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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
Why are group 1 hydroxides strong ionic bases
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
26
Disassociation
The splitting of anionic compound into its irons
27
Disassociation of KOH Evidence of being a base
Strong base H20 KOH(s)—-> K+(aq) + OH-(aq) Produces OH in aqueous solution as OH is the proton exceptor
28
Dissociation of MG (OH) 2
Mg(OH)2(s)🔄Mg2+(aq)+2OH-(aq)
29
A weak base
A bass that only dissociates/I am noises particularly in an aqueous solution
30
Why are carbonates week
1: dissociation: carbonate of the proton exceptor 2: carbonate iron undergoes hydrolysis and produces OH from water
31
KB value
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
Ionisation of ammonia
NH3 + H2O🔁NH4+ +OH-
33
Strong base versus concentrated bass
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
Acid-base conjugates
The conjugate acid of a weak base is Strong The conjugate acid of a strong base is weak
35
Amphoteric
A substance that can either act as an acid or base
36
Equations to show how an amphoteric substance can act as an acid or base
H2C03 + H2 0🔁 HCO3 - +H30 Or HCO3- + H2O🔁H2CO3 + OH-
37
Auto ionisation of water
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
Auto ionisation equilibrium constant
KW equals [H30 ] [OH] The value of the equilibrium constant does not change equals 10^-14 & 25°C 
39
the pH scale 
The measure of hydronium iron concentration in water at 25°C
40
PH
Minus log [HPlus ]
41
Explain qualitatively the pH range of 0 to 14
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
Standard acid-base reactions: Acid plus metal
Salt plus hydrogen (redox)
43
Standard acid-base reactions: Acid plus metal oxide
Salt plus water
44
Standard acid-base reactions: Acid plus metal hydroxide
Salt plus water
45
Standard acid-base reactions: Acid plus metal carbonate
Salt plus water plus carbon dioxide
46
Standard as a base reactions acid plus metal hydrocarbonate
Salt plus water plus carbon dioxide
47
Salt
A substance in which the hydrogen Of an acid has been replaced by a Cation 
48
Identify the acid and base that could react to Produce a given salt
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
Hydrolysis of a salt
A reaction of an iron (from a salt) with water
50
Hydrolysis of HSO3
HSO-3 + H2O —> H2SO3 +OH- This reveals that HSO3 is a base
51
Hydrolysis of NH4
NH4+ + H2O —> NH3 + H3O+
52
Hydrolysis of F
F- + H20 —> HF + OH-
53
Which irons can go under hydrolysis/react with water
Conjugate irons of strong acids and bases do not undergo hydrolysis Irons from weak acids or bases will react with water
54
Predict the approximate pH of the salts Steps
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
What is the pH of NACL
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
Determine approximate pH of CH3COONA
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
Why do we do titrations
Titrations are performed to accurately determine the concentration of a particular acid or base solution
58
What is a titration
A titration is an experimental process used to accurately determine the concentration of an acid or base solution
59
Neutralisation/equivalence point
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
Standard solution
A solution of known concentration
61
Describe quantitatively and qualitatively how to make up a standard solution
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
Explain titration method
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
Describe and explain the physical process of performing a titration to ensure appropriate precision
Make sure to wash the conical flask with water Wash the pipets with solution Select the correct indicator Prepare a standard solution
64
Are indicators acids or bases and how do you know
Indicators are weak acidsIn equilibrium with their can’t you get bases. The acid and conjugate base are different colours in solution
65
Selecting the correct indicator
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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