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Alevel CHEM > Acids And Bases > Flashcards

Acids And Bases Flashcards

1
Q

What is hydrochloride acid

A

Hcl

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2
Q

Sulphuric avid

A

H2 so4

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3
Q

Nitric avid

A

HNO3

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4
Q

Ethanoic acid

A

Ch3cooh

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5
Q

What do acids do when dissolved in water ?

A

Dissociate to release hydrogen ions

Proton donors

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6
Q

What is dissociation

A

Process of giving up a proton

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7
Q

Strong acids

A

Release all their atoms ( hydrogen ) into a solution as H+ ions

Completely dissociate

Have a low pH

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8
Q

Example of strong acids

A

Hcl

H2 so 4

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9
Q

Weak acids

A

Only release a proportion of its available hygogrn atom is to solution

Reversible

Lower concentration of h + ions in solution

Partially dissociate

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10
Q

What is an alkali

A

A base that dissolved in water release ing hydroxide ions

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11
Q

What are alkalis

A

Proton acceptors

Neutralise acids

Strength depends on its solubility

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12
Q

Bases

A

Metal carbonates
Metal oxides

Metal hydroxides

Ammonia

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13
Q

Strong bases

A

Almost all of the base dissociates in water to produce oh

Forward reaction favoured

Eg NaOH

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14
Q

Weak bases

A

Ionise only slightly in water

Backwards reaction favoured - small amount dissociates

Few OH- released

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15
Q

Neutralisation

A

H+ ions react with a vase to forma salt and neutral water

The h+ionsfrom the acid are replaced by metal or ammonium ions from the base

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16
Q

Acid + base =

A

Salt and water

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17
Q

Acid + metal oxide/ hydroxide

A

Salt and water

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18
Q

Acid and carbonate =

A

Salt and water and co2

19
Q

Ammonia

A

Doesn’t produce hydroxide ions, but aqueous ammonia is an alkali

This is because the reaction between ammonia and water produce hydroxide ions

Ammonia accepts a hydrogen ions from h20 molecule - forming an ammonium ion and hydroxide ion

Nh3+ h20 = nh4+ + oh-

20
Q

Sulphuric avid

A

Strong avid

When mixed with water each h2so4 molecule dissociates releasing 1 of its 2 hydrogen atoms as a h+ ion

21
Q

What is a titration

A

Measure he volume of one solution that reacts exactly with another solution

22
Q

What can triteations be used for

A

Finding conc of solution

Identification of unknown chemicals

Finding the purity of a substance

23
Q

standard solution ?

A

Known concentration
Volumetric flask

  1. Weigh solid
  2. Dissolve solid using distilled water
  3. Transfer to volumetric flask
  4. Rinse last traces
  5. filled to graduation line
  6. Invert
24
Q

The titration

A

Add 2nd solutions to burette
Record initial burette Reading
Drop one solution into the toher - use white tile

End Point

Repeats - so 2 concordant results are obtained ( within 0.1)

MEAN TITRE

25
Q

Indicators - methyl orange

A

Yellow - orange < acid to alkali

26
Q

Phenophthalein

A

Pink to colourless ( acid to alkali)

27
Q

Systematic error

A

Constant error due to equipment

Eg balance

28
Q

Random error

A

May not always occur eg air bubble in burette

29
Q

Margin of error of equipment

A

Limits of precision of equipment used to take measurements

Eg pippette

30
Q

Percentage error of equipment

A

Max margin of error / measured value

  • 100
31
Q

Titration calculation

A

Concentration = amount/ volume

C1v1= c2v2

32
Q

What is oxidation number

A

Inform u about he number of electrons used when an atom binds with another element

33
Q

Positive oxidation number

A

Electrons lost

34
Q

Negative oxidation number

A

Electrons gained

35
Q

Name of FeCl3

A

Iron (111) chloride

36
Q

Rules for oxidation numbers

A

All I combined elements have an oxidation number of 0 and sum of oxidation number in a compound is 0

Sum of all oxidation numbers in an ion equals the charge on that ion

Group 1,2,3= 1+, 2+, 3+

Fluorine - oxidation number -1

Hydrogen +1 , metal hydride = -1

Oxygen - -2

Compound with fluorine, peroxide and superoxide - e.g. h202 =-1

37
Q

Fluorine oxidation number

38
Q

Roman numerals

A

Used in the names of compounds of elements that form ions with different charges

Shoes oxidation state of elementary without a sign

Iron (2)= Fe2+

39
Q

What is a redox reactions

A

Electron transmitted

40
Q

What is oxidation

A

Loss of electrons , increase in oxidation number = more positive

Metals commonly lose electrons to form positive ions

41
Q

Reduction

A

Gain in electron
Decrease in oxidation number

Non medals - gain electrons to form negative ions

42
Q

Oxidising agent

A

Receive / take in electrons

Are themselves reduced

E.g. oxygen

43
Q

Reducing agent

A

Donate electrons to
Other species

Are themselves oxidised

44
Q

What is disproportion

A

Species reduced and oxidised

Alevel CHEM (13 decks)

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