprotic acids
Examples and definition

A

Acids which can donate two protons per acid molecule
H2SO4 (COOH)2

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6
Q

Polyprotic acids

A

Acids which can donate more than one proton per acid molecule
H2 SO4
H 3PO4
(Cooh)2

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7
Q

Ionisation

A

The reaction of a molecular substance with water to produce irons

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8
Q

Ionisation of HCl

A

HCl+H2O—> H30+ + Cl-

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9
Q

Ionisation of strong acids and water
Which type of arrow?

A

Single arrow

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10
Q

Ionisation of sulphuric acid

A

Strong acids
H2SO4 +2H2O->SO42- + 2H30+

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11
Q

Ionisation of HCl

A

Hcl + H2O->Cl- +H3O+
Strong acids

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12
Q

Ionisation of nitric acid

A

Strong acid
HNO3 + H20 —> HNO3- + H3O+

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13
Q

Ionisation of weak acids in water
What type of arrow?

A

Reversible arrow

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14
Q

Ionisation of HF

A
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15
Q

Ionisation of H2SO3

A
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16
Q

Ionisation of H3PO4

A
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17
Q

Ionisation of CH3COOH

A
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18
Q

Strong acid
Definition

A

An acid that ionises completely in an aqueous solution

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19
Q

Definition of weak acid

A

An acid that only ionises partially in an aqueous solution

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20
Q

KA

A

KA= p\r
KA expression equals compounds
Strong Ka greater than one
Weak Ka less than one

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21
Q

Conductivity of an acid solution

A

A solution of a stronger as it will be a better conductor as it will contain more irons

A stronger acid when mixed with water but ionise completely therefore producing huge amounts of irons

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22
Q

Strength of an acid versus concentration

A

The strength of the acid is determined by the identity of the acid, and to what extent it ionise in the solution

The concentration of an acid is determined by how the solution is prepared (how many moles of acid are added to each DM3 of solvent)

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23
Q

Ionic strong bases

A

NAOH
KOH
LIOH
Na2O Forms a strong base in the water

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24
Q

Weak covalent acid

A

NH3

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25
Q

Why are group 1 hydroxides strong ionic bases

A

One: dissociation: oxygen is the proton exceptor
To: Ionisation:Oxide ions undergo hydrolysis and 0H ions are produced from water

This forms a strong base in a xOH

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26
Q

Disassociation

A

The splitting of anionic compound into its irons

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27
Q

Disassociation of KOH
Evidence of being a base

A

Strong base
H20
KOH(s)—-> K+(aq) + OH-(aq)
Produces OH in aqueous solution as OH is the proton exceptor

28
Q

Dissociation of MG (OH) 2

A

Mg(OH)2(s)🔄Mg2+(aq)+2OH-(aq)

29
Q

A weak base

A

A bass that only dissociates/I am noises particularly in an aqueous solution

30
Q

Why are carbonates week

A

1: dissociation: carbonate of the proton exceptor
2: carbonate iron undergoes hydrolysis and produces OH from water

31
Q

KB value

A

Strong bases: value very high
Weak bases: KB is very small
Given from an ionisation reaction

Ionic bases do not undergo ionisation, only dissociation and hydrolysis. We do not write KB expressions for these bases. We only write a KB expression for ammonia

32
Q

Ionisation of ammonia

A

NH3 + H2O🔁NH4+ +OH-

33
Q

Strong base versus concentrated bass

A

The strength of the base is determined by the identity of the base, and to what extent it dissociates in solution

The concentration of a base solution is determined by how the solution is prepared (how many moles of base are added to each Diem three of solvent)

34
Q

Acid-base conjugates

A

The conjugate acid of a weak base is Strong
The conjugate acid of a strong base is weak

35
Q

Amphoteric

A

A substance that can either act as an acid or base

36
Q

Equations to show how an amphoteric substance can act as an acid or base

A

H2C03 + H2 0🔁 HCO3 - +H30
Or HCO3- + H2O🔁H2CO3 + OH-

37
Q

Auto ionisation of water

A

Because water is M3 project, and acid-base reaction can occur between two water molecules. This auto ionisation reaction occurs to a small extent

H2O + H2O🔄OH-+H3O+
The concentration of 0H equals the concentration of H30

38
Q

Auto ionisation equilibrium constant

A

KW equals [H30 ] [OH]
The value of the equilibrium constant does not change equals 10^-14 & 25°C


39
Q

the pH scale 

A

The measure of hydronium iron concentration in water at 25°C

40
Q

PH

A

Minus log [HPlus ]

