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Chemistry Y11 > Acids, Bases And Salts > Flashcards

Acids, Bases And Salts Flashcards

1
Q

Define indicator

A

A dye that changes colour according to whether it is an acidic or alkaline solution

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2
Q

Define a strong acid

A

Turns universal indicator red and has a pH of 1-2, ionises completely in water

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3
Q

Define weak acid

A

Turns orange - yellow in universal indicator. Has a pH of 3-6 and ionises partially in water

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4
Q

Define base

A

A compound that will react with an acid producing salt and water

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5
Q

Define alkali

A

A soluble base

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6
Q

What makes an acid strong or weak?

A

A strong acid dissociates all of its hydrogen atoms when dissolved in water, whereas a weak acid only partially dissociates its hydrogen atoms

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7
Q

Write out the Ionic equation for the neutralisation reaction

A

H+(aq) + OH- (aq) —> H2O (l)

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8
Q

Name the piece of apparatus used to add hydrochloric acid to the comical flask

A

Burette

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9
Q

Explain how a result with universal indicator paper may be converted to a pH value

A

Red on the universal indicator indicates a strong acid

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10
Q

Name three everyday examples of acids

A

Lemon, vinegar and battery acid

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11
Q

What do acids do when dissolved in water?

A

Release H+ ions/hydrogen ions/protons on dissolving in water

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12
Q

List two properties of acids

A

Sour taste

Corrosive

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13
Q

What do alkalis do when dissolved in water?

A

Alkalis release OH- ions (hydroxide ions) when dissolved in water

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14
Q

List two properties of bases

A

Soapy feel

Corrosive

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15
Q

Name three everyday examples of a base

A

Oven cleaner, ammonia, soap powder

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16
Q

What hazard symbols look like:

  • skull and crossbones?
  • gas cylinder?
  • test tubes drilling into hand and bench?
A
  • acutely toxic
  • gas under pressure
  • corrosive
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17
Q

Describe the colour changes in phenolphthalein when exposed to;

  • acid
  • alkali
  • neutral
A
  • colourless
  • pink
  • colourless
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18
Q

Describe the colour change in methyl orange in;

  • acid
  • alkali
  • neutral
A
  • red
  • yellow
  • orange
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19
Q

Define neutralisation

A

The reaction between the hydrogen ions in an acid and the hydroxide ions in an alkali to produce water

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20
Q

Name the salt and ion which hydrochloric acid forms

A

Chlorides

Cl- ions

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21
Q

Name the salt and ion which sulfuric acid forms

A

Sulfates

SO4(2-) ions

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22
Q

Name the salt and ion which nitric acid forms

A

Nitrates

NO3(-) ions

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23
Q

Name the salt and ion which ethanoic acid produces

A

Ethanoates

CH3COO- ions

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24
Q

Metal oxides are … and non mental oxides are ..

A

Basic

Acidic

25
Q

Name three observations for reactions with acids

A

Heat is released
Bubbles of gas produced
Solid disappears and a solution is produced

26
Q 
Copper (ii) oxide - 
Copper (ii) carbonate - 
Hydrated copper (ii) Sulfate - 
Copper (ii) salts in solution - 
Group 1, Group 2, Aluminium and zinc compounds -
A 
Black oxide 
Green solid 
Blue crystals 
Blue solution 
White solids and if they dissolve in water they give colourless solutions
27
Q

Name three methods of drying salt crystals

A
  • place in a dessicator
  • place in a low temperature oven
  • dry between two sheets of filter paper
28
Q

Colour of solution after reaction between magnesium and sulfuric acid

A

Colourless

29
Q

Was a gas given off after the reaction between magnesium and sulfuric acid

A

Yes, hydrogen

30
Q

Colour of solution after the reaction between copper oxide and sulfuric acid

31
Q

Was a gas given off after the reaction between copper oxide and sulfuric acid

32
Q

Colour of solution after the reaction between copper carbonate and sulfuric acid

33
Q

Was a gas given off after the reaction between copper carbonate and sulfuric acid

A

Yes, carbon dioxide

34
Q

Explain why a salt is added until it is in excess

A

To ensure that all the acids are reactive

35
Q

State one way that you would know that a salt is in excess

A

Solid is at the bottom of the beaker or no more gas given off

36
Q

Why is the solution not evaporated to dryness

A

If evaporated to dryness the water of crystallisation would be driven out of the crystals

37
Q

Why do crystals form as the solution is cooled

A

As solution is cooled, solubility decreased and crystals will form

38
Q

What does a high concentration of hydrogen ions in an acidic solution indicate?

