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Chemistry Y11 > Acids, Bases And Salts > Flashcards

Acids, Bases And Salts Flashcards

(58 cards)

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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 ..

25
Name three observations for reactions with acids
Heat is released Bubbles of gas produced Solid disappears and a solution is produced
26
``` Copper (ii) oxide - Copper (ii) carbonate - Hydrated copper (ii) Sulfate - Copper (ii) salts in solution - Group 1, Group 2, Aluminium and zinc compounds - ```
``` Black oxide Green solid Blue crystals Blue solution White solids and if they dissolve in water they give colourless solutions ```
27
Name three methods of drying salt crystals
- place in a dessicator - place in a low temperature oven - dry between two sheets of filter paper
28
Colour of solution after reaction between magnesium and sulfuric acid
Colourless
29
Was a gas given off after the reaction between magnesium and sulfuric acid
Yes, hydrogen
30
Colour of solution after the reaction between copper oxide and sulfuric acid
Pale blue
31
Was a gas given off after the reaction between copper oxide and sulfuric acid
No
32
Colour of solution after the reaction between copper carbonate and sulfuric acid
Blue
33
Was a gas given off after the reaction between copper carbonate and sulfuric acid
Yes, carbon dioxide
34
Explain why a salt is added until it is in excess
To ensure that all the acids are reactive
35
State one way that you would know that a salt is in excess
Solid is at the bottom of the beaker or no more gas given off
36
Why is the solution not evaporated to dryness
If evaporated to dryness the water of crystallisation would be driven out of the crystals
37
Why do crystals form as the solution is cooled
As solution is cooled, solubility decreased and crystals will form
38
What does a high concentration of hydrogen ions in an acidic solution indicate?
A lower pH
39
Give an example of a weak acid
Ethanoic acid
40
Give an example of a weak alkaline
Ammonia
41
Define concentrated acid
Contains a larger number of acid particles dissolved per unit volume
42
Define dilute acid
Contains a small number of acid particles dissolved per unit volume
43
Define salt
A compound formed when some of all of the hydrogen ions in an acid are replaced by metal ions or ammonium ions
44
What is the use of charcoal in an experiment?
To remove the indicator
45
List three possible observations for reactions with acids
- bubbles of gas produced - solid disappears and a solution is produced - heat is released
46
In the reaction between magnesium and sulfuric acid, what is the colour of the solution after reaction?
Colourless
47
In the reaction between magnesium and sulfuric acid was a gas given off?
Yes, hydrogen
48
In the reaction between copper oxide and sulfuric acid, what was the colour of solution after reaction?
Pale blue
49
In the reaction between copper oxide and sulfuric acid was a gas given off ?
No
50
In the reaction between copper carbonate and sulfuric acid what was the colour after reaction?
Blue
51
In the reaction between copper carbonate and sulfuric acid was a gas given off?
Yes carbon dioxide
52
Flame colours of lithium, sodium, potassium, calcium and copper
* lithium (crimson); * sodium (yellow/orange); * potassium (lilac); * calcium (brick red); and * copper(II) (blue–green/green
53
Describe paper chromatography
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
How to make water potable ?
- filtration - sedimentation - chlorination;
55
How can seawater be made potable ?
using distillation
56
How to test for water ?
use anhydrous copper(II) sulfate to test for water.
57
How to carry out titration and what is it used for
- 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
How to use an insoluble solid
- 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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