41
Q

Explain qualitatively the pH range of 0 to 14

A

PH5 to 7: dilute Weak acids – acid that ionises partially
PH5-3: strong die loot acid/concentrated weak acids
PH2-0: concentrated strong acids
PH 14 to 12 concentrated strong bases
PH 12 to 10: concentrated weak bases/dilute strong bases
PH9 to 7: dilute weak bases

42
Q

Standard acid-base reactions:
Acid plus metal

A

Salt plus hydrogen (redox)

43
Q

Standard acid-base reactions:
Acid plus metal oxide

A

Salt plus water

44
Q

Standard acid-base reactions:
Acid plus metal hydroxide

A

Salt plus water

45
Q

Standard acid-base reactions:
Acid plus metal carbonate

A

Salt plus water plus carbon dioxide

46
Q

Standard as a base reactions
acid plus metal hydrocarbonate

A

Salt plus water plus carbon dioxide

47
Q

Salt

A

A substance in which the hydrogen Of an acid has been replaced by a Cation 

48
Q

Identify the acid and base that could react to Produce a given salt

A

NA2SO4: NA2 is from the base NAOH
SO4 is from the acid H2 SO4

Kate to see 03:K2 is from the base KOH
CO3 is from the acid H203

NH4CL: in age 4 is from the base NH40H
CL is From the acid HCl

49
Q

Hydrolysis of a salt

A

A reaction of an iron (from a salt) with water

50
Q

Hydrolysis of HSO3

A

HSO-3 + H2O —> H2SO3 +OH-
This reveals that HSO3 is a base

51
Q

Hydrolysis of NH4

A

NH4+ + H2O —> NH3 + H3O+

52
Q

Hydrolysis of F

A

F- + H20 —> HF + OH-

53
Q

Which irons can go under hydrolysis/react with water

A

Conjugate irons of strong acids and bases do not undergo hydrolysis

Irons from weak acids or bases will react with water

54
Q

Predict the approximate pH of the salts
Steps

A
  1. identify iron that will go under hydrolysis
  2. write hydrolysis reaction (reaction of iron with water)
  3. conclude what the pH of the solution will be
55
Q

What is the pH of NACL

A

One: the Cation that will go under hydrolysis is NH4 plus
To: the equation for this reaction: in the age 4+ plus water reversible arrow and age 3+ H30+
Hence predict the approximate PH: slightly acidic

56
Q

Determine approximate pH of CH3COONA

A

One: the anion that will go under hydrolysis is CH3COO minus
To: the equation for this reaction is: CH3COO minus plus water reversible arrow CH3COOH plus 0H -
Three: helps predict the approximate PH: slightly basic

57
Q

Why do we do titrations

A

Titrations are performed to accurately determine the concentration of a particular acid or base solution

58
Q

What is a titration

A

A titration is an experimental process used to accurately determine the concentration of an acid or base solution

59
Q

Neutralisation/equivalence point

A

The point where an acid and base have reacted so neither is an access

Add the equivalence point no reactants are left, only salt and water are present

60
Q

Standard solution

A

A solution of known concentration

61
Q

Describe quantitatively and qualitatively how to make up a standard solution

A

Qualitatively:
One: mass the required quantity of the salt using an accurate mass balance
To: dissolve the salt in a little water and place the solution in the volumetric flask
Three: fill the volumetric flask to the mark carefully with water

Since you know the mass accurately can determine the number of moles accurately
Hence determine volume then concentration (present formulas)


62
Q

Explain titration method

A

1: a burette is filled with a standard solution of known concentration

2: a burette is filled with the solution of unknown concentration.

3: a fixed volume of the solution of Unknown concentration is emptied into a clean conical flask.

4: a few drops of a suitable indicator or added to the solution in the conical flask

5: the conical flask is placed on a white tile To easily see the colour change

6: run a small quantity of the solution out of the be ready and record various readings

7: record the final be ready reading. Determine the volume of the solution added by subtracting the initial be reading from the final be a reading as the first reading is a rough measurement.

8: repeat three times to find average volume of standard solution that is needed to achieve colour change.

9: use the balanced equation for the reaction, The measured volumes as well as the known concentration to calculate the unknown concentration

63
Q

Describe and explain the physical process of performing a titration to ensure appropriate precision

A

Make sure to wash the conical flask with water
Wash the pipets with solution
Select the correct indicator
Prepare a standard solution

64
Q

Are indicators acids or bases and how do you know

A

Indicators are weak acidsIn equilibrium with their can’t you get bases. The acid and conjugate base are different colours in solution

65
Q

Selecting the correct indicator

A

Strong acid versus strong base: equivalence point is at PH7

Weak acid versus strong base equivalence point is the pH is greater than seven

Strong acid versus weak base the equivalence point pH is lower than seven

Physics (14 decks)

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