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Chemistry > 2.1.4: Acids > Flashcards

2.1.4: Acids Flashcards

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1
Q

Define concentration

A

Moles per unit volume

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2
Q

Define acid

A

Species that is a proton donor

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3
Q

Define alkali

A

a soluble base that RELEASES OH- ions into aqueas solution

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4
Q

Give the formula of hydrochloric acid

A

HCl

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5
Q

Give the formula of sulfuric acid

A

H2SO4

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6
Q

Give the formula of nitric acid

A

HNO3

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7
Q

Give the formula of ethanoic acid

A

CH3COOH

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8
Q

Define base

A

Species that is a proton acceptor

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9
Q

What are features of a weak acid ?

A

Partially dissociate H+ ions ( could be due to the backward reaction being favoured so little H+ released)

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10
Q

Give an example of weak acids

A

Carboxylic acids

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11
Q

What are features of strong acids ?

A

Fully dissociate H+ ions ( could be due to forward reaction being favoured so lots of H+ produced)

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12
Q

Give 3 examples of strong acids

A
  • HCl
  • H2SO4
  • HNO3
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13
Q

What does an reversible reaction sign usually indicate about acids/bases ?

A

They are a weak base/ acid as reactants and products are in equilibrium

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14
Q

What do monobasic, dibasic and tribasic acids mean

A

Determines how many H+ ions there are so how many bases it will react with
HCl
H2SO4
H3PO4

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15
Q

Give features of a strong base

A

Full dissociation of OH- ions ( could be due to forward reaction being favoured so lots of OH- ions produced)

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16
Q

Give 2 examples of strong bases

A
  • NaOH
  • KOH
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17
Q

What are features of weak bases ?

A

Partial dissociation of OH- ions ( could be due to backwards reaction being favoured so little OH- ions produced)

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18
Q

Give an example of a weak base

A

NH3

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19
Q

Give the ionic equation for the dissociation of ammonia and water

A

NH3 + H20 (reversible) NH4+ + OH-

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20
Q

Give two general examples of common bases in reactions

A

Metal oxides and metal hydroxides

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21
Q

Give 2 examples of common alkalis

A

NaOH and KOH

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22
Q

What type of bond do bases commonly form ?

A

Dative covalent bond as they often have a lone pair of electrons when accepting H+ ions they can bond with

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23
Q

Give formula of the base magnesium hydroxide

A

MgO

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24
Q

Give formula of the base copper oxide

A

CuO

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25
Q

Give formula of the base sodium hydroxide

A

NaOH

26
Q

Give formula of the base magnesium hydroxide

A

Mg(OH)2

27
Q

Give formula of the base ammonia

A

NH3

28
Q

Give formula of the base methylamine

A

CH3NH2

29
Q

What are all amines examples of ?

A

Bases

30
Q

Define a salt

A

An ionic compound formed from an acid when a H+ ion is replaced by a metal or positive ion

31
Q

Turn sulfuric acid, H2SO4, into a sulfate salt with potassium

A

Replace H+ with metal, K2SO4

32
Q

Acid + carbonate =

A

Salt + CO2 + H20

33
Q

Acid + base =

A

Salt + water

34
Q

Acid + alkali =

A

Salt + water

35
Q

Acid + metal oxide =

A

Salt + H20

36
Q

Give equation for how water is formed through ions

A

H+ (aq) + OH- (aq) (reversible) H20 (l)

37
Q

What equipment do you use to measure volumes in acid-base titrations ?

A
  • Graduated pipette and burette
38
Q

Explain how to prepare a standard solution

A
  • Weigh precise amount of solid on 3.d.p balance
  • Add a small volume of water and dissolve
  • Transfer to volumetric flask whilst rinsing beaker to transfer washings to flask with distilled water
  • Make up to the mark with more water using a dropping pipette so the meniscus is on the mark
  • Secure stopper and invert several times to mix contents
39
Q

What can reduce impacts of measurement uncertainties during acid-base titrations ?

A
  • Use a balance which measures to 3 decimal places (smaller resolution with more precision)
  • Use a volumetric flask
  • Measure a larger quantity
40
Q

How do you work out % uncertainty ?

A

(uncertainty/ measured value) x 100

41
Q

Describe the steps to perform a titration

A
  • Measure a known volume of 25cm3 of alkali using a graduated pipette into a conical flask
  • Fill the burette to 0.00cm3 with acid
  • Add a few drops of indicator phenolpthalin to conical flask
  • Slowly add the acid to the alkali and the colour should go from pink to colourless
  • Repeat and record to 2.d.p until concordant results within 0.1 of eachother are obtained
42
Q

What are concordant results ?

A

Within 0.1 of eachother

43
Q

Define amphoteric

A

Substances that can behave as both acids and bases

44
Q

Give 2 examples of amphoteric compounds

A
  • Water
  • Amino acid if R group isn’t an acid or base
45
Q

Give formula of nitrile ion

A

NO2-

46
Q

Give formula of phosphate ion

A

PO43-

47
Q

Give formula of hydrogen carbonate ion

A

HC03-

48
Q

Give formula of sulphate ion

A

SO3 2-

49
Q

Give formula of dichromate ion

A

Cr2O7 2-

50
Q

Give formula of potassium hydroxide

A

KOH

51
Q

Give formula of sodium hydroxide

A

NaOH

52
Q

What do you use to calculate the mean titre for a titration?

A

Concordant values !

53
Q

What needs to be accounted for when doing burette uncertainty calculations for titrations ?

A

Burette is used twice so uncertainty of equipment on top of equation is x21

54
Q

What should be used instead of a beaker in titrations?

A

Volumetric flask

55
Q

Define standard solution

A

A solution of known concentration

56
Q

When making a standard solution what step ensures no solution remains in the beaker ?

A

Rinse out the beaker with distilled water and transfer to the volumetric flask before making up to 250cm3

57
Q

After one reading is taken during a titration what needs to happen next to ensure reliable results ?

A

Repeat titres taken until concordant results within 0.1cm3 of eachother are obtained and calculate mean titre from concordant results

58
Q

Give a reason for mass loss during a reaction

A

C02 produced as a gas

59
Q

Explain why rate of reaction decreases on a graph

A

Decreases as reactants are used up as there are less frequent collisions

60
Q

What products are formed when calcium nitrate is reacted with nitric acid ?

A

Calcium carbonate and carbon dioxide

Chemistry (33 decks)

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