A

A lower pH

39
Q

Give an example of a weak acid

A

Ethanoic acid

40
Q

Give an example of a weak alkaline

41
Q

Define concentrated acid

A

Contains a larger number of acid particles dissolved per unit volume

42
Q

Define dilute acid

A

Contains a small number of acid particles dissolved per unit volume

43
Q

Define salt

A

A compound formed when some of all of the hydrogen ions in an acid are replaced by metal ions or ammonium ions

44
Q

What is the use of charcoal in an experiment?

A

To remove the indicator

45
Q

List three possible observations for reactions with acids

A
  • bubbles of gas produced
  • solid disappears and a solution is produced
  • heat is released
46
Q

In the reaction between magnesium and sulfuric acid, what is the colour of the solution after reaction?

A

Colourless

47
Q

In the reaction between magnesium and sulfuric acid was a gas given off?

A

Yes, hydrogen

48
Q

In the reaction between copper oxide and sulfuric acid, what was the colour of solution after reaction?

49
Q

In the reaction between copper oxide and sulfuric acid was a gas given off ?

50
Q

In the reaction between copper carbonate and sulfuric acid what was the colour after reaction?

51
Q

In the reaction between copper carbonate and sulfuric acid was a gas given off?

A

Yes carbon dioxide

52
Q

Flame colours of lithium, sodium, potassium, calcium and copper

A
  • lithium (crimson);
  • sodium (yellow/orange);
  • potassium (lilac);
  • calcium (brick red); and
  • copper(II) (blue–green/green
53
Q

Describe paper chromatography

A

The separation of mixtures of soluble substances by running a solvent (mobile phase) through the mixture on the paper (stationary phase), which causes the substances to move at different rates over the paper;

54
Q

How to make water potable ?

A
  • filtration
  • sedimentation
  • chlorination;
55
Q

How can seawater be made potable ?

A

using distillation

56
Q

How to test for water ?

A

use anhydrous copper(II) sulfate to test for water.

57
Q

How to carry out titration and what is it used for

A
  • Used for making all sodium and potassium salts - the alkali used is either sodium hydroxide solution or potassium hydroxide solution
  • Titration is carried out using a Pipette to measure the exact volume of one solution. The other solution is added from a burette
  • Pipette 25cm3 of the alkali into a conical flask and add a few drops of phenolphthalein indicator which gives a pink colour
  • Fill The burette to the mark with the acid and run it into the conical flask until the colour changes to colourless
  • record the volume of acid used
  • Repeat without the indicator using the same volumes to get a solution which only contains salt
  • Or Add charcoal, heat it and filter the solution to absorb the indicator
  • Heat the solution to evaporate water from it
  • Reduce The volume by half and leave it to cool and crystallise
  • Then Filter off the crystals and dry them between two sheets of filter paper
58
Q

How to use an insoluble solid

A
  • This method uses an insoluble solid (base or carbonate) containing the metal ion
  • Using a metal carbonate has an advantage because when it reacts it produces a gas (CO2) so when all the acid has been neutralised no more gas will be produced
  • Add excess of the insoluble solid to 25cm3 of acid in a conical flask
  • Heat and stir and make sure that there is some unreacted solid left
  • Then filter off the insoluble solid (residue) and pour the filtered liquid (filtrate) into an evaporating basin
  • Heat to evaporate water from it - reduce the volume by half and leave it to cool and crystallise
  • Then filter off the crystals and dry them between two sheets of filter paper

Chemistry Y11 (9 decks)